Question 1

Which of the following is an exact or approximate value of the pH at the equivalence point of a titration of a strong acid with a strong base?

Accepted Answer

A) 14.0 
B) 7.0 
C) 3.5 
D) 1.0 
E) 0.0 
A) 14.0 
B) 7.0 
C) 3.5 
D) 1.0 
E) 0.0 B

Question 2

What is 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 E

Question 3

Which cation would form an insoluble chloride when reacted with HCl?

Accepted Answer

A) Na+ 
B) Ag+ 
C) B3+ 
D) Ca2+ 
E) Cs+ 
A) Na+ 
B) Ag+ 
C) B3+ 
D) Ca2+ 
E) Cs+ B

Question 4

Which pair of substances is capable of forming a buffer in aqueous solution?

Accepted Answer

A) H3PO4,Na3PO3 
B) HNO3,NaNO3 
C) HCl,NaCl 
D) H2CO3,NaNO2 
E) CH3COOH,CH3COONa 
A) H3PO4,Na3PO3 
B) HNO3,NaNO3 
C) HCl,NaCl 
D) H2CO3,NaNO2 
E) CH3COOH,CH3COONa

Question 5

A 50.00-mL solution of 0.10 M HNO2 is titrated with a 0.10 M KOH solution.After 25.00 mL of the KOH solution is added,what is the pH in the titration flask?
[Ka(HNO2)= 4.5 × 10-4]

Accepted Answer

A) 2.17 
B) 3.35 
C) 2.41 
D) 1.48 
E) 7.00 
A) 2.17 
B) 3.35 
C) 2.41 
D) 1.48 
E) 7.00

Question 6

Which is more soluble in an acidic solution than in pure water?

Accepted Answer

A) CuI 
B) PbCl2 
C) Ca3(PO4)2 
D) NaNO3 
E) NaBr 
A) CuI 
B) PbCl2 
C) Ca3(PO4)2 
D) NaNO3 
E) NaBr

Question 7

What is the [H3O+] in a solution that consists of 1.5 M NH3 and 2.5 M NH4Cl? Kb = 1.8 × 10-5

Accepted Answer

A) 1.1 × 10-5 M 
B) 3.0 × 10-6 M 
C) 3.3 × 10-9 M 
D) 5.6 × 10-10 M 
E) 9.3 × 10-10 M 
A) 1.1 × 10-5 M 
B) 3.0 × 10-6 M 
C) 3.3 × 10-9 M 
D) 5.6 × 10-10 M 
E) 9.3 × 10-10 M

Question 8

Which compound has the highest solubility in pure water?

Accepted Answer

A) Ag2C2O4,Ksp = 1.0 × 10-11 
B) PbCl2,Ksp = 1.7 × 10-5 
C) CaSO4,Ksp = 2.4 × 10-5 
D) Ca3(PO4)2,Ksp = 1.2 × 10-26 
E) MgF2,Ksp = 6.9 × 10-9 
A) Ag2C2O4,Ksp = 1.0 × 10-11 
B) PbCl2,Ksp = 1.7 × 10-5 
C) CaSO4,Ksp = 2.4 × 10-5 
D) Ca3(PO4)2,Ksp = 1.2 × 10-26 
E) MgF2,Ksp = 6.9 × 10-9

Question 9

A buffer is prepared by adding 150 mL of 1.0 M NaOH to 250 mL of 1.0 M NaH2PO4.How many moles of HCl must be added to this buffer solution to change the pH by 0.18 units?

Accepted Answer

A) 0.025 mol HCl 
B) 0.063 mol HCl 
C) 0.082 mol HCl 
D) 0.50 mol HCl 
E) 1.0 mol HCl 
A) 0.025 mol HCl 
B) 0.063 mol HCl 
C) 0.082 mol HCl 
D) 0.50 mol HCl 
E) 1.0 mol HCl

Question 10

What is the pH at the equivalence point in the titration of 100 mL of 0.10 M HCl with 0.10 M NaOH?

