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[answered] 1. Ka for HF is 6.8 x 10-4. What is the pH of a 0.35M solut



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1. Ka for HF is 6.8 x 10-4. What is the pH of a 0.35M solution of HF?

 

a. 1.81

 

b. 3.62

 

c. 0.46

 

d. 13.54

 

2. Calculate the pH of a 0.0015M HCl solution.

 

a. -2.82

 

b. 6.50

 

c. 2.82

 

d. 1.5 x 10-3

 

e. 11.18

 

3. Given the following Ka values,

 

HC2H3O2

 

Ka = 1.8 x 10-5

 

HClO3

 

Ka = 5.0 x 102

 

HCN

 

Ka = 4.9 x 10-10

 

HF

 

Ka = 6.8 x 10-4

 

HOCl

 

Ka = 3.0 x 10-8 4. 5. 6. 7. 8. Which of the following is the weakest base?

 

a. ClO3b. C2H3O2c. CNd. OCle. FIdentify the acid and base on each side of the following equation:

 

HSO3- + HPO42SO32- + H2PO4a. base/acid---acid/base

 

b. not an acid-base reaction

 

c. acid/base ---acid/base

 

d. acid/base---base/acid

 

e. base/acid---base/acid

 

Milk of Magnesia antacid has a pH of 10.25. What is the [OH -] in this solution?

 

a. 1.8 x 10-4

 

b. 5.6 x 10-11

 

c. 2.4 x 10-2

 

d. 3.75

 

e. 5.6 x 10-25

 

The Ka of nicotinic acid is 1.4 x 10-5. What is the percent ionization of nicotinic acid in a 0.10 M solution?

 

a. 10 percent

 

b. 100 percent

 

c. 98.8 percent

 

d. 1.2 percent

 

e. 0.12 percent

 

Which one of the following does not act as an acid in water?

 

a. Al3+

 

b. Ca2+

 

c. Fe2+

 

d. Cu2+

 

e. Cr3+

 

Which one of the following statements is true regarding strengths of acids and bases? 9. 10. 11. 12. 13. 14. 15. a. The conjugate of a ?weak? acid is a ?strong? base.

 

b. Once a hydrogen cation dissociates from a weak acid, it never pairs itself again with the

 

conjugate base.

 

c. The conjugates of strong acids and bases have no significant base-acid strengths in aqueous

 

solution and are essentially ?neutral?.

 

d. A weaker acid can be mixed with a weaker base to yield a stronger acid and a stronger base.

 

e. All weak acids are equally weak.

 

The pH of a 0.25 M solution of HCN is 4.90. Calculate the Ka value for HCN.

 

a. 6.3 x 10-10

 

b. 1.26 x 10-5

 

c. More information is needed.

 

d. 2.29 x 10-4

 

e. 7.94 x 10-10

 

Which one of the following salts will have a water solution with a pH less than 7?

 

a. K2CO3

 

b. NaBr

 

c. NH4Cl

 

d. KCN

 

e. NaC2H3O2

 

A mixture is prepared with [CO] = 0.035, [Cl 2] = 0.015, and [COCl2] = 0.95. It is known that Kc for the

 

equilibrium CO(g) + Cl2(g)

 

COCl2(g) is 1.2 x 103 at 400?C. Predict what will happen.

 

a. The reaction occurs in the reverse direction.

 

b. The reaction occurs in the forward direction.

 

c. The reaction is at equilibrium, so no net reaction occurs.

 

d. It is impossible to predict without more information.

 

At a particular temperature Kc = 54 for the reaction H2(g) + I2(g)

 

2HI(g).

 

If 1.0 mole of H2 and 1.0 mole of I2 are placed in a 5.0 L container, what would be the equilibrium

 

concentration of HI?

 

a. 0.88 M

 

b. 0.16 M

 

c. 0.31 M

 

d. 0.79 M

 

e. 1.57 M

 

Which of the following statements is true?

 

a. Q does not change with temperature.

 

b. Keq does not change with temperature, whereas Q is temperature dependent.

 

c. K does not depend on the concentrations or partial pressures of reaction components.

 

d. Q does not depend on the concentrations or partial pressures of reaction components.

 

e. Q is the same as Keq when a reaction is at equilibrium.

 

C6H6(g) + 3H2(g)

 

C6H12(g)

 

When 1.00 mol C6H6 and 3.00 mol H2 are put into a 200-L container and allowed to reach equilibrium

 

over a catalyst at an elevated temperature, the resulting mixture contains 0.137 mol C 6H12. What is the

 

equilibrium amount of H2 in moles?

 

a. 3.41 mol

 

b. 0.137 mol

 

c. 2.59 mol

 

d. 3.14 mol

 

e. 2.86 mol

 

A mixture of H2, S, and H2S is held in a 1.0-L vessel at 90?C until the following equilibrium is achieved:

 

H2(g) + S(s)

 

H2S(g) At equilibrium the mixture contains 0.46 g of H 2S and 0.40 g H2. What is the value of Kc for the reaction at

 

this temperature?

 

a. 3.4 x 10-1

 

b. Need to know the amount of S present

 

c. 1.5 x 101

 

d. 6.8 x 10-2

 

e. 2.9

 

16. For the endothermic reaction

 

CaCO3 (s)

 

CaO (s) + CO2 (g)

 

Le Chatelier?s principle predicts that ________ will result in an increase in the number of moles of CO 2.

 

a. Increasing the temperature

 

b. Decreasing the temperature

 

c. Increasing the pressure

 

d. Removing some of the CaCO3(s)

 

17. The equilibrium-constant expression depends on the ________ of the reaction.

 

a. Stoichiometry

 

b. Mechanism

 

c. Stoichiometry and mechanism

 

d. The quantities of reactants and products initially present

 

e. Temperature

 

18. The value of Keq at the same temperature for the reaction below is ________. 3C (g) + 3D (g)

 

3A (g) + 3B (g)

 

a. 2.4 x 102

 

b. 2.1

 

c. 4.1 x 10-3

 

d. 5.3 x 10-2

 

e. 6.3

 

19. The expression of Keq for the following reaction will not include ________.

 

A(g) + B (g)

 

C (l) + D (g)

 

a. [C]

 

b. [A]

 

c. [B]

 

d. [D]

 

e. None of the above

 

20. Phosphorous trichloride and phosphorous pentachloride equilibrate in the presence of molecular

 

chlorine according to the reaction:

 

PCl3 (g) + Cl2 (g) ? PCl5 (g)

 

An equilibrium mixture at 450 K contains

 

PPCl = 0.224 atm,

 

3

 

PCl = 0.284 atm, and

 

2

 

PPCl = 4.24 atm. What is the value of K p at this temperature?

 

5

 

a.

 

b.

 

c.

 

d. 66.7

 

1.50 x 10-2

 

2.70 x 10-1

 

3.75 e. 8.36

 


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