Question 1

For which type of titration will the pH be basic at the equivalence point?

Accepted Answer

A) Strong acid vs.strong base. 
B) Strong acid vs.weak base. 
C) Weak acid vs.strong base. 
D) All of the above. 
E) None of the above. 
A) Strong acid vs.strong base. 
B) Strong acid vs.weak base. 
C) Weak acid vs.strong base. 
D) All of the above. 
E) None of the above.

Question 2

What volume of 0.200 M potassium hydroxide should be added to 300.mL of 0.150 M propanoic acid (C2H5COOH)to obtain a solution with a pH of 5.25? [Ka(C2H5COOH)= 1.34 × 10-5]

Accepted Answer

A) 32 mL 
B) 210 mL 
C) 160 mL 
D) 65 mL 
E) 13 mL 
A) 32 mL 
B) 210 mL 
C) 160 mL 
D) 65 mL 
E) 13 mL

Question 3

Calculate the pH of a buffer solution prepared by dissolving 0.20 mole of cyanic acid (HCNO)and 0.80 mole of sodium cyanate (NaCNO)in enough water to make 1.0 liter of solution. [Ka(HCNO)= 2.0 × 10-4]

Accepted Answer

A) 0.97 
B) 3.10 
C) 4.40 
D) 3.70 
E) 4.30 
A) 0.97 
B) 3.10 
C) 4.40 
D) 3.70 
E) 4.30

Question 4

Bromothymol blue is a common acid-base indicator.It has a Ka equal to 1.6 × 10-7.Its un-ionized form is yellow and its conjugate base is blue.What color would a solution have at pH = 5.8?

Accepted Answer

Question 5

What mass of sodium fluoride must be added to 250.mL of a 0.100 M HF solution to give a buffer solution having a pH of 3.50? [Ka(HF)= 7.1 × 10-4]

Accepted Answer

A) 0.49 g 
B) 1.5 g 
C) 3.4 g 
D) 2.3 g 
E) 0.75 g 
A) 0.49 g 
B) 1.5 g 
C) 3.4 g 
D) 2.3 g 
E) 0.75 g

Question 6

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 7

Starting with 0.250L of a buffer solution containing 0.250 M benzoic acid (C6H5COOH)and 0.20 M sodium benzoate (C6H5COONa), what will the pH of the solution be after the addition of 25.0 mL of 0.100M HCl? (Ka (C6H5COOH)= 6.5 x 10-5)

Accepted Answer

A) 4.19 
B) 4.10 
C) 4.28 
D) 4.05 
E) 3.78 
A) 4.19 
B) 4.10 
C) 4.28 
D) 4.05 
E) 3.78

Question 8

The pH of a solution that is 0.20 M CH3COOH and 0.20 M CH3COONa should be higher than the pH of a 0.20 M CH3COOH solution.

Accepted Answer

A) True 
 B)False

Question 9

Calculate the molar solubility of lead (II)fluoride (Ksp (PbF2 = 4.1 x 10-8))

Accepted Answer

Question 10

Starting with 0.750L of a buffer solution containing 0.30 M benzoic acid (C6H5COOH)and 0.35 M sodium benzoate (C6H5COONa), what will the pH of the solution be after the addition of 340.0 mL of 0.350M HCl? (Ka (C6H5COOH)= 6.5 x 10-5)

Accepted Answer

A) 4.19 
B) 4.25 
C) 3.81 
D) 0.45 
E) 6.54 
A) 4.19 
B) 4.25 
C) 3.81 
D) 0.45 
E) 6.54

Question 11

Calculate the molar solubility of Mg(OH)2 in a solution with pH = 12.20. (Ksp (Mg(OH)2 = 1.2 x 10-11)

Accepted Answer

A) 4.8 x 10-8 M 
B) 7.6 x 10-10 M 
C) 3.5 x 10-6 M 
D) 1.4 x 10-4 M 
E) 2.4 x 10-6 M 
A) 4.8 x 10-8 M 
B) 7.6 x 10-10 M 
C) 3.5 x 10-6 M 
D) 1.4 x 10-4 M 
E) 2.4 x 10-6 M

Question 12

Will a precipitate (ppt)form when 300.mL of 5.0 × 10-5 M AgNO3 are added to 200.mL of 2.5 × 10-7 M NaBr? 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 AgBr(s). 
C) Yes, the ppt is NaBr(s). 
D) Yes, the ppt is NaNO3(s). 
E) No, a precipitate will not form. 
A) Yes, the ppt is AgNO3(s). 
B) Yes, the ppt is AgBr(s). 
C) Yes, the ppt is NaBr(s). 
D) Yes, the ppt is NaNO3(s). 
E) No, a precipitate will not form.

