Question 1

Calculate the pH of a solution that is 0.410 M in HOCl and 0.050 M in NaOCl.[Ka(HOCl)= 3.2 * 10-8]

Accepted Answer

A) 0.39 
B) 3.94 
C) 6.58 
D) 7.49 
E) 8.40 
A) 0.39 
B) 3.94 
C) 6.58 
D) 7.49 
E) 8.40

Question 2

Which of the following is the most acidic solution?

Accepted Answer

A) 0.10 M CH3COOH and 0.10 M CH3COONa 
B) 0.10 M CH3COOH 
C) 0.10 M HNO2 
D) 0.10 M HNO2 and 0.10 M NaNO2 
E) 0.10 M CH3COONa 
A) 0.10 M CH3COOH and 0.10 M CH3COONa 
B) 0.10 M CH3COOH 
C) 0.10 M HNO2 
D) 0.10 M HNO2 and 0.10 M NaNO2 
E) 0.10 M CH3COONa

Question 3

The solubility product for chromium(III)fluoride is Ksp = 6.6 * 10-11. What is the molar solubility of chromium(III)fluoride?

Accepted Answer

A) 1.6 * 10-3 M 
B) 1.2 * 10-3 M 
C) 6.6 * 10-11 M 
D) 2.2 * 10-3 M 
E) 1.6 * 10-6 M 
A) 1.6 * 10-3 M 
B) 1.2 * 10-3 M 
C) 6.6 * 10-11 M 
D) 2.2 * 10-3 M 
E) 1.6 * 10-6 M

Question 4

Will a precipitate of magnesium fluoride form when 300.mL of 1.1 * 10-3 M MgCl2 are added to 500.mL of 1.2 * 10-3 M NaF? [Ksp (MgF2)= 6.9 * 10-9]

Accepted Answer

A) Yes, Q > Ksp 
B) No, Q sp 
C) No, Q = Ksp 
D) Yes, Q sp 
A) Yes, Q > Ksp 
B) No, Q sp 
C) No, Q = Ksp 
D) Yes, Q sp

Question 5

Will a precipitate (ppt)form when 20.0 mL of 1.1 * 10-3 M Ba(NO3)2 are added to 80.0 mL of 8.4 *10-4 M Na2CO3?

Accepted Answer

A) Yes, the ppt is Ba(NO3 )2. 
B) Yes, the ppt is NaNO3. 
C) Yes, the ppt is BaCO3. 
D) Yes, the ppt is Na2CO3. 
E) No, a precipitate will not form. 
A) Yes, the ppt is Ba(NO3 )2. 
B) Yes, the ppt is NaNO3. 
C) Yes, the ppt is BaCO3. 
D) Yes, the ppt is Na2CO3. 
E) No, a precipitate will not form.

Question 6

Will a precipitate (ppt)form when 300.mL of 2.0 * 10-5 M AgNO3 are added to 200.mL of 2.5 * 10-9 M NaI? Answer yes or no, and identify the precipitate if there is one.

Accepted Answer

A) Yes, the ppt is AgNO3(s). 
B) Yes, the ppt is NaNO3(s). 
C) Yes, the ppt is NaI(s). 
D) Yes, the ppt is AgI(s). 
E) No, a precipitate will not form. 
A) Yes, the ppt is AgNO3(s). 
B) Yes, the ppt is NaNO3(s). 
C) Yes, the ppt is NaI(s). 
D) Yes, the ppt is AgI(s). 
E) No, a precipitate will not form.

Question 7

Calculate the concentration of chloride ions in a saturated lead(II)chloride (Ksp = 2.4 * 10-4)solution.

Accepted Answer

A) 2.4 * 10-4 M 
B) 4.8 * 10-4 M 
C) 3.9 * 10-2 M 
D) 1.2 * 10-1 M 
E) 7.8 * 10-2 M 
A) 2.4 * 10-4 M 
B) 4.8 * 10-4 M 
C) 3.9 * 10-2 M 
D) 1.2 * 10-1 M 
E) 7.8 * 10-2 M

Question 8

Calculate the minimum concentration of Mg2+ that must be added to 0.10 M NaF in order to initiate a precipitate of magnesium fluoride. (For MgF2 , Ksp = 6.9 * 10-9.)

