Library Guides: Chemistry Textbook: Self-Assessments

1. Matter and MeasurementsToggle Dropdown
2. Atoms, Molecules and IonsToggle Dropdown
3. Composition of Substances and SolutionsToggle Dropdown
4. Stoichiometry of Chemical ReactionsToggle Dropdown
5. ThermochemistryToggle Dropdown
6. GasesToggle Dropdown
7. Chemical Bonding and Molecular GeometryToggle Dropdown
8. Liquids, Solids, and Modern MaterialsToggle Dropdown
9. Solutions and Colligative PropertiesToggle Dropdown
10. KineticsToggle Dropdown
11. Chemical Equilibria and Applications
12. ThermodynamicsToggle Dropdown
13. ElectrochemistryToggle Dropdown
14. AppendicesToggle Dropdown

Self-Assessments

Equilibrium Constant
LeChatelier's Principle
Calculating Equillibrium constants or concentrations
pH, pOH, [H+] and [OH-]
Acid-base and solubility equilibria

Which of the following is the correct expression of equilibrium constant, K_P, for the following reaction?
2SO₂(g)+O₂(g)⇌2SO₃(g)

Choose 1 answer

K_{P} = \frac{P_{S O_{2}} P_{O_{2}}}{P_{S O_{3}}}

K_{P} = \frac{P_{S O_{3}}}{P_{S O_{2}} P_{O_{2}}}

K_{P} = \frac{{P_{S O_{2}}}^{2} P_{O_{2}}}{{P_{S O_{3}}}^{2}}

K_{P} = \frac{{P_{S O_{3}}}^{2}}{{P_{S O_{2}}}^{2} P_{O_{2}}}

K_{P} = \frac{{P_{S O_{3}}}^{2} + P_{O_{2}}}{{P_{S O_{3}}}^{2}}

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Which of the following reactions does NOT have the equilibrium constant correctly written?

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{2 N a H C O}_{3} (s) ⇌ {N a}_{2} C O_{3} (s) + H_{2} O (g) + {C O}_{2} (g); K = [H_{2} O] [C O_{2}]

P b I_{2} (s) ⇌ {P b}^{2 +} (a q) + 2 I^{-} (a q); K = [{P b}^{2 +}] {[I^{-}]}^{2}

2 H_{2} O (l) ⇌ H_{3} O^{+} (a q) + O H^{-} (a q); K = \frac{[H_{3} O^{+}] [O H^{-}]}{{[H_{2} O]}^{2}}

H F (a q) ⇌ H^{+} (a q) + F^{-} (a q); K = \frac{[H^{+}] [F^{-}]}{[H F]}

N_{2} O (g) + \frac{1}{2} O_{2} (g) ⇌ 2 N O (g); K = \frac{{[N O]}^{2}}{[N_{2} O] {[O_{2}]}^{1 / 2}}

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If the equilibrium constant, is large (K>>1), it means _________.

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The products predominate at equilibrium

The reactants predominate at equilibrium

Both reactants and products predominate at equilibrium.

The forward reaction is faster than the reverse reaction.

There is not enough information to determine.

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Hydrogen and nitrogen react to form ammonia according to the following balanced chemical equation. The value of equilibrium constant (K_p) for the reaction at 745 K is shown below:
3H₂(g)+N₂(g) ⇌ 2NH₃(g); K_P = 3.16 × 10^-5.

If the partial pressure of Hydrogen, nitrogen and ammonia gases in a reaction container were 30.1 atm, 60.5 atm and 15.2 atm at 745 K, is the reaction at equilibrium? Which direction will it proceed to reach equilibrium?

Choose 1 answer

the reaction is already at equilibrium.

the reaction is not at equilibrium; it will proceed in the forward direction producing more NH₃ to reach equilibrium.

the reaction is not at equilibrium; it will proceed in the reverse direction producing more H₂ and N₂ to reach equilibrium.

The reaction will never reach equilibrium.

Not enough information to determine.

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The equilibrium constant (K_P) for the following reaction at 25^oC is provided below:
CaCl₂⋅6H₂O(s) ⇌ CaCl₂(s) + 6H₂O(g); K_P= 09 × 10⁻⁴⁴

What is the value of K_c for the reaction?

Choose 1 answer

2.38 × 10⁻⁵²

1.42 × 10⁻⁴⁹

1.82 × 10⁻³⁸

1.09 × 10⁻³⁵

3.16 × 10⁻²⁹

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For the reaction, CH₄(g) + 2H₂S(g) ⇌ CS₂(g) + 4H₂(g) at equilibrium, which of the following favors the formation of products?

