Answer: The pH of the solution is 2.420
Explanation: pH = -Log [H+]
= - Log [ 3.8 x 10^-3]
= 3 - 0.579784
= 2.420
gas mixture with a total pressure of 765 mmHg contains each of the following gases at the indicated partial pressures: 131 mmHg CO2, 226 mmHg Ar, and 186 mmHg O2. The mixture also contains helium gas. what is the partial pressure of the helium gas
Answer:
322mmHg
Explanation:
To calculate the partial pressure of the helium gas, we use the Dalton’s law of partial pressure.
It states that for a mixture of gases which do not react, the total pressure is equal to the sum of the individual partial pressures.
This means that:
Total pressure = Partial pressure of CO2 + partial pressure of Ar + Partial pressure of O2 + Partial pressure of helium.
Hence, Partial pressure of the helium gas = 765-131-226-86 = 322 mmHg
2' A mixture containing 2.75 gof ammonium chloride (NH4cl) in 5.0 g of water was heated to dissolve the solid and then allowed to cool in air. At 6f"C, the first crystals appeared in solution. What is the solubility of ammonium chloride (in g of NH4CIper 100 gof water) at 61 'C
Answer:
55g NH₄Cl / 100g Water
Explanation:
Solubility of a substance define the amount of solute per solvent in a saturated solution. The solution can dissolve additional solute if heated.
In the problem, as the first crystal appears at 61°C the solubility in this temperature is the concentration of the solution, that is:
2,75g NH₄Cl / 5,0g water ₓ 100 = 55g NH₄Cl / 100g Water
I hope it helps!
The solubility of ammonium chloride at 61°C is 55 grams per 100 grams of water.
The solubility of ammonium chloride at 61°C is 2.75 grams per 5 grams of water, which can be expressed as a ratio to find the solubility per 100 grams of water.
To find the solubility per 100 grams of water, we can set up a proportion:
[tex]\[\frac{2.75 \text{ g NH}_4\text{Cl}}{5 \text{ g water}} = \frac{x \text{ g NH}_4\text{Cl}}{100 \text{ g water}}\][/tex]
Now, we solve for [tex]\(x\)[/tex]:
[tex]\[x = \frac{2.75 \text{ g NH}_4\text{Cl}}{5 \text{ g water}} \times 100 \text{ g water}\] \[x = \frac{2.75}{5} \times 100\] \[x = 0.55 \times 100\] \[x = 55\][/tex]
The answer is: 55.
The specific heat capacity of water is 4.18 J K⁻¹ g⁻¹. What is the enthalpy (heat) change when 10.00 g of water is heated from 285.0 to 300.0 K (Hint temperature change is the same in °C or Kelvin)?
Answer:627j
Explanation:
H=mcΔT
ΔH= 10*4.18*(300-285)
ΔH=10*4.18*15
ΔH=627j
The heat of the given water sample has been 0.627 kJ.
The specific heat has been described as the amount of heat required to raise the temperature of 1 gram of substance by 1 degree Celsius. The expression for specific heat has been given as:
Heat = mass × specific heat × change in temperature
For the given water sample:
Specific heat = 4.18 J/K/g
Mass = 10 g
Initial temperature ([tex]T_i[/tex]) = 285 K
Final temperature ([tex]T_f[/tex]) = 300 K
Change in temperature ([tex]\rm \Delta T[/tex]) can be given as:
[tex]\Delta T =T_f\;-\;T_i\\\Delta T=300\;\text K\;-\;285\;\text K\\\Delta T=15\;\text K[/tex]
Substituting the values for heat:
[tex]\rm Heat=10\;g\;\times\;4.18\;J/K/g\;\times\;15\;K\\Heat\;=\;627.6\;J\\Specific\;heat\;=\;0.627\;kJ[/tex]
The heat of the given water sample has been 0.627 kJ.
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What pressure does 3.54 moles of chlorine gas at 376 k exert on the walls of it 51.2 l container? I'm Lazy sooooo
Answer:
The answer to your question is P = 2.13 atm
Explanation:
Data
Pressure = ?
number of moles = 3.54
Temperature = 376 °K
Volume = 51.2 L
R = 0.08205 atm L/mol°K
Formula
PV = nRT
- Solve for P
P = nRT / V
- Substitution
P = (3.54)(0.08205)(376) / 51.2
- Simplification
P = 109.21 / 51.2
Result
P = 2.13 atm
Answer:
2.13
Explanation:
I just did the problem on acellus and got it right
In the 1 H NMR spectrum of chloroethane the methylene group is split into a quartet by the α and β nuclear spins of the protons on the neighboring methyl group. If the external magnetic field, Bo, directs upward, which sequence of nuclear spins contributes to the second farthest peak downfield within the spin-spin splitting pattern?
Answer:+1/2 and -1/2.
Explanation:the presence of an external magnetic field (B0), two spin states exist, +1/2 and -1/2.
The magnetic moment of the lower energy +1/2 state is aligned with the external field, but that of the higher energy -1/2 spin state is opposed to the external field.
The intermediate deshielding, when two methyl protons align with Bo and one opposes, breaking methylene protons into a quartet, is indicated by the second furthest peak in the ¹H NMR spectrum of chloroethane.
