Test 3 Review
REVIEW OUESTIONS TEST 3
- Calculate the pH of a solution containing 0.100 M sodium formate
and 0.180 M formic acid formic acid - A buffer is prepared by adding 5.00 g of
and 20.0 g of to enough water to form 2.50 L of solution.
a) Calculate the pH of this buffer.
b) Calculate the pH of the solution when 0.200 g of NaOH is added to 1.50 L of this buffer. - Will
precipitate from solution if the pH of a 0.050 M solution of is adjusted to 8.00 ? ( of manganese hydroxide is ) - Calculate the
in 1.0 L of a solution that contains mole of and that is 0.10 M in . for - Consider the titration of 25.0 mL of
with 0.100 M KOH . Calculate the pH of the solution after (a) addition of 10.0 mL of base, and (b) at equivalence point. ( for carbonic acid ) - A
sample of an unknown monoprotic acid is titrated with 0.112 M NaOH . The resulting titration curve is shown below. Based on this information, determine the molar mass and the Ka of the acid.
- Calculate the solubility of
in 1.0 M nitric acid solution. Is this value greater or less than the solubility in pure water? Explain. - A 0.25 mol sample of a weak acid with an unknown pKa was combined with 10.0 mL of 3.00 M KOH , and the resulting solution was diluted to 1.500 L . The measured pH of the final solution was 3.85 . What is the pKa of the weak acid?
- A solution consists of
and .
(a) Which ion will precipitate first asis added to the solution?
(b) What concentration ofis necessary to begin the precipitation of each cation? for and for - Calculate the solubility of CuX in a solution that is 0.150 M in NaCN .
for for
ANSWERS
-
- a)
b) - No precipitation occurs
-
- a)
b) - molar mass
- a)
b) greater -
- a)
will precipitate first
b)for to precipitate