Choose 1 answer

decreasing the concentration of CH₄

decreasing the concentration of H₂S

decreasing the concentration of CS₂

increasing the pressure

increasing the concentration of H₂.

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For the exothermic reaction, 2C(s)+O₂(g) ⇌ 2CO(g) at equilibrium, which of the following causes more product formation?

Choose 1 answer

A) decreasing the volume of the container

B) lowering the temperature

C) increasing the temperature

D) both A and B

E) both A and C

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For the reaction,
CO₂(g) + C(s) ⇄ 2CO(g); DH = +171 kJ,
which of the following will shift the equilibrium to the right?

Choose 1 answer

adding carbon

removing CO₂

adding CO

lowering the temperature

decreasing the pressure

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For the reaction,
2SO₂(g) + O₂(g) ⇄ 2SO₃(g); DH = -196 kJ,
what causes an increase in concentration of SO₂(g)?

Choose 1 answer

removing SO₃(g)

decreasing the temperature

increasing the pressure

decreasing the volume of the container

removing O₂(g)

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Consider the dissociation of the weak acid, HF:
HF(aq) ⇌ H⁺(aq) + F^-(aq).
Which of the following will increase the ionization of the acid?

Choose 1 answer

adding HCl(aq)

adding KF(aq)

adding NaOH(aq)

adding water

adding a catalyst

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Calculate the value of the equilibrium constant (K_P) for the reaction 2NO(g)+Cl₂(g)⇌2NOCl(g)from these equilibrium pressures: NO, 0.050 atm; Cl₂, 0.30 atm; NOCl, 1.2 atm.

Choose 1 answer

1.9 × 10³

170

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A flask initially contained hydrogen sulfide at a pressure of 5.00 atm at 313 K. When the reaction reached equilibrium, the partial pressure of sulfur vapor was found to be 0.15 atm.
2H₂S(g)⇌2H₂(g)+S₂(g) What is the K_p for the reaction?

Choose 1 answer

0.125

1.82 × 10^-3

4.32 × 10^-3

6.11 × 10^-4

2.35 × 10^-5

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At a certain temperature and pressure, NO₂with an initial concentration of 1.00 M is 4.0% decomposed into NO and O₂. Calculate the value of the equilibrium constant for the reaction.
2NO2(g)⇌2NO(g)+O2(g)

Choose 1 answer

0.21

1.3 × 10^-4

3.5 × 10^-5

7.4 × 10^-6

0.0092

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For the reaction of bromine gas with chlorine gas shown below, K_c=7.0 at 400 K.
A container was charged with 0.60 M bromine gas and 0.60 M chlorine gas at 400 K. Calculate the equilibrium concentration of BrCl.
Br₂(g) + Cl₂(g) ⇌ 2BrCl(g)

Choose 1 answer

0.68 M

0.53 M

0.44 M

0.26 M

2.30 M

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Calculate the equilibrium concentration of NO₂ in 2.00 L vessel that was charged with 1.3 mol of N₂O₄and 1.1 mol at 100^o
N₂O₄(g)⇌2NO₂(g); K_c=0.21 at 100^oC.

Choose 1 answer

0.71 M

0.57 M

0.41 M

0.39 M

0.27 M

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What is the conjugate base of H₃O₂⁺?

Choose 1 answer

H₂O

H₄O₂²⁺

H₂O₂

H₂O₂⁺

H₄O₃

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The water in an aquarium has a pH of 7.50. What is the hydroxide ion concentration in the aquarium?

Choose 1 answer

3.1 × 10^-7 M

3.2 × 10^-8 M

6.5 M

4.2 × 10^-8 M

4.2 × 10^-4 M

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What is the pH of 4.0 × 10^-3 M Ca(OH)₂?

Choose 1 answer

10.60 M

10.90 M

11.24 M

3.10 M

3.40 M

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The hydronium ion concentration in a sample of rainwater is found to be 1.7 ×10⁻⁶ M at 25 °C. What is the concentration of hydroxide ions in the rainwater?

Choose 1 answer

1.87 × 10^-8 M

4.12 × 10^-8 M

3.09 × 10^-9 M

5.88 × 10^-9 M

2.43 × 10^-7 M

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Which of the following solutions is the most acidic?

Choose 1 answer

pH = 5.06

[OH^-] = 4.5 × 10^-6 M

[H⁺] = 1.23 × 10^-3 M

pOH = 11.29

0.0016 M HNO₃

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Calculate the Ka of 2.38×10^-4 M hypochlorous acid (HClO) if it has a pH of 5.57.