Accepted Answer

A) 1.4 * 107 M 
B) 6.9 * 10-9 M 
C) 6.9 * 10-8 M 
D) 1.7 * 10-7 M 
E) 6.9 * 10-7 M 
A) 1.4 * 107 M 
B) 6.9 * 10-9 M 
C) 6.9 * 10-8 M 
D) 1.7 * 10-7 M 
E) 6.9 * 10-7 M

Question 9

The molar solubility of lead(II)iodate in water is 4.0 * 10-5 mol/L. Calculate Ksp for lead(II)iodate.

Accepted Answer

A) 1.6 * 10-9 
B) 6.4 * 10-14 
C) 2.6 * 10-13 
D) 4.0 * 10-5 
E) 4.0 * 10-15 
A) 1.6 * 10-9 
B) 6.4 * 10-14 
C) 2.6 * 10-13 
D) 4.0 * 10-5 
E) 4.0 * 10-15

Question 10

Calculate the equilibrium constant Kc for the following overall reaction:
AgCl(s)+ 2CN-(aq)   Ag(CN)2-(aq)+ Cl-(aq)
For AgCl, Ksp = 1.6 * 10-10; for Ag(CN)2-, Kf = 1.0 * 1021.

Accepted Answer

1.6 * 10<s

Question 11

The concentration of Mg2+ in seawater is 5.0 * 10-2 M. What hydroxide concentration is needed to remove 90% of the Mg2+ by precipitation? (For Mg(OH)2, Ksp = 1.2 * 10-11.)

Accepted Answer

4.9 * 10<s

Question 12

At 25 °C, the base ionization constant for NH3 is 1.8 * 10-5. Determine the pH of a solution prepared by adding 0.0500 mol of solid ammonium chloride to 100.mL of 0.150 M ammonia.

Accepted Answer

The answer of At 25 °C, the base ionization constant...

Question 13

Calculate the equilibrium constant Kc for the net reaction shown below.
AgI(s)+ 2NH3(aq)   Ag(NH3)2+(aq)+ I-(aq)
For AgI, Ksp = 8.3 * 10-17; for Ag(NH3)2+, Kf = 1.5 * 107.

Accepted Answer

1.2 * 10<s

Question 14

The Ksp value for lead(II)chloride is 2.4 * 10-4. What is the molar solubility of lead(II)chloride?

Accepted Answer

A) 2.4 * 10-4 mol/L 
B) 6.2 * 10-2 mol/L 
C) 7.7 * 10-3 mol/L 
D) 3.9 * 10-2 mol/L 
E) 6.0 * 10-5 mol/L 
A) 2.4 * 10-4 mol/L 
B) 6.2 * 10-2 mol/L 
C) 7.7 * 10-3 mol/L 
D) 3.9 * 10-2 mol/L 
E) 6.0 * 10-5 mol/L

Question 15

How many moles of NaF must be dissolved in 1.00 liter of a saturated solution of PbF2 at 25°C to reduce the [Pb2+] to 1.0 * 10-6 M? The Ksp for PbF2 at 25 °C is 4.0 * 10-8.

Accepted Answer

The answer of How many moles of NaF must be...

Question 16

What is the effective pH range for a sodium acetate/acetic acid buffer? (For CH3COOH, Ka = 1.8 * 10-5)

Accepted Answer

The answer of What is the effective pH range for...

Question 17

Assuming equal concentrations of conjugate base and acid, which one of the following mixtures is suitable for making a buffer solution with an optimum pH of 9.2-9.3?

Accepted Answer

A) CH3COONa / CH3COOH (Ka = 1.8 * 10-5) 
B) NH3 / NH4Cl (Ka = 5.6 * 10-10) 
C) NaOCl / HOCl (Ka = 3.2 * 10-8) 
D) NaNO2 / HNO2 (Ka = 4.5 * 10-4) 
E) NaCl / HCl 
A) CH3COONa / CH3COOH (Ka = 1.8 * 10-5) 
B) NH3 / NH4Cl (Ka = 5.6 * 10-10) 
C) NaOCl / HOCl (Ka = 3.2 * 10-8) 
D) NaNO2 / HNO2 (Ka = 4.5 * 10-4) 
E) NaCl / HCl

Question 18

Will Fe(OH)3 precipitate from a buffer solution that is 0.60 M CH3COOH and 0.10 M CH3COONa, if the solution is also made to be 0.001 M in Fe3+? For Fe(OH)3, Ksp = 6.8 * 10-36.