Understanding the spin-spin splitting in the ¹H NMR spectrum of chloroethane requires recognizing that the methylene (-CH₂-) protons are split into a quartet by the neighboring methyl (-CH₃) protons. These four peaks arise due to the interactions of the methylene protons with the three methyl protons, leading to different possible alignments.
The quartet results from the following combinations where the external magnetic field (Bo) is considered:
All three methyl protons aligned with Bo.Two aligned with Bo and one opposed.One aligned with Bo and two opposed.All three opposed to Bo.Focusing on the second farthest peak downfield, this corresponds to the scenario where two of the methyl protons are aligned with Bo, and one is opposed. This configuration causes intermediate deshielding, placing this peak slightly less downfield than the most deshielded single proton state.
If you combine 270.0 mL of water at 25.00 ∘ C and 140.0 mL of water at 95.00 ∘ C, what is the final temperature of the mixture? Use 1.00 g/mL as the density of water.
The final temperature of the mixture of cold water and hot water is 48.9 ⁰C.
The given parameters;
volume of the cold water = 270 mltemperature of the cold water = 25⁰Cvolume of the hot water, = 140 mltemperature of the hot water, = 95⁰Cdensity of water, = 1 g/mlThe mass of the cold water is calculated as follows;
[tex]m = \rho \times V\\\\m_c = 1 \ g/ml \ \ \times \ \ 270 \ ml \\\\m_c = 270 \ g[/tex]
The mass of the hot water is calculated as follows;
[tex]m_h = 1 \ g/ml \ \ \times \ \ 140 \ ml\\\\m_h = 140 \ g[/tex]
The final temperature of the mixture is determined by applying the principle of conservation of energy;
[tex]m_c C \Delta \theta_c = m_h C \Delta \theta_h\\\\ m_c \Delta \theta_c = m_h \Delta \theta_h\\\\m_c (t - 25) = m_h(95 - t)\\\\270(t- 25) = 140(95-t)\\\\270t - 6750 = 13,300 - 140t\\\\410t = 20,050\\\\t = \frac{20,050}{410} \\\\t = 48.9 \ ^0C[/tex]
Thus, the final temperature of the mixture of cold water and hot water is 48.9 ⁰C.
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The final temperature of the mixture is 55.00 °C.
To calculate the final temperature of the mixture, we can use the following equation:
T_final = (m_1T_1 + m_2T_2) / (m_1 + m_2)
where:
* T_final is the final temperature of the mixture (in °C)
* m_1 is the mass of the first water sample (in grams)
* T_1 is the temperature of the first water sample (in °C)
* m_2 is the mass of the second water sample (in grams)
* T_2 is the temperature of the second water sample (in °C)
We are given the following information:
* m_1 = 270.0 mL * 1.00 g/mL = 270.0 g
* T_1 = 25.00 °C
* m_2 = 140.0 mL * 1.00 g/mL = 140.0 g
* T_2 = 95.00 °C
Substituting these values into the equation above, we get the following:
T_final = (270.0 g * 25.00 °C + 140.0 g * 95.00 °C) / (270.0 g + 140.0 g)
T_final = 55.00 °C
Therefore, the final temperature of the mixture is 55.00 °C.
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How much electrical charge does an atom with 6 protons, 6 neutrons, and 5 electrons have? How much electrical charge does an atom with 6 protons, 6 neutrons, and 5 electrons have? a total charge of +17 a negative charge of -5 a positive charge of +7 a positive charge of +1 none of the above
Answer:
a positive charge of +1
Explanation:
The charge carried by atom depends on the number of protons and electrons present. The neutrons are not charged hence they do not contribute to the net charge of the specie.
The specie mentioned in the question has six protons and five electrons. Hence it has an excess of one positive charge hence a net charge of +1.
The requirements for one type of atom to substitute for another in a solid solution are:_______.A. All substitutions must be limited to the same element. B. An atom must be identical in size. C. An atom must be similar in size. D. The substituting atom must be from the same period. E. The substituting atom must be from the same group.
Answer:
E. The substituting atom must be from the same group.
Explanation:
Usually members higher-up in the group can replace or substitute lower members of a group
Suppose that the uncertainty in determining the position of an electron circling an atom in an orbit is 0.4 A. What is the uncertainty in its velocity
Answer:
Explanation:
Applying the Heisenberg uncertainty principle,
Δx X mΔv = h/4π
where Δx = uncertainty in measurement of position
Δv = uncertainty in measurement of velocity
m = mass of object
h = planck's constant
Here:
Δv = 0.4 A° = 4.0 x 10^-11 m
mass, m = 9.11 x 10^-31 Kg
Plugging the values,
4.0 x 10^-11 x Δ v = (6.626 x 10^-34) / (4 x 3.14 x 9.11E-31)
4.0 x 10^-11 x Δ v = 5.791 x 10^-5
Δv = 1.448 x 10^6 m/s, the uncertainty in its velocity
Answer = 1.45 x 10^6 m/s
The uncertainty in an electron's velocity, given an uncertainty in its position, is calculated using the Heisenberg Uncertainty Principle. By applying the principle's formula with the given position uncertainty and known electron mass, we can determine the minimum uncertainty in the electron's velocity.
