QUESTION 1

Equal molar amounts of nitric acid (a strong acid) and methylamine (a weak base) are combined in an aqueous solution.

The pH of the resulting solution is:

greater than 7

close to 7

less than 7

QUESTION 2

A 1.00 L aqueous solution contains 0.10 mol acetic acid and 0.10 mol sodium acetate. The initial pH is 4.74. Calculate the pH after the addition of 0.049 mol of OH-.

QUESTION 3

Using the Henderson-Hasselbalch equation, calculate the pH of a buffer solution that contains 0.96 M NH4Cl and 0.33 M NH3.

QUESTION 4

A 10.0 mL volume of 0.49 M HNO3 is combined with a 15.0 mL volume of 0.58 M NaOH. Calculate the pH.

QUESTION 5

A diprotic acid is being titrated with a strong base. A volume of 0.0500 L of 0.0750 M diprotic acid (H2A+) is combined with 0.0150 L of 0.250 M NaOH.

Ka1 for the diprotic acid is 3.6 x 10-3.

Ka2 for the diprotic acid is 4.7 x 10-7.

Calculate the pH of the solution.

QUESTION 6

A saturated solution of Ca3(PO4)2 has a concentration of Ca2+ = 5.65 x 10-7 M and a concentration of PO43- = 9.80 x 10-8 M. Calculate Ksp for Ca3(PO4)2.

Answer in exponential notation. Examples:

Scientific Notation Exponential Notation

1.00 x 10-10 1.00e-10

5.00 x 105 5.00e5

QUESTION 7

A solution is prepared by combining 0.125 L of 0.020 M Pb(NO3)2 and 0.125 L of 0.050 M PbBr2. Does a precipitate of PbBr2 form? Ksp of PbBr2= 6.6 x 10-6

Yes, a precipitate forms.

No, a precipitate does not form.

QUESTION 8

Calculate the molar solubility of MgF2 in 0.37 M NaF at 25Â°C. Ksp = 7.4 x 10-11.

Answer in exponential format.

QUESTION 9

Determine the concentration of Ag+ in a solution prepared by adding 0.10 mol AgNO3 to 1.0 L of 3.9 M NH3.

Ag+(aq) + NH3(aq) [left right double arrow] AgNH3+(aq) K1 = 2.1 x 103

AgNH3+(aq) + NH3(aq) [left right double arrow] Ag(NH3)2+(aq) K2 = 8.1 x 103

Ag+(aq) + 2 NH3(aq) [left right double arrow] Ag(NH3)2+(aq) Kf = 1.7 x 107

QUESTION 10

Determine the molar solubility of MgCO3 at 25Â°C in pure water.

Ksp = 6.8 x 10-6