Accepted Answer

The answer of Will Fe(OH)3 precipitate from a buffer solution...

Question 19

Describe how to prepare 500.mL of a cyanic acid (HCNO)/sodium cyanate (NaCNO)buffer having a pH of 4.80. [Ka(HCNO)= 2.0 * 10-4]

Accepted Answer

Dissolve amounts of the two compounds eq

Question 20

At 25 °C, the base ionization constant for NH3 is 1.8 * 10-5. Determine the hydroxide ion concentration in a 0.150 M solution of ammonia at 25 °C.

Accepted Answer

1.6 * 10<s

Exam 16: Acid-Base Equilibria and Solubility Equilibria

Calculate the pH of a solution that is 0.410 M in HOCl and 0.050 M in NaOCl.[Ka(HOCl)= 3.2 * 10-8]

Which of the following is the most acidic solution?

The solubility product for chromium(III)fluoride is Ksp = 6.6 * 10-11. What is the molar solubility of chromium(III)fluoride?

Will a precipitate of magnesium fluoride form when 300.mL of 1.1 * 10-3 M MgCl2 are added to 500.mL of 1.2 * 10-3 M NaF? [Ksp (MgF2)= 6.9 * 10-9]

Will a precipitate (ppt)form when 20.0 mL of 1.1 * 10-3 M Ba(NO3)2 are added to 80.0 mL of 8.4 *10-4 M Na2CO3?

Will a precipitate (ppt)form when 300.mL of 2.0 * 10-5 M AgNO3 are added to 200.mL of 2.5 * 10-9 M NaI? Answer yes or no, and identify the precipitate if there is one.

Calculate the concentration of chloride ions in a saturated lead(II)chloride (Ksp = 2.4 * 10-4)solution.

Calculate the minimum concentration of Mg2+ that must be added to 0.10 M NaF in order to initiate a precipitate of magnesium fluoride. (For MgF2 , Ksp = 6.9 * 10-9.)

The molar solubility of lead(II)iodate in water is 4.0 * 10-5 mol/L. Calculate Ksp for lead(II)iodate.

Calculate the equilibrium constant Kc for the following overall reaction: AgCl(s)+ 2CN-(aq) Ag(CN)2-(aq)+ Cl-(aq) For AgCl, Ksp = 1.6 * 10-10; for Ag(CN)2-, Kf = 1.0 * 1021.

The concentration of Mg2+ in seawater is 5.0 * 10-2 M. What hydroxide concentration is needed to remove 90% of the Mg2+ by precipitation? (For Mg(OH)2, Ksp = 1.2 * 10-11.)

At 25 °C, the base ionization constant for NH3 is 1.8 * 10-5. Determine the pH of a solution prepared by adding 0.0500 mol of solid ammonium chloride to 100.mL of 0.150 M ammonia.

Calculate the equilibrium constant Kc for the net reaction shown below. AgI(s)+ 2NH3(aq) Ag(NH3)2+(aq)+ I-(aq) For AgI, Ksp = 8.3 * 10-17; for Ag(NH3)2+, Kf = 1.5 * 107.

The Ksp value for lead(II)chloride is 2.4 * 10-4. What is the molar solubility of lead(II)chloride?

How many moles of NaF must be dissolved in 1.00 liter of a saturated solution of PbF2 at 25°C to reduce the [Pb2+] to 1.0 * 10-6 M? The Ksp for PbF2 at 25 °C is 4.0 * 10-8.

What is the effective pH range for a sodium acetate/acetic acid buffer? (For CH3COOH, Ka = 1.8 * 10-5)

Assuming equal concentrations of conjugate base and acid, which one of the following mixtures is suitable for making a buffer solution with an optimum pH of 9.2-9.3?