Explanation:The question pertains to the Heisenberg Uncertainty Principle which is a fundamental concept in quantum physics that describes the limit to the precision with which certain pairs of physical properties of a particle, such as position and momentum, can be known simultaneously. To find the uncertainty in velocity, we use the principle's formula ΔxΔp >= ĩ/2, where Δx is the uncertainty in position, Δp is the uncertainty in momentum, and ĩ is the reduced Planck's constant (about 1.055 × 10-34 Js). Since momentum is mass times velocity (p = mv), the uncertainty in velocity (Δ4v) can be found by rearranging the formula to Δ4v >= (ĩ/(2mΔ4x)).
Given that the uncertainty in the position (Δ4x) is 0.4 Å, which is 0.4 × 10-10 meters, and assuming the electron's mass (m) as 9.11 × 10-31 kg, we can calculate the minimum uncertainty in the electron's velocity using the formula.
Remember, this is a simplification and in real-world applications, one would need to account for other factors that could affect the measurement.
Rank the solutions in order of decreasing [H3O ]. Rank solutions from largest to smallest hydronium ion concentration. To rank items as equivalent, overlap them. a. 0.10 M HNO3.
b. 0.10 M HCN.
c. 0.10 M HNO2.
d. 0.10 M HClO.e. smallest concentration.f. largest concentration.
Answer:
0.10M HCN < 0.10 M HClO < 0.10 M HNO₂ < 0.10 M HNO₃
Explanation:
We are comparing acids with the same concentration. So what we have to do first is to determine if we have any strong acid and for the rest ( weak acids ) compare them by their Ka´s ( look for them in reference tables ) since we know the larger the Ka, the more Hydronium concentration will be in these solutions at the same concentration.
HNO₃ is a strong acid and will have the largest hydronium concentration.
HCN Ka = 6.2 x 10⁻¹⁰
HNO₂ Ka = 4.0 x 10⁻⁴
HClO Ka = 3.0 x 10⁻⁸
The ranking from smallest to largest hydronium concentration will then be:
0.10M HCN < 0.10 M HClO < 0.10 M HNO₂ < 0.10 M HNO₃
Acids are substances that produce hydronium ions in solution.
According to Arrhenius definition, acids are substances that produce hydronium ions in solution. The concentration of these hydronium ions depends on the strength of the H-X bond.
The ease with which the H-X bond is broken to yield the proton is given by the Ka. The Ka is called the acid dissociation constant and shows the degree of ionization of an acid.
A strong acid has a high Ka hence it is completely dissociated in solution. A weak acid has a low Ka hence it dissociates only to a small extent in solution.
Given the equimolar solutions listed in the question, the order of hydronium ion concentration from smallest to largest is; HCN < HClO < HNO2< HNO3.
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Alkanes and alkenes differ in that alkene molecules contain at least one:
A. oxygen atom
B. double bond
C. triple bond
D. chlorine atom
Answer:
Double bond
Explanation:
an alkene is a unsaturated hydrocarbon which means that it contain at least one double bond
Answer:
The answer to your question is B. double bond.
Explanation:
Both alkanes and alkenes are hydrocarbons composed by carbon and hydrogen.
The different between these compounds is that alkanes have only single bonds are are represented as: H H
| |
H - C - C - H
| |
H H
Alkenes have at least one double bound in their structure and are represented as
H - C = C - H
| |
H H
When a solution of AgNO3 is mixed with a solution of NaBr (multiple options could be correct):
1) NaNO3 precipitate will spontaneously form.
2) After a few minutes pass, the concentration of Ag+ and Br- will be lower than when the two solutions were first mixed.
3) After a few minutes pass, the concentration of Ag+ and Br- will be the same as when the two solutions were first mixed
4) The concentration of Ag+ and Br- are momentarily greater than in a saturated solution of AgBr.
5) AgBr precipitate will spontaneously form.
Answer:
After a few minutes pass, the concentration of Ag+ and Br- will be lower than when the two solutions were first mixed.
AgBr precipitate will spontaneously form.
Explanation:
After the net ionic equation AgBr forms
The reaction between AgNO3 and NaBr leads to the formation of AgBr, a precipitate, and NaNO3, which remains dissolved in the solution. The concentration of Ag+ and Br- ions in the resulting solution will therefore be decreased.
Explanation:When a solution of AgNO3 is mixed with a solution of NaBr, a double displacement reaction or metathesis occurs, producing AgBr and NaNO3. According to solubility rules, AgBr is a precipitate, hence the options 2 and 5 are correct: After a few minutes, the concentration of Ag+ and Br- ions will be lower than when the two solutions were first mixed, and AgBr precipitate will spontaneously form. On the other hand, NaNO3 is soluble in water, so it remains dissolved and no precipitate of NaNO3 forms, which makes option 1 incorrect. Options 3 and 4 are also incorrect because the concentration of Ag+ and Br- ions will decrease as they form a precipitate and won't exceed the saturation point of AgBr.
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Which of the following statements about buffers is true? Group of answer choices A buffer composed of a weak acid of pKa = 5 is stronger at pH 4 than at pH 6. At pH values lower than the pKa, the salt concentration is higher than that of the acid. The strongest buffers are those composed of strong acids and strong bases. The pH of a buffered solution remains constant (exactly the same) no matter how much acid or base is added to the solution. When pH = pKa, the weak acid and salt concentrations in a buffer are equal.
