Question 1

Calculate the pH of a solution formed by mixing 300.0 mL of 0.30 M HClO with 150.0 mL of 0.20 M LiClO.The Ka for HClO is 2.9 × 10-8.

Accepted Answer

A)  5.99 
B)  8.01 
C)  7.54 
D)  7.06 
E)  6.46 
A)  5.99 
B)  8.01 
C)  7.54 
D)  7.06 
E)  6.46

Question 2

Give the mathematical relationship for an unsaturated solution in comparing Q with Ksp.

Accepted Answer

A)  Q > Ksp 
B)  Q sp 
C)  Q = Ksp 
D)  Q ≠ Ksp 
E)  none of the above 
A)  Q > Ksp 
B)  Q sp 
C)  Q = Ksp 
D)  Q ≠ Ksp 
E)  none of the above

Question 3

What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M methylamine,CH3NH2,with 20.00 mL of 0.10 M methylammonium chloride,CH3NH3Cl? Assume that the volume of the solutions are additive and that Kb = 3.70 × 10-4 for methylamine.

Accepted Answer

A)  10.17 
B)  10.57 
C)  10.97 
D)  11.78 
A)  10.17 
B)  10.57 
C)  10.97 
D)  11.78

Question 4

A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M NaOH.Determine the pH of the solution after the addition of 200.0 mL of NaOH.The Ka of HF is 3.5 × 10-4.

Accepted Answer

A)  9.62 
B)  7.00 
C)  3.46 
D)  10.54 
E)  8.14 
A)  9.62 
B)  7.00 
C)  3.46 
D)  10.54 
E)  8.14

Question 5

A solution containing CaCl2 is mixed with a solution of Li2C2O4 to form a solution that is 3.5 × 10-4 M in calcium ion and 2.33 × 10-4 M in oxalate ion.What will happen once these solutions are mixed? Ksp (CaC2O4)= 2.3 × 10-9.

Accepted Answer

A)  Nothing will happen since both calcium chloride and lithium oxalate are soluble compounds. 
B)  Nothing will happen Ksp > Q for all possible precipitants. 
C)  A precipitate will form as calcium oxalate is not soluble to any extent. 
D)  A precipitate will form since Q > Ksp for calcium oxalate. 
E)  There is not enough information to determine. 
A)  Nothing will happen since both calcium chloride and lithium oxalate are soluble compounds. 
B)  Nothing will happen Ksp > Q for all possible precipitants. 
C)  A precipitate will form as calcium oxalate is not soluble to any extent. 
D)  A precipitate will form since Q > Ksp for calcium oxalate. 
E)  There is not enough information to determine.

Question 6

Which of the following acids (listed with pKa values)and their conjugate base would form a buffer with a pH of 8.10?

Accepted Answer

A)  HC2H3O2, pKa = 4.74 
B)  H2SO3, pKa = 1.77 
C)  HClO, pKa = 7.54 
D)  HIO, pKa = 10.64 
E)  HNO2, pKa = 3.34 
A)  HC2H3O2, pKa = 4.74 
B)  H2SO3, pKa = 1.77 
C)  HClO, pKa = 7.54 
D)  HIO, pKa = 10.64 
E)  HNO2, pKa = 3.34

Question 7

A 140.0 mL sample of 0.10 M Ba(OH)2 is titrated with 0.10 M HCl.Determine the pH of the solution after the addition of 560.0 mL HCl.

Accepted Answer

A)  1.00 
B)  1.40 
C)  1.22 
D)  1.30 
E)  2.11 
A)  1.00 
B)  1.40 
C)  1.22 
D)  1.30 
E)  2.11

Calculate the pH of a solution formed by mixing 300.0 mL of 0.30 M HClO with 150.0 mL of 0.20 M LiClO.The K_a for HClO is 2.9 × 10^-8.

Give the mathematical relationship for an unsaturated solution in comparing Q with K_sp.

What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M methylamine,CH₃NH₂,with 20.00 mL of 0.10 M methylammonium chloride,CH₃NH₃Cl? Assume that the volume of the solutions are additive and that K_b = 3.70 × 10^-4 for methylamine.

A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M NaOH.Determine the pH of the solution after the addition of 200.0 mL of NaOH.The K_a of HF is 3.5 × 10^-4.

A solution containing CaCl₂ is mixed with a solution of Li₂C₂O₄ to form a solution that is 3.5 × 10^-4 M in calcium ion and 2.33 × 10^-4M in oxalate ion.What will happen once these solutions are mixed? K_sp (CaC₂O₄)= 2.3 × 10^-9.

Which of the following acids (listed with pK_a values)and their conjugate base would form a buffer with a pH of 8.10?

A 140.0 mL sample of 0.10 M Ba(OH)₂ is titrated with 0.10 M HCl.Determine the pH of the solution after the addition of 560.0 mL HCl.

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Exam 17: Aqueous Ionic Equilibrium