Question 13

In which one of the following solutions will acetic acid have the greatest percent ionization?

Accepted Answer

A) 0.1 M CH3COOH 
B) 0.1 M CH3COOH dissolved in 1.0 M HCl 
C) 0.1 M CH3COOH plus 0.1 M CH3COONa 
D) 0.1 M CH3COOH plus 0.2 M CH3COONa 
A) 0.1 M CH3COOH 
B) 0.1 M CH3COOH dissolved in 1.0 M HCl 
C) 0.1 M CH3COOH plus 0.1 M CH3COONa 
D) 0.1 M CH3COOH plus 0.2 M CH3COONa

Question 14

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 15

Which of the following compounds is more soluble in acidic solution than in pure neutral water?

Accepted Answer

A) BaCO3 
B) CuI 
C) PbCl2 
D) AgBr 
E) NH4NO3 
A) BaCO3 
B) CuI 
C) PbCl2 
D) AgBr 
E) NH4NO3

Question 16

What is the pH at the equivalence point in the titration of 100 mL of 0.10 M HCN (Ka = 4.9 × 10-10)with 0.10 M NaOH?

Accepted Answer

A) 3.0 
B) 6.0 
C) 7.0 
D) 11.0 
E) 12.0 
A) 3.0 
B) 6.0 
C) 7.0 
D) 11.0 
E) 12.0

Question 17

A titration of an acid and base to the equivalence point results in a noticeably acidic solution.It is likely this titration involves

Accepted Answer

A) a strong acid and a weak base. 
B) a weak acid and a strong base. 
C) a weak acid and a weak base (where Ka equals Kb). 
D) a strong acid and a strong base. 
A) a strong acid and a weak base. 
B) a weak acid and a strong base. 
C) a weak acid and a weak base (where Ka equals Kb). 
D) a strong acid and a strong base.

Question 18

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

Question 19

Calculate the silver ion concentration in a saturated solution of silver(I)carbonate (Ksp = 8.1 × 10-12).

Accepted Answer

A) 5.0 × 10-5 M 
B) 2.5 × 10-4 M 
C) 1.3 × 10-4 M 
D) 2.0 × 10-4 M 
E) 8.1 × 10-4 M 
A) 5.0 × 10-5 M 
B) 2.5 × 10-4 M 
C) 1.3 × 10-4 M 
D) 2.0 × 10-4 M 
E) 8.1 × 10-4 M

Question 20

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.

Exam 16: Acid-Base Equilibria and Solubility Equilibria

For which type of titration will the pH be basic at the equivalence point?

What volume of 0.200 M potassium hydroxide should be added to 300.mL of 0.150 M propanoic acid (C2H5COOH)to obtain a solution with a pH of 5.25? [Ka(C2H5COOH)= 1.34 × 10-5]

Calculate the pH of a buffer solution prepared by dissolving 0.20 mole of cyanic acid (HCNO)and 0.80 mole of sodium cyanate (NaCNO)in enough water to make 1.0 liter of solution. [Ka(HCNO)= 2.0 × 10-4]

Bromothymol blue is a common acid-base indicator.It has a Ka equal to 1.6 × 10-7.Its un-ionized form is yellow and its conjugate base is blue.What color would a solution have at pH = 5.8?

What mass of sodium fluoride must be added to 250.mL of a 0.100 M HF solution to give a buffer solution having a pH of 3.50? [Ka(HF)= 7.1 × 10-4]

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

Starting with 0.250L of a buffer solution containing 0.250 M benzoic acid (C6H5COOH)and 0.20 M sodium benzoate (C6H5COONa), what will the pH of the solution be after the addition of 25.0 mL of 0.100M HCl? (Ka (C6H5COOH)= 6.5 x 10-5)

The pH of a solution that is 0.20 M CH3COOH and 0.20 M CH3COONa should be higher than the pH of a 0.20 M CH3COOH solution.