The statement "When pH = pKa, the weak acid and salt concentrations in a buffer are equal." is true.
A solution or system that resists pH changes when small amounts of acid or base are introduced to it is called a buffer. A weak acid and its conjugate base, or a weak base and its conjugate acid, make up the substance. In order to maintain a steady pH environment for various chemical reactions or biological processes, buffers are frequently utilised in chemistry and biological sciences. They are essential for preserving homeostasis in biological systems like blood, where a steady pH is necessary for proper operation.
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Final answer:
The true statement about buffers is that they have their maximum buffering capacity when pH equals pKa, meaning the concentrations of the weak acid and its salt (conjugate base) are equal. Buffer solutions resist changes in pH effectively within a range of ± 1 pH unit from their pKa, and their buffering capacity depends on the buffer concentration.
Explanation:
The correct statement about buffers is: When pH = pKa, the weak acid and salt concentrations in a buffer are equal. This is because buffers consist of a weak acid and its conjugate base and exhibit maximum buffering capacity when the pH is numerically equal to the weak acid's pKa. At this pH, the buffer effectively resists changes in pH when small amounts of acid or base are added.
Buffer solutions are most effective within a pH range of ± 1 unit from their pKa. They are not invincible; their ability to maintain the pH level depends on the buffer concentration and the amount of strong acid or base added. The higher the concentration of the buffer components, the greater the buffer capacity, meaning more acid or base can be added before a significant change in pH occurs.
Buffers composed of weak acids work best for pH less than 7, while those composed of weak bases are more suitable for pH greater than 7. Moreover, buffers created from strong acids or bases are not effective, as they do not establish an equilibrium that is necessary for buffering action.
a 25% alcohol solution is to be mixed with a 40% alcohol solution to obtain 18 liters of a 30% alcohol solution. How many liters of each solution should be used
Answer : The volume of solution used should be, 12 L
Explanation :
Let the volume of solution be, x
Thus the equation will be:
[tex]25\%\times (x)+40\%\times (18-x)=30\%\times (18)[/tex]
Now solving the term 'x', we get:
[tex]\frac{25}{100}\times (x)+\frac{40}{100}\times (18-x)=\frac{30}{100}\times (18)[/tex]
[tex]0.25\times (x)+0.4\times (18-x)=0.3\times (18)[/tex]
[tex]0.25x+7.2-0.4x=5.4[/tex]
[tex]-0.15x=-1.8[/tex]
[tex]0.15x=1.8[/tex]
[tex]x=12[/tex]
Thus, the volume of solution used should be, 12 L
Select the compound that is most likely to increase the solubility of ZnSe when added to water.NaCnMgBr2NaClKClO4
Final answer:
NaCN is likely to increase the solubility of ZnSe in water due to complexation with Zn2+, which drives the dissolution equilibrium forward.
Explanation:
The question asks which compound is most likely to increase the solubility of ZnSe when added to water. Considering the principles of solubility and the common ion effect, the best compound to increase ZnSe solubility would not be one that provides a common ion, as that would decrease solubility. Among the options provided, NaCN seems to be the most suitable choice.
Cyanide ions from NaCN can form a complex with Zn2+, effectively removing Zn2+ from the solution and driving the dissolution equilibrium of ZnSe forward. This complexation increases the solubility of ZnSe due to Le Chatelier's principle, where the reaction shifts to alleviate the stress of the added CN- ions by dissolving more ZnSe.
A chemistry student needs of isopropenylbenzene for an experiment. He has available of a w/w solution of isopropenylbenzene in acetone. Calculate the mass of solution the student should use. If there's not enough solution, press the "No solution" button.
Question:
A chemistry student needs of 10 g isopropenylbenzene for an experiment. He has available 120 g of a 42.7% w/w solution of isopropenylbenzene in acetone. Calculate the mass of solution the student should use. If there's not enough solution, press the "No solution" button.
Answer:
The answer to the question is as follows
The mass of solution the student should use is 23.42 g.
Explanation:
To solve the question we note the following
A solution containing 42.7 % w/w of isopropenylbenzene in acetone has 42.7 g of isopropenylbenzene in 100 grams of the solution
Therefore we have 10 g of isopropenylbenzene contained in
100 g * 10 g/ 42.7 g = 23.42 g of solution
Available solution = 120 g
Therefore the quantity to used from the available solution = 23.42 g of the isopropenylbenzene in acetone solution.
Predict the precipitate produced by mixing a(n) Al(NO3)3 solution with a(n) NaOH solution. Write the molecular equation for the reaction. (Use the lowest possible coefficients. Include states-of-matter under SATP conditions in your answer.)
Answer:
Al(NO₃)₃ (aq) + NaOH(aq) → Al(OH)₃ (s)↓ + 3NaNO₃ (aq)
Explanation:
Al³⁺ cation can generate a precipitate when it bonds to OH⁻ from a strong base but it is important to the base, not to be in excess.
When the OH⁻is in excess, the produced aluminium hydroxide will be soluble.
Al³⁺(aq) + 3OH⁻(aq) ⇄ Al(OH)₃(s) ↓ Kps
At 19.9 degrees Celsius, we dissolve a salt crystal.
