Homework #7
- Page ID
- 42487
Due on Mar 4 (Friday)
Q1
Calculate the pH at the following points in a titration of 40.0 mL of 0.100 M benzoic acid (\(K_a= 6.3\times10^{−5}\)) with 0.200 M KOH.
- 10.0 mL of KOH solution added
- 15.0 mL of KOH solution added
- At the equivalence point. Verify any assumption you made.
- 21.0 mL of KOH solution added
Q2
Ethylamine, C2H5NH2, is a weak base. 250.0 mL of a 0.160 M C2H5NH2 solution is titrated with 0.500 M HCl (aq). Find the \(K_b\) value in a lecture slide. Calculate the pH at the following points.
- 30. mL of HCl solution added.
- At the halfway point.
- At the equivalence point. Verify any assumption you made.
- 90. mL of HCl solution added.
Q3
Assuming that no equilibria other than dissolution are involved, calculate the molar solubility of PbI2 (\(K_{sp}=7.1\times10^{-9}\)).
Q4
How many moles of Ag2CO3 (\(K_{\rm sp}=8.5\times 10^{-12}\)) will dissolve in 500. mL of 0.010 M (NH4)2CO3 solution?
Q5
Calculate the molar solubility of Cr(OH)3 (\(K_{\rm sp}=6.3\times 10^{-31}\)) in a buffer solution of a pH of 10.10.