Calculate the molar solubility of lead (II)fluoride (Ksp (PbF2 = 4.1 x 10-8))

Starting with 0.750L of a buffer solution containing 0.30 M benzoic acid (C6H5COOH)and 0.35 M sodium benzoate (C6H5COONa), what will the pH of the solution be after the addition of 340.0 mL of 0.350M HCl? (Ka (C6H5COOH)= 6.5 x 10-5)

Calculate the molar solubility of Mg(OH)2 in a solution with pH = 12.20. (Ksp (Mg(OH)2 = 1.2 x 10-11)

Will a precipitate (ppt)form when 300.mL of 5.0 × 10-5 M AgNO3 are added to 200.mL of 2.5 × 10-7 M NaBr? Answer yes or no, and identify the precipitate if there is one.

In which one of the following solutions will acetic acid have the greatest percent ionization?

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]

Which of the following compounds is more soluble in acidic solution than in pure neutral water?

What is the pH at the equivalence point in the titration of 100 mL of 0.10 M HCN (Ka = 4.9 × 10-10)with 0.10 M NaOH?

A titration of an acid and base to the equivalence point results in a noticeably acidic solution.It is likely this titration involves

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.

Calculate the silver ion concentration in a saturated solution of silver(I)carbonate (Ksp = 8.1 × 10-12).

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?

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What volume of 0.200 M potassium hydroxide should be added to 300.mL of 0.150 M propanoic acid (C₂H₅COOH)to obtain a solution with a pH of 5.25? [K_a(C₂H₅COOH)= 1.34 × 10^-5]

Calculate the pH of a buffer solution prepared by dissolving 0.20 mole of cyanic acid (HCNO)and 0.80 mole of sodium cyanate (NaCNO)in enough water to make 1.0 liter of solution. [K_a(HCNO)= 2.0 × 10^-4]

Bromothymol blue is a common acid-base indicator.It has a K_a equal to 1.6 × 10^-7.Its un-ionized form is yellow and its conjugate base is blue.What color would a solution have at pH = 5.8?

What mass of sodium fluoride must be added to 250.mL of a 0.100 M HF solution to give a buffer solution having a pH of 3.50? [K_a(HF)= 7.1 × 10^-4]

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

Starting with 0.250L of a buffer solution containing 0.250 M benzoic acid (C₆H₅COOH)and 0.20 M sodium benzoate (C₆H₅COONa), what will the pH of the solution be after the addition of 25.0 mL of 0.100M HCl? (K_a (C₆H₅COOH)= 6.5 x 10^-5)

The pH of a solution that is 0.20 M CH₃COOH and 0.20 M CH₃COONa should be higher than the pH of a 0.20 M CH₃COOH solution.

Calculate the molar solubility of lead (II)fluoride (K_sp (PbF₂ = 4.1 x 10^-8))

Starting with 0.750L of a buffer solution containing 0.30 M benzoic acid (C₆H₅COOH)and 0.35 M sodium benzoate (C₆H₅COONa), what will the pH of the solution be after the addition of 340.0 mL of 0.350M HCl? (K_a (C₆H₅COOH)= 6.5 x 10^-5)

Calculate the molar solubility of Mg(OH)₂ in a solution with pH = 12.20. (K_sp (Mg(OH)₂ = 1.2 x 10^-11)

Will a precipitate (ppt)form when 300.mL of 5.0 × 10^-5 M AgNO₃ are added to 200.mL of 2.5 × 10^-7 M NaBr? Answer yes or no, and identify the precipitate if there is one.

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]

What is the pH at the equivalence point in the titration of 100 mL of 0.10 M HCN (K_a = 4.9 × 10^-10)with 0.10 M NaOH?

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.

Calculate the silver ion concentration in a saturated solution of silver(I)carbonate (K_sp = 8.1 × 10^-12).

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?