Question 1

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

Accepted Answer

A)  0.00
B)  3.00
C)  3.70
D)  4.40
E)  5.00F) A) and D)
G) C) and E)

Question 2

Increasing the concentrations of the components of a buffer solution will increase the buffer capacity.

Accepted Answer

A) True 
 B)False

Question 3

Below is a representation of the sparingly soluble salt MX at equilibrium in aqueous solution.(Each circle represents 1.0 ×10-3 mol of atoms,and the volume of the box is 1.0 L.Solvent water molecules are omitted for clarity.)  -3 mol of atoms,and the volume of the box is 1.0 L.Solvent water molecules are omitted for clarity.)    What is Ksp for MX? A) 1.5 ×10-5 B) 6.0 ×10-6 C) 3.6 ×10-1 D) 1.8 ×10-3 E) 9.0 ×10-6" class="answers-bank-image d-inline" rel="preload" > What is Ksp for MX?

Accepted Answer

A)  1.5 ×10-5
B)  6.0 ×10-6
C)  3.6 ×10-1
D)  1.8 ×10-3
E)  9.0 ×10-6F) A) and B)
G) A) and E)

Question 4

Calculate the pH at the equivalence point for the titration of 50.0 mL of 0.20 M NH3 with 0.20 M HCl. [Kb(NH3) = 1.8 × 10-5]

Accepted Answer

A)  2.87
B)  4.98
C)  5.13
D)  7.00
E)  11.13F) B) and D)
G) A) and C)

Question 5

Which is more soluble in a basic solution than in pure water?

Accepted Answer

A)  AgF
B)  AgCN
C)  CO2
D)  NaCl
E)  CH3COOKF) B) and D)
G) C) and D)

Question 6

Write the ion product expression for calcium phosphate,Ca3(P O4) 2.

Accepted Answer

A)   3(P O4) 2. 
A)     
B)     
C)     
D)     
E)  (3 × [Ca2+]) (2 × [P O43- ]" class="answers-bank-image d-inline" rel="preload" >
B)   3(P O4) 2. 
A)     
B)     
C)     
D)     
E)  (3 × [Ca2+]) (2 × [P O43- ]" class="answers-bank-image d-inline" rel="preload" >
C)   3(P O4) 2. 
A)     
B)     
C)     
D)     
E)  (3 × [Ca2+]) (2 × [P O43- ]" class="answers-bank-image d-inline" rel="preload" >
D)   3(P O4) 2. 
A)     
B)     
C)     
D)     
E)  (3 × [Ca2+]) (2 × [P O43- ]" class="answers-bank-image d-inline" rel="preload" >
E)  (3 × [Ca2+]) (2 × [P O43- ]F) All of the above
G) A) and B)

Question 7

What name is given to a solution that contains a weak acid and its conjugate base?

Accepted Answer

The answer of What name is given to a solution...

Question 8

A 25.0-mL sample of 0.10 M C2H5NH2 (ethylamine) is titrated with 0.15 M HCl.What is the pH of the solution after 9.00 mL of acid have been added to the amine? [Kb(C2H5NH2) = 6.5 × 10-4]

Accepted Answer

A)  11.08
B)  10.74
C)  10.81
D)  10.55
E)  10.49F) None of the above
G) All of the above

Question 9

Which one of the following is the best representation of the titration curve which will be obtained in the titration of a weak diprotic acid H2A (0.10 M) with a strong base of the same concentration?

Accepted Answer

A)   2A (0.10 M) with a strong base of the same concentration? 
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
B)   2A (0.10 M) with a strong base of the same concentration? 
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
C)   2A (0.10 M) with a strong base of the same concentration? 
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
D)   2A (0.10 M) with a strong base of the same concentration? 
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
E)   2A (0.10 M) with a strong base of the same concentration? 
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >F) C) and D)
G) C) and E)

Exam 17: Acid-Base Equilibria and Solubility Equilibria

Calculate the pH at the equivalence point for the titration of 50.0 mL of 0.20 M NH₃ with 0.20 M HCl. [Kb(NH₃) = 1.8 × 10^-5]

Correct Answer
verified

Which one of the following is the best representation of the titration curve which will be obtained in the titration of a weak diprotic acid H₂A (0.10 M) with a strong base of the same concentration?