The Red dot on the graph in the image above represents the time it took to dissolve this salt crystal and the temperature at which it dissolved.
What temperature is represented by the red dot?
Enter the number of degrees Celsius only; no units.
Answer:
The red dot represents the melting point of the element, which as stated is approximately 19.9 degrees Celsius and how long it took for the heat to properly completely dissolve it.
The question kind of answers itself however, is there a way to re-word it or is there a different answer you're looking for?
The temperature i,e represented by the red dot is 19.9 degrees.
Calculation of the temperature;Since the Red dot on the graph shows for dissolve this salt crystal and the temperature at which it dissolved. So here the red dot shows the element melting point i.e. 19.9 degrees and also it should be take so much time for heating it properly for completely dissolving it.
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Consider mixture C, which will cause the net reaction to proceed in reverse. Concentration (M)initial:change:equilibrium:[XY]0.200+x0.200+x←net⇌[X]0.300−x0.300−x+[Y]0.300−x0.300−x The change in concentration, x, is positive for the reactants because they are produced and negative for the products because they are consumed.
This is an incomplete question, here is a complete question.
Calculating equilibrium concentrations when the net reaction proceeds in reverse Consider mixture C, which will cause the net reaction to proceed in reverse.
The chemical reaction is:
[tex]XY(g)\rightleftharpoons X(g)+Y(g)[/tex]
Concentration(M) [XY] [X] [Y]
(M)initial: 0.200 0.300 0.300
change: +x -x -x
equilibrium: 0.200+x 0.300-x 0.300-x
The change in concentration, x, is positive for the reactants because they are produced and negative for the products because they are consumed. Based on a Kc value of 0.140 and the data table given, what are the equilibrium concentrations of XY, X, and Y, respectively?
Answer : The Equilibrium concentrations of XY, X, and Y is, 0.104 M, 0.204 M and 0.204 M respectively.
Explanation :
The chemical reaction is:
[tex]XY(g)\rightleftharpoons X(g)+Y(g)[/tex]
initial: 0.200 0.300 0.300
change: +x -x -x
equilibrium: (0.200+x) (0.300-x) (0.300-x)
The equilibrium constant expression will be:
[tex]K_c=\farc{[X][Y]}{[XY]}[/tex]
Now put all the given values in this expression, we get:
[tex]0.140=\frac{(0.300-x)\times (0.300-x)}{(0.200+x)}[/tex]
By solving the term 'x', we get:
x = 0.0963 and x = 0.644
We are neglecting the value of x = 0.644 because the equilibrium concentration can not be more than initial concentration.
Thus, the value of x = 0.0963
Equilibrium concentrations of XY = 0.200+x = 0.200+0.0963 = 0.104 M
Equilibrium concentrations of X = 0.300-x = 0.300-0.0963 = 0.204 M
Equilibrium concentrations of X = 0.300-x = 0.300-0.0963 = 0.204 M
In the context of equilibrium chemistry, a net reaction can proceed in either direction until equilibrium is reached. In this case, mixture C causes the reaction to shift in the reverse direction, thereby increasing the concentration of the reactants and decreasing the concentration of the products. This continues until the forward and reverse reaction rates equalize, achieving a state of equilibrium.
Explanation:The process being described in your question is related to chemical equilibrium. When we speak about a reaction reaching equilibrium, it describes the point at which the concentrations of reactants and products do not change over time. This doesn't mean the reaction has stopped, but instead, the forward and reverse reactions are happening at the same rate due to the dynamic nature of chemical equilibria. In the case of your query, mixture C will cause the net reaction to proceed in reverse.
Using your example, [XY] represents the reactant and [X] and [Y] represent the products. Since the reaction shifts in the reverse direction, the reactants (the products in the forward reaction) increase, hence the positive change in concentration, 'x'. This process continues until the forward and reverse reaction rates become equal, which signifies the reaction's equilibrium state where concentrations of its reactants and products remain constant.
The aforementioned process is guided by the principle of Le Chatelier's, which states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change.
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Let us write the appropriate equilibria and associate the correction [tex]K_b[/tex] values. Remember, we will want to calculate the concentrations of all species in a 0.390 M Na ₂SO₃ (sodium sulfite) solution. The ionization constants for sulfurous acid are [tex]K_a_1[/tex] = 1.4 × 10⁻² and [tex]K_a_2[/tex] = 6.3 × 10⁻⁸.
Explanation:
The relation between [tex]K_a\&K_b[/tex] is given by :
[tex]K_w=K_a\times K_b[/tex]
Where :
[tex]K_w=1\times 10^{-14}[/tex] = Ionic prodcut of water
The value of the first ionization constant of sodium sulfite = [tex]K_{a1}=1.4\times 10^{-2}[/tex]
The value of [tex]K_{b1}[/tex]:
[tex]1\times 10^{-14}=1.4\times 10^{-2}\times K_{b1}[/tex]
[tex]K_{b1}=\frac{1\times 10^{-14}}{1.4\times 10^{-2}}=7.1\times 10^{-13}[/tex]
The value of the second ionization constant of sodium sulfite = [tex]K_{a2}=6.3\times 10^{-8}[/tex]
The value of [tex]K_{b2}[/tex]:
[tex]1\times 10^{-14}=6.3\times 10^{-8}\times K_{b1}[/tex]
[tex]K_{b1}=\frac{1\times 10^{-14}}{6.3\times 10^{-8}}=1.6\times 10^{-7}[/tex]
Final answer:
To find the equilibrium constant for the ionization of HSO4−, we use the equilibrium concentrations of H3O+, HSO4−, and SO42− in the given reaction formula to compute Ka.