Choose 1 answer

9.07 × 10^-6

4.01 × 10^-7

1.01 × 10^-7

7.01 × 10^-8

3.08 × 10^-8

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What is the K_b and percent ionization of a 0.012 M weak base that has a pH of 11.01.

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K_b = 4.9 × 10^-6; 3.2%

K_b = 7.3 × 10^-6; 6.2%

K_b = 2.1 × 10^-5; 4.5%

K_b = 9.5 × 10^-5; 8.5%

K_b = 8.0 × 10^-21; 0.85%

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The ionization constant of lactic acid, CH₃CH(OH)CO₂H, an acid found in the blood after strenuous exercise, is 1.36 ×10⁻⁴.
What is the pH of 0.22 M lactic acid?

Choose 1 answer

2.26

3.21

4.17

4.58

5.49

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What is [H₃O⁺] in a buffer solution of 0.25 MCH₃CO₂H and 0.030 M NaCH₃CO₂?
K_a of CH₃CO₂H is 1.8 × 10^-5

Choose 1 answer

2.8 × 10^-6 M

1.5 × 10^-6 M

2.4 × 10^-5 M

1.4 × 10^-5 M

6.3 × 10^-5 M

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Ag₂CrO₄ has a molar solubility of 1.2 × 10^-4mol/L at a certain temperature. What is the solubility product (K_sp) of Ag₂CrO₄ at that temperature?

Choose 1 answer

5.1 × 10^-12

6.9 × 10^-12

4.5 × 10^-12

5.1 × 10^-13

7.3 × 10^-13

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Chemistry Textbook

Self-Assessments

Which of the following is the correct expression of equilibrium constant, KP, for the following reaction? 2SO2(g)+O2(g)⇌2SO3(g)

Which of the following reactions does NOT have the equilibrium constant correctly written?

If the equilibrium constant, is large (K>>1), it means _________.

The equilibrium constant (KP) for the following reaction at 25oC is provided below:CaCl2⋅6H2O(s) ⇌ CaCl2(s) + 6H2O(g); KP = 09 × 10−44What is the value of Kc for the reaction?

For the reaction, CH4(g) + 2H2S(g) ⇌ CS2(g) + 4H2(g) at equilibrium, which of the following favors the formation of products?

For the exothermic reaction, 2C(s)+O2(g) ⇌ 2CO(g) at equilibrium, which of the following causes more product formation?

For the reaction, CO2(g) + C(s) ⇄ 2CO(g); DH = +171 kJ,which of the following will shift the equilibrium to the right?

For the reaction, 2SO2(g) + O2(g) ⇄ 2SO3(g); DH = -196 kJ,what causes an increase in concentration of SO2(g)?

Consider the dissociation of the weak acid, HF:HF(aq) ⇌ H+(aq) + F-(aq).Which of the following will increase the ionization of the acid?

Calculate the value of the equilibrium constant (KP) for the reaction 2NO(g)+Cl2(g)⇌2NOCl(g)from these equilibrium pressures: NO, 0.050 atm; Cl2, 0.30 atm; NOCl, 1.2 atm.

A flask initially contained hydrogen sulfide at a pressure of 5.00 atm at 313 K. When the reaction reached equilibrium, the partial pressure of sulfur vapor was found to be 0.15 atm.2H2S(g)⇌2H2(g)+S2(g) What is the Kp for the reaction?

At a certain temperature and pressure, NO2with an initial concentration of 1.00 M is 4.0% decomposed into NO and O2. Calculate the value of the equilibrium constant for the reaction. 2NO2(g)⇌2NO(g)+O2(g)

For the reaction of bromine gas with chlorine gas shown below, Kc=7.0 at 400 K.A container was charged with 0.60 M bromine gas and 0.60 M chlorine gas at 400 K. Calculate the equilibrium concentration of BrCl.Br2(g) + Cl2(g) ⇌ 2BrCl(g)

Calculate the equilibrium concentration of NO2 in 2.00 L vessel that was charged with 1.3 mol of N2O4and 1.1 mol at 100oN2O4(g)⇌2NO2(g); Kc=0.21 at 100oC.

What is the conjugate base of H3O2+?

The water in an aquarium has a pH of 7.50. What is the hydroxide ion concentration in the aquarium?

What is the pH of 4.0 × 10-3 M Ca(OH)2?