Correct Answer
verified

Increasing the concentrations of the components of a buffer solution will increase the buffer capacity.

Correct Answer
verified

What name is given to a solution that contains a weak acid and its conjugate base?

Correct Answer
verified

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

Correct Answer
verified

Write the ion product expression for calcium phosphate,Ca₃(P O₄) ₂.

Correct Answer
verified

A 25.0-mL sample of 0.10 M C₂H₅NH₂ (ethylamine) is titrated with 0.15 M HCl.What is the pH of the solution after 9.00 mL of acid have been added to the amine? [K_b(C₂H₅NH₂) = 6.5 × 10^-4]

Correct Answer
verified

Which is more soluble in a basic solution than in pure water?

Correct Answer
verified

Below is a representation of the sparingly soluble salt MX at equilibrium in aqueous solution.(Each circle represents 1.0 ×10^-3 mol of atoms,and the volume of the box is 1.0 L.Solvent water molecules are omitted for clarity.) What is K_sp for MX?

Correct Answer
verified

Exam 17: Acid-Base Equilibria and Solubility Equilibria

Calculate the pH at the equivalence point for the titration of 50.0 mL of 0.20 M NH3 with 0.20 M HCl. [Kb(NH3) = 1.8 × 10-5]

Correct AnswerverifiedShow Answer

Which one of the following is the best representation of the titration curve which will be obtained in the titration of a weak diprotic acid H2A (0.10 M) with a strong base of the same concentration?

Correct AnswerverifiedShow Answer

Increasing the concentrations of the components of a buffer solution will increase the buffer capacity.

Correct AnswerverifiedShow Answer

What name is given to a solution that contains a weak acid and its conjugate base?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Write the ion product expression for calcium phosphate,Ca3(P O4) 2.

Correct AnswerverifiedShow Answer

A 25.0-mL sample of 0.10 M C2H5NH2 (ethylamine) is titrated with 0.15 M HCl.What is the pH of the solution after 9.00 mL of acid have been added to the amine? [Kb(C2H5NH2) = 6.5 × 10-4]

Correct AnswerverifiedShow Answer

Which is more soluble in a basic solution than in pure water?

Correct AnswerverifiedShow Answer

Below is a representation of the sparingly soluble salt MX at equilibrium in aqueous solution.(Each circle represents 1.0 ×10-3 mol of atoms,and the volume of the box is 1.0 L.Solvent water molecules are omitted for clarity.) What is Ksp for MX?

Correct AnswerverifiedShow Answer

Calculate the pH at the equivalence point for the titration of 50.0 mL of 0.20 M NH₃ with 0.20 M HCl. [Kb(NH₃) = 1.8 × 10^-5]

Correct Answer
verified

Which one of the following is the best representation of the titration curve which will be obtained in the titration of a weak diprotic acid H₂A (0.10 M) with a strong base of the same concentration?

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

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

Correct Answer
verified

Write the ion product expression for calcium phosphate,Ca₃(P O₄) ₂.

Correct Answer
verified

A 25.0-mL sample of 0.10 M C₂H₅NH₂ (ethylamine) is titrated with 0.15 M HCl.What is the pH of the solution after 9.00 mL of acid have been added to the amine? [K_b(C₂H₅NH₂) = 6.5 × 10^-4]

Correct Answer
verified

Correct Answer
verified

Below is a representation of the sparingly soluble salt MX at equilibrium in aqueous solution.(Each circle represents 1.0 ×10^-3 mol of atoms,and the volume of the box is 1.0 L.Solvent water molecules are omitted for clarity.) What is K_sp for MX?

Correct Answer
verified