Explanation:
To compute the equilibrium constant for the ionization of the HSO4− ion, we need to use the expression for the equilibrium constant (Ka) which is based on the concentrations of products over reactants, excluding water because its concentration is considered constant in dilute aqueous solutions. The given equilibrium is HSO4−(aq) + H2O(l) ⇒ H3O+(aq) + SO42−(aq). Given equilibrium concentrations are [H3O+] = 0.027 M, [HSO4−] = 0.29 M, and [SO42−] = 0.13 M. Hence, the equilibrium constant (Ka) is calculated as Ka = [H3O+][SO42-−]/[HSO4−] = (0.027)(0.13)/(0.29).
If a student performs an exothermic reaction in a calorimeter, how does the calculated value of ΔH (Hcalc) differ from the actual value (Hactual) if the heat exchanged with the calorimeter is not taken into account?
Answer:
The actual ∆H would be greater than the calculated value of ∆H with no calorimeter.
Explanation:
The amount of heat changed during this process at a fixed pressure is termed Enthalpy
enthalpy change ∆H = ∆E + P∆V
∆E = internal energy change
P = fixed pressure
∆V = change in volume
When energy is absorbed during reaction, it is called endothermic reaction.
Endothermic reaction carried out in the calorimeter and enthalpy change for the reaction. Since we have that
q(surrounding) = q(solution)+q(calorimeter)
Therefore, q(calorimeter) > 0(endothermic).
The actual ∆H would be greater than the calculated value of ∆H with no calorimeter.
The actual ∆H would be greater than the calculated value of ∆H with no calorimeter.
What is Enthalpy change?The amount of heat changed during this process at a fixed pressure is termed Enthalpy.
Enthalpy change ∆H = ∆E + P∆V
∆E = internal energy change
P = fixed pressure
∆V = change in volume
When energy is absorbed during reaction, it is called endothermic reaction.
Endothermic reaction carried out in the calorimeter and enthalpy change for the reaction. Since we have that
q(surrounding) = q(solution)+q(calorimeter)
Thus, q(calorimeter) > 0(endothermic).
The actual ∆H would be greater than the calculated value of ∆H with no calorimeter.
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What condition must occur when a chemical reaction is at equilibrium?
The condition is that the amounts of reactants or products do not change when a chemical reaction is in state of equilibrium.
Amounts of reactants or products do not change.
Chemical ReactionChemical equilibrium is a dynamic process in which the rate of product formation by the forward reaction equals the rate of product re-formation by the reverse reaction.
A chemical reaction is a process that results in the chemical change of one set of chemical substances into another set of chemical substances. Rust is an example of iron and oxygen mixing. Sodium acetate, carbon dioxide, and water are formed when vinegar and baking soda are combined.
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At chemical equilibrium, the forward and reverse reactions are happening at equal rates, resulting in no net change in the concentrations of reactants and products. This state is known as dynamic equilibrium. The system must also be closed for equilibrium to be maintained.
The correct answer is: The forward and reverse reactions are happening at equal rates.
Chemical equilibrium is the state in which both reactants and products are present in concentrations that remain constant over time. This occurs when the rate of the forward reaction equals the rate of the reverse reaction, meaning that there are no net changes in the concentrations of the reactants and products. This is known as dynamic equilibrium, indicating that reactions continue to occur in both directions at equal rates.
Ca3(PO4)2 + 3 H2SO4 ⟶ 2 H3PO4 + 3 CaSO4
Joaquin needs to react [m] grams of calcium phosphate. He will need to measure out ____ grams H2SO4 for this reaction.
Answer:
The answer to your question is below
Explanation:
Balanced chemical reaction
Ca₃(PO₄)₂ + 3H₂SO₄ ⇒ 2H₃SO₄ + 3CaSO₄
To answer this question just calculate the molar mass of both reactants.
Molar mass of Ca₃(PO₄)₂ = (3 x 40) + (2 x 31) + (8 x 16)
= 120 + 62 + 128
= 310 g
Molar mass of 3H₂SO₄ = 3[(2 x 1) + (1 x 32) + (4 x 16)]
= 3[2 + 32 + 64]
= 3[98]
= 294 g
Conclusion
310 g of Ca₃(PO₄)₂ will react with 294 g of 3H₂SO₄
When a strong acid is titrated with a strong base using pheolphthalein as an indicator, the color changes abruptly at the endpoint of the titration and can be switched back and forth by the addition of only one drop of acid or base. The reason for the abruptness of this color change is that:
Final answer:
The abrupt color change in a titration using phenolphthalein occurs because this indicator exhibits a sharp transition at the equivalence point, which corresponds to a steep pH change when titrating strong acids with strong bases.
Explanation:
The abrupt color change observed when titrating a strong acid with a strong base using phenolphthalein as an indicator is due to the steep pH change that occurs at the equivalence point during the titration.