Accepted Answer

A) 1.0 
B) 6.0 
C) 7.0 
D) 8.0 
E) 13.0 
A) 1.0 
B) 6.0 
C) 7.0 
D) 8.0 
E) 13.0

Question 11

mL of 3.0 M NH3?
(Kf for Ag(NH3)2+ is 1.5 × 107; Ksp (AgCl)= 1.6 × 10-10)

Accepted Answer

Question 12

A(n)________________ is an ion containing a central metal cation bonded to one or more molecules or ions.

Accepted Answer

The answer of A(n)________________ is an ion containing a central...

Question 13

A solution is prepared by mixing 50.0 mL of 0.50 M Cu(NO3)2 with 50.0 mL of 0.50 M Co(NO3)2. Sodium hydroxide is slowly added to the mixture.Which precipitates first?
[Ksp(Cu(OH)2)= 2.2 × 10-20,Ksp(Co(OH)2)= 1.3 × 10-15]

Accepted Answer

A) Co(OH)2 
B) Co(NO3)2 
C) Cu(NO3)2 
D) Cu(OH)2 
E) No precipitate is formed. 
A) Co(OH)2 
B) Co(NO3)2 
C) Cu(NO3)2 
D) Cu(OH)2 
E) No precipitate is formed.

Question 14

For a conjugate acid-base pair,Kw = Ka /Kb

Accepted Answer

A) True 
 B)False

Question 15

You have 500.0 mL of a buffer solution containing 0.30 M acetic acid (CH3COOH)and 0.20 M sodium acetate (CH3COONa).What will the pH of this solution be after the addition of 20.0 mL of 1.00 M NaOH solution?
[Ka(CH3COOH)= 1.8 × 10-5]

Accepted Answer

A) 4.65 
B) 4.71 
C) 4.56 
D) 4.84 
E) 5.07 
A) 4.65 
B) 4.71 
C) 4.56 
D) 4.84 
E) 5.07

Question 16

Which pair of substances could form a buffered aqueous solution?

Accepted Answer

A) HCl,NaCl 
B) HNO3,NaNO3 
C) H3PO4,Na H2PO4 
D) H SO4,CH3COOH 
E) NH3,NaOH 
A) HCl,NaCl 
B) HNO3,NaNO3 
C) H3PO4,Na H2PO4 
D) H SO4,CH3COOH 
E) NH3,NaOH

Question 17

The solubility of lead(II)chloride is 0.45 g/100 mL of solution.What is the Ksp of PbCl2?

Accepted Answer

A) 4.9 × 10-2 
B) 1.7 × 10-5 
C) 8.5 × 10-6 
D) 4.2 × 10-6 
E) 2.6 × 10-4 
A) 4.9 × 10-2 
B) 1.7 × 10-5 
C) 8.5 × 10-6 
D) 4.2 × 10-6 
E) 2.6 × 10-4

Question 18

Which is the best choice for preparing a buffer with a pH of 3.5?

Accepted Answer

A) C5H5O5COOH,Ka = 4.0 × 10-6 
B) HOC6H4OCOOH,Ka = 1.0 × 10-3 
C) HBrO,Ka = 2.3 × 10-9 
D) C6H4(COOH)2,Ka = 2.9 × 10-4 
E) CH3COOH,Ka = 1.8 ×10-5 
A) C5H5O5COOH,Ka = 4.0 × 10-6 
B) HOC6H4OCOOH,Ka = 1.0 × 10-3 
C) HBrO,Ka = 2.3 × 10-9 
D) C6H4(COOH)2,Ka = 2.9 × 10-4 
E) CH3COOH,Ka = 1.8 ×10-5

Question 19

The amount of strong acid added to a buffer solution cannot exceed the original amount of conjugate base present in order for the buffer to still work.

Accepted Answer

A) True 
 B)False

Question 20

What is the name of the principle of selective precipitation used to identify the types of ions present in a solution?

Accepted Answer

A) Ionization 
B) Selective ion precipitation 
C) Selective ion typing 
D) Limited precipitation 
E) Qualitative analysis 
A) Ionization 
B) Selective ion precipitation 
C) Selective ion typing 
D) Limited precipitation 
E) Qualitative analysis

Exam 17: Acid-Base Equilibria and Solubility Equilibria

Which of the following is an exact or approximate value of the pH at the equivalence point of a titration of a strong acid with a strong base?

