Question 1

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.

Question 2

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

Question 3

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

Question 4

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.

Question 5

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

Question 6

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 7

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.

Question 8

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 9

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

Question 10

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

Question 11

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

Question 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?

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.

Question 13

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 14

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

Question 15

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

Question 16

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

Question 17

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 18

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

Question 19

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

Question 20

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

Accepted Answer

Exam 16: Acid-Base Equilibria and Solubility Equilibria

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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]

Correct AnswerverifiedShow Answer

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?

Correct AnswerverifiedShow Answer

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)

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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.

Correct AnswerverifiedShow Answer

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)

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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?

Correct AnswerverifiedShow Answer

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

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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]

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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.

Correct AnswerverifiedShow Answer

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]

Correct AnswerverifiedDissolve amounts of the two compounds eq...View AnswerShow Answer

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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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]

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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?

Correct AnswerverifiedShow Answer

Correct Answer
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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]

Correct Answer
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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?

Correct Answer
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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)

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

Correct Answer
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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.

Correct Answer
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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)

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

Correct Answer
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Correct Answer
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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?

Correct Answer
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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)

Correct Answer
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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]

Correct Answer
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Correct Answer
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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.

Correct Answer
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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]

Correct Answer
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Dissolve amounts of the two compounds eq...
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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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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]

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

Correct Answer
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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?

Correct Answer
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