Phenolphthalein is a visual indicator that exhibits a clear and distinct color change—it turns from colorless to pink—around the equivalence point.
This sharp transition is suitable for accurately determining the end point of a titration between strong acids and bases, where the pH rises rapidly, allowing for the indicator to shift from its acidic form (colorless) to its basic form (pink) in a small volume interval of titrant addition.
The general chemistry of indicators can be represented by the equation: HIn(aq) → H+ (aq) + In¯¯(aq), where 'HIn' is the acid form of the indicator that is different in color compared to its ionized form 'In¯¯'.
Such distinct color changes of acid-base indicators are critical in titrations, since they provide a visual cue for the completion of the reaction without the need to continuously monitor the pH level.
A 10.0 mL 10.0 mL aliquot is removed from the described stock solution and diluted to a total volume of 100.0 mL. 100.0 mL. Calculate the molarity of the dilute solution.
The molarity of the dilute solution is 0.5 M.
The given parameters;
initial volume of the liquid, V₁ = 10 mLvolume of the diluted solution, V₂ = 100 mLConcentration of the initial stock, C = 5 MThe molarity of the dilute solution is calculated as follows;
[tex]C_{stock} = D.F \times c_{dilute}[/tex]
where;
D.F is dilute factor
The dilute factor of the given solution is calculated as follows;
[tex]D.F = \frac{V_{dilute}}{V_{concentrate}} \\\\D.F = \frac{100}{10} \\\\D.F = 10[/tex]
[tex]C_{stock} = D.F \times c_{dilute}[/tex]
[tex]5 = D.F \times c_{dilute}\\\\c_{dilute} = \frac{5}{DF} \\\\c_{dilute} = \frac{5}{10} \\\\c_{dilute} = 0.5 \ M[/tex]
Thus, the molarity of the dilute solution is 0.5 M.
"Your question is incomplete, it seems to be missing the following information":
A 10.0 mL of a liquid is removed from the described stock solution with molarity of 5M and diluted to a total volume of 100.0 mL. Calculate the molarity of the dilute solution.
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The molar enthalpy of vaporization (∆Hvap) for ammonia (NH3) is 23.3 kJ/mol (at −33.3 °C). How much energy is required to evaporate 100. g of ammonia at this temperature?
Answer: 137 kJ
Explanation:
Latent heat of vaporization is the amount of heat required to convert 1 mole of liquid to gas at atmospheric pressure.
To calculate the moles, we use the equation:
[tex]\text{Number of moles}=\frac{\text{Given mass}}{\text {Molar mass}}=\frac{100g}{17g/mol}=5.9moles[/tex]
1 mole of ammonia requires heat = 23.3 kJ
Thus 5.9 moles of ammonia require heat =[tex]\frac{23.3}{1}\times 5.9=137kJ [/tex]
Thus the energy is required to evaporate 100 g of ammonia at this temperature is 137 kJ
Final answer:
To evaporate 100 g of ammonia at -33.3 °C, 136.76 kJ of energy is required.
Explanation:
To calculate the amount of energy required to evaporate 100 g of ammonia at -33.3 °C, we need to use the molar enthalpy of vaporization (∆Hvap). The ∆Hvap for ammonia is 23.3 kJ/mol. First, we need to convert the mass of ammonia to moles using its molar mass. The molar mass of ammonia is 17.03 g/mol. So, 100 g of ammonia is equal to 100/17.03 = 5.87 mol. Now, we can calculate the energy required:
Energy required = ∆Hvap × number of moles = 23.3 kJ/mol × 5.87 mol = 136.76 kJ
Based on Table F, which of these saturated solutions has the lowest concentration of dissolved ions? (Explain why shortly please)
1) NaCl (aq)
2) MgCl² (aq)
3) NiCl (aq)
4) AgCl (aq)
AgCl (aq)
Option: 4
Explanation:
AgCl has the lowest concentration of dissolved ions because it is insoluble. Hence, it does not allow any ions into the solution.
According to the Solubility rule, the salts that have Cl⁻ are usually soluble but Ag⁺ is an exception which shows that AgCl is insoluble. It is insoluble because the lattice structure of AgCl is very strong that it cannot be overcome by the forces that favor the formation of hydrated ions, Ag⁺(aq) and Cl⁻(aq). Solubility of AgCl in water is very low but however, it can precipitate in water.
The saturated solution that contains the concentration of dissolved ions is AgCl (aq)
Solubility rule:AgCl should contain a less concentration of dissolved ions due to insoluble. Due to this, it permits any ions into the solution. As per the above rule, the salts that have Cl⁻ are normally soluble however Ag⁺ should be an exception which represents that AgCl is insoluble. It is insoluble due to the lattice structure of AgCl should be very strong. The solubility of AgCl in water should be very low but it should be precipitated in water.
Hence, The saturated solution that contains the concentration of dissolved ions is AgCl (aq)
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Write balanced chemical equations for the complete neutralization reactions that take place when the following acids are titrated with sodium hydroxide (a) hydrochloric acid, (b) acetic acid, and (c) phosphoric acid.