The hydronium ion concentration in a sample of rainwater is found to be 1.7 ×10−6 M at 25 °C. What is the concentration of hydroxide ions in the rainwater?

Which of the following solutions is the most acidic?

Calculate the Ka of 2.38×10-4 M hypochlorous acid (HClO) if it has a pH of 5.57.

What is the Kb and percent ionization of a 0.012 M weak base that has a pH of 11.01.

The ionization constant of lactic acid, CH3CH(OH)CO2H, an acid found in the blood after strenuous exercise, is 1.36 ×10−4. What is the pH of 0.22 M lactic acid?

What is [H3O+] in a buffer solution of 0.25 MCH3CO2H and 0.030 M NaCH3CO2?Ka of CH3CO2H is 1.8 × 10-5

Ag2CrO4 has a molar solubility of 1.2 × 10-4 mol/L at a certain temperature. What is the solubility product (Ksp) of Ag2CrO4 at that temperature?

Which of the following is the correct expression of equilibrium constant, K_P, for the following reaction?
2SO₂(g)+O₂(g)⇌2SO₃(g)

The equilibrium constant (K_P) for the following reaction at 25^oC is provided below:
CaCl₂⋅6H₂O(s) ⇌ CaCl₂(s) + 6H₂O(g); K_P= 09 × 10⁻⁴⁴

What is the value of K_c for the reaction?

For the reaction, CH₄(g) + 2H₂S(g) ⇌ CS₂(g) + 4H₂(g) at equilibrium, which of the following favors the formation of products?

For the exothermic reaction, 2C(s)+O₂(g) ⇌ 2CO(g) at equilibrium, which of the following causes more product formation?

For the reaction,
CO₂(g) + C(s) ⇄ 2CO(g); DH = +171 kJ,
which of the following will shift the equilibrium to the right?

For the reaction,
2SO₂(g) + O₂(g) ⇄ 2SO₃(g); DH = -196 kJ,
what causes an increase in concentration of SO₂(g)?

Consider the dissociation of the weak acid, HF:
HF(aq) ⇌ H⁺(aq) + F^-(aq).
Which of the following will increase the ionization of the acid?

Calculate the value of the equilibrium constant (K_P) for the reaction 2NO(g)+Cl₂(g)⇌2NOCl(g)from these equilibrium pressures: NO, 0.050 atm; Cl₂, 0.30 atm; NOCl, 1.2 atm.

A flask initially contained hydrogen sulfide at a pressure of 5.00 atm at 313 K. When the reaction reached equilibrium, the partial pressure of sulfur vapor was found to be 0.15 atm.
2H₂S(g)⇌2H₂(g)+S₂(g) What is the K_p for the reaction?

At a certain temperature and pressure, NO₂with an initial concentration of 1.00 M is 4.0% decomposed into NO and O₂. Calculate the value of the equilibrium constant for the reaction.
2NO2(g)⇌2NO(g)+O2(g)

For the reaction of bromine gas with chlorine gas shown below, K_c=7.0 at 400 K.
A container was charged with 0.60 M bromine gas and 0.60 M chlorine gas at 400 K. Calculate the equilibrium concentration of BrCl.
Br₂(g) + Cl₂(g) ⇌ 2BrCl(g)

Calculate the equilibrium concentration of NO₂ in 2.00 L vessel that was charged with 1.3 mol of N₂O₄and 1.1 mol at 100^o
N₂O₄(g)⇌2NO₂(g); K_c=0.21 at 100^oC.

What is the conjugate base of H₃O₂⁺?

What is the pH of 4.0 × 10^-3 M Ca(OH)₂?

The hydronium ion concentration in a sample of rainwater is found to be 1.7 ×10⁻⁶ M at 25 °C. What is the concentration of hydroxide ions in the rainwater?

Calculate the Ka of 2.38×10^-4 M hypochlorous acid (HClO) if it has a pH of 5.57.

What is the K_b and percent ionization of a 0.012 M weak base that has a pH of 11.01.

The ionization constant of lactic acid, CH₃CH(OH)CO₂H, an acid found in the blood after strenuous exercise, is 1.36 ×10⁻⁴.
What is the pH of 0.22 M lactic acid?

What is [H₃O⁺] in a buffer solution of 0.25 MCH₃CO₂H and 0.030 M NaCH₃CO₂?
K_a of CH₃CO₂H is 1.8 × 10^-5

Ag₂CrO₄ has a molar solubility of 1.2 × 10^-4mol/L at a certain temperature. What is the solubility product (K_sp) of Ag₂CrO₄ at that temperature?