What is 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]

Which cation would form an insoluble chloride when reacted with HCl?

Which pair of substances is capable of forming a buffer in aqueous solution?

A 50.00-mL solution of 0.10 M HNO2 is titrated with a 0.10 M KOH solution.After 25.00 mL of the KOH solution is added,what is the pH in the titration flask? [Ka(HNO2)= 4.5 × 10-4]

Which is more soluble in an acidic solution than in pure water?

What is the [H3O+] in a solution that consists of 1.5 M NH3 and 2.5 M NH4Cl? Kb = 1.8 × 10-5

Which compound has the highest solubility in pure water?

A buffer is prepared by adding 150 mL of 1.0 M NaOH to 250 mL of 1.0 M NaH2PO4.How many moles of HCl must be added to this buffer solution to change the pH by 0.18 units?

What is the pH at the equivalence point in the titration of 100 mL of 0.10 M HCl with 0.10 M NaOH?

mL of 3.0 M NH3? (Kf for Ag(NH3)2+ is 1.5 × 107; Ksp (AgCl)= 1.6 × 10-10)

A(n)________________ is an ion containing a central metal cation bonded to one or more molecules or ions.

A solution is prepared by mixing 50.0 mL of 0.50 M Cu(NO3)2 with 50.0 mL of 0.50 M Co(NO3)2. Sodium hydroxide is slowly added to the mixture.Which precipitates first? [Ksp(Cu(OH)2)= 2.2 × 10-20,Ksp(Co(OH)2)= 1.3 × 10-15]

For a conjugate acid-base pair,Kw = Ka /Kb

You have 500.0 mL of a buffer solution containing 0.30 M acetic acid (CH3COOH)and 0.20 M sodium acetate (CH3COONa).What will the pH of this solution be after the addition of 20.0 mL of 1.00 M NaOH solution? [Ka(CH3COOH)= 1.8 × 10-5]

Which pair of substances could form a buffered aqueous solution?

The solubility of lead(II)chloride is 0.45 g/100 mL of solution.What is the Ksp of PbCl2?

Which is the best choice for preparing a buffer with a pH of 3.5?

The amount of strong acid added to a buffer solution cannot exceed the original amount of conjugate base present in order for the buffer to still work.

What is the name of the principle of selective precipitation used to identify the types of ions present in a solution?

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What is 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]

A 50.00-mL solution of 0.10 M HNO₂ is titrated with a 0.10 M KOH solution.After 25.00 mL of the KOH solution is added,what is the pH in the titration flask? [K_a(HNO₂)= 4.5 × 10^-4]

What is the [H₃O⁺] in a solution that consists of 1.5 M NH₃ and 2.5 M NH₄Cl? K_b = 1.8 × 10^-5

A buffer is prepared by adding 150 mL of 1.0 M NaOH to 250 mL of 1.0 M NaH₂PO₄.How many moles of HCl must be added to this buffer solution to change the pH by 0.18 units?

mL of 3.0 M NH₃? (Kf for Ag(NH₃)₂⁺ is 1.5 × 10⁷; K_sp (AgCl)= 1.6 × 10^-10)

A solution is prepared by mixing 50.0 mL of 0.50 M Cu(NO₃)₂ with 50.0 mL of 0.50 M Co(NO₃)₂. Sodium hydroxide is slowly added to the mixture.Which precipitates first? [K_sp(Cu(OH)₂)= 2.2 × 10^-20,K_sp(Co(OH)₂)= 1.3 × 10^-15]

For a conjugate acid-base pair,K_w = K_a /K_b

You have 500.0 mL of a buffer solution containing 0.30 M acetic acid (CH₃COOH)and 0.20 M sodium acetate (CH₃COONa).What will the pH of this solution be after the addition of 20.0 mL of 1.00 M NaOH solution? [K_a(CH₃COOH)= 1.8 × 10^-5]

The solubility of lead(II)chloride is 0.45 g/100 mL of solution.What is the K_sp of PbCl₂?