Answer:
(a) [tex]NaOH_{(aq)} + HCl_{(aq)} --> NaCl_{(aq)} + H_2O_{(l)}[/tex]
(b) [tex]NaOH_{(aq)} + CH_3COOH_{(aq)} --> CH_3COONa_{(aq)} + H_2O_{(l)}[/tex]
(c) [tex]H_3PO_4_{(aq)} + 3NaOH_{(aq)} --> 3H_2O{(l)} + Na_3PO_4_{(aq)}[/tex]
Explanation:
For a reaction involving sodium hydroxide and hydrochloric acid, the balanced equation of reaction is:
[tex]NaOH_{(aq)} + HCl_{(aq)} --> NaCl_{(aq)} + H_2O_{(l)}[/tex]
For a reaction involving sodium hydroxide and acetic acid, the balanced equation of reaction is:
[tex]NaOH_{(aq)} + CH_3COOH_{(aq)} --> CH_3COONa_{(aq)} + H_2O_{(l)}[/tex]
For a reaction involving sodium hydroxide and phosphoric acid, the balanced equation of reaction is:
[tex]H_3PO_4_{(aq)} + 3NaOH_{(aq)} --> 3H_2O{(l)} + Na_3PO_4_{(aq)}[/tex]
Final answer:
This answer provides balanced chemical equations for the neutralization reactions of hydrochloric acid, acetic acid, and phosphoric acid with sodium hydroxide.
Explanation:
Neutralization Reactions:
Hydrochloric Acid with Sodium Hydroxide: HCl(aq) + NaOH(aq) → NaCl(aq) + H₂O(l)
Acetic Acid with Sodium Hydroxide: HC2H3O2(aq) + NaOH(aq) → NaC2H3O2(aq) + H₂O(l)
Phosphoric Acid with Sodium Hydroxide: H3PO4(aq) + 3NaOH(aq) → Na3PO4(aq) + 3H₂O(l)
Consider the reaction for the decomposition of hydrogen disulfide: 2H2S(g)⇌2H2(g)+S2(g), Kc = 1.67×10−7 at 800∘C A 0.500 L reaction vessel initially contains 0.163 mol of H2S and 5.00×10−2 mol of H2 at 800∘C. Find the equilibrium concentration of [S2].
Final answer:
The equilibrium concentration of [[tex]S_2[/tex]] is [tex]1.12 \times 10^{-3} M[/tex].
Explanation:
To find the equilibrium concentration of [[tex]S_2[/tex]], we need to use the equilibrium constant expression [tex]\( K_c = \frac{{[H_2]^2[S_2]}}{{[H_2S]^2}} \)[/tex]. Given the initial concentrations of [tex]H_{2}S[/tex] and [tex]H_2[/tex], and assuming x moles of [tex]H_{2}S[/tex] decompose, we can set up an ICE table and solve for the equilibrium concentrations. Substituting the equilibrium concentrations into the equilibrium constant expression and solving for [[tex]S_{2[/tex]], we find the equilibrium concentration to be [tex]1.12 \times 10^{-3} M[/tex]. This indicates the concentration of [tex]S_2[/tex] at equilibrium after the reaction has reached its dynamic equilibrium state at 800°C.
A compound is composed of 13% carbon, 4.3% hydrogen, 30.4% nitrogen, and 52.2% oxygen. The mystery compound has a molar mass of 184 grams per mole. What is the molecular formula of the compound
Answer:
C₂H₈N₄O₆ is the molecular formula for the compound
Explanation:
Data from the problem:
13 g of C in 100 g of compound
4.3 g of H in 100 g of compound
30.4 g of N in 100 g of compound
52.2 g of O in 100 g of compound
Firstly we determine, the mass of each in 184 g of compound, which is 1 mol
(13 g / 100 g) . 184 g = 24 g C
(4.3 g / 100 g) . 184 g = 7.91 g H ≅ 8 g H
(30.4 g / 100 g) . 184 g = 56 g N
(52.2 g / 100 g) . 184 g = 96 g O
And now, we divide the mass by the molar mass of each to determine the moles:
24 g C / 12 g/mol = 2 mol C
8g H / 1 g/mol = 8 mol H
56 g N / 14 g/mol = 4 mol N
96 g O / 16 g/mol = 6 mol O
So the molecular formula of the compound is C₂H₈N₄O₆
Final answer:
To determine the molecular formula of the given compound, one must calculate the moles of each element from their percentages, derive the empirical formula, and scale it by the compound's molar mass. However, the provided data seems contradictory and does not accurately represent a real calculation process.
Explanation:
To determine the molecular formula of a compound with 13% carbon, 4.3% hydrogen, 30.4% nitrogen, and 52.2% oxygen with a molar mass of 184 grams per mole, we need to first calculate the empirical formula from the given percentages. Assuming we have 100 grams of this compound, the masses of each element would directly convert to grams (e.g. 13g C, 4.3g H, 30.4g N, and 52.2g O).
To find the moles of each element, we divide the mass of each by its atomic mass (C: 12.01, H: 1.01, N: 14.01, O: 16.00) and get the ratios of moles of each element. However, the provided dissolution involves an inaccurate representation of the compound's composition and seems to contradict the given percentages.
For an accurate molecular formula determination, we use the correct composition to find the lowest whole number ratio of elements and scale it up using the compound's molar mass. This approach accurately identifies the compound's molecular makeup by aligning the empirical formula mass to the given molar mass.