Will Fe(OH)3 precipitate from a buffer solution that is 0.60 M CH3COOH and 0.10 M CH3COONa, if the solution is also made to be 0.001 M in Fe3+? For Fe(OH)3, Ksp = 6.8 * 10-36.

Describe how to prepare 500.mL of a cyanic acid (HCNO)/sodium cyanate (NaCNO)buffer having a pH of 4.80. [Ka(HCNO)= 2.0 * 10-4]

At 25 °C, the base ionization constant for NH3 is 1.8 * 10-5. Determine the hydroxide ion concentration in a 0.150 M solution of ammonia at 25 °C.

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Calculate the pH of a solution that is 0.410 M in HOCl and 0.050 M in NaOCl.[K_a(HOCl)= 3.2 * 10^-8]

The solubility product for chromium(III)fluoride is K_sp = 6.6 * 10^-11. What is the molar solubility of chromium(III)fluoride?

Will a precipitate of magnesium fluoride form when 300.mL of 1.1 * 10^-3 M MgCl₂ are added to 500.mL of 1.2 * 10^-3 M NaF? [K_sp (MgF₂)= 6.9 * 10^-9]

Will a precipitate (ppt)form when 20.0 mL of 1.1 * 10^-3 M Ba(NO₃)₂ are added to 80.0 mL of 8.4 *10^-4 M Na₂CO₃?

Will a precipitate (ppt)form when 300.mL of 2.0 * 10^-5 M AgNO₃ are added to 200.mL of 2.5 * 10^-9 M NaI? Answer yes or no, and identify the precipitate if there is one.

Calculate the concentration of chloride ions in a saturated lead(II)chloride (K_sp = 2.4 * 10^-4)solution.

Calculate the minimum concentration of Mg²⁺ that must be added to 0.10 M NaF in order to initiate a precipitate of magnesium fluoride. (For MgF₂ , K_sp = 6.9 * 10^-9.)

The molar solubility of lead(II)iodate in water is 4.0 * 10^-5 mol/L. Calculate K_sp for lead(II)iodate.

Calculate the equilibrium constant K_c for the following overall reaction: AgCl(s)+ 2CN^-(aq) Ag(CN)₂^-(aq)+ Cl^-(aq) For AgCl, K_sp = 1.6 * 10^-10; for Ag(CN)₂^-, K_f = 1.0 * 10²¹.

The concentration of Mg²⁺ in seawater is 5.0 * 10^-2M. What hydroxide concentration is needed to remove 90% of the Mg²⁺ by precipitation? (For Mg(OH)₂, K_sp = 1.2 * 10^-11.)

At 25 °C, the base ionization constant for NH₃ is 1.8 * 10^-5. Determine the pH of a solution prepared by adding 0.0500 mol of solid ammonium chloride to 100.mL of 0.150 M ammonia.

Calculate the equilibrium constant K_c for the net reaction shown below. AgI(s)+ 2NH₃(aq) Ag(NH₃)₂⁺(aq)+ I^-(aq) For AgI, K_sp = 8.3 * 10^-17; for Ag(NH₃)₂⁺, K_f = 1.5 * 10⁷.

The K_sp value for lead(II)chloride is 2.4 * 10^-4. What is the molar solubility of lead(II)chloride?

How many moles of NaF must be dissolved in 1.00 liter of a saturated solution of PbF₂ at 25°C to reduce the [Pb²⁺] to 1.0 * 10^-6 M? The K_sp for PbF₂ at 25 °C is 4.0 * 10^-8.

What is the effective pH range for a sodium acetate/acetic acid buffer? (For CH₃COOH, K_a = 1.8 * 10^-5)

Will Fe(OH)₃ precipitate from a buffer solution that is 0.60 M CH₃COOH and 0.10 M CH₃COONa, if the solution is also made to be 0.001 M in Fe³⁺? For Fe(OH)₃, K_sp = 6.8 * 10^-36.

Describe how to prepare 500.mL of a cyanic acid (HCNO)/sodium cyanate (NaCNO)buffer having a pH of 4.80. [K_a(HCNO)= 2.0 * 10^-4]

At 25 °C, the base ionization constant for NH₃ is 1.8 * 10^-5. Determine the hydroxide ion concentration in a 0.150 M solution of ammonia at 25 °C.