General Chemistry 2: Acids and Bases

Find the concentration of HS##^-##, S##^{2-}## and H##_3##O##^+## in a 0.075 M solution of H##_2##S
H##_2##S + H##_2##O ##\longrightarrow## HS##^-## + H##_3##O##^+##, K##_{a1}## = 1.0 x 10##^{-7}##
HS##^-## + H##_2##O ##\longrightarrow## S##^2-## + H##_3##O##^+##, K##_{a2}## = 1.0 x 10##^{-19}##

Calculate the pH and concentration of all species of a 3.0 M solution of phosphoric acid, H##_3##PO##_4##

What is the pH of a 0.1 M sulfuric acid solution? (did you know sulphuric is an alternative spelling?)
H##_2##SO##_4## + H##_2##O ##\longrightarrow## HSO##_4^-## + H##_3##O##^+##, K##_{a1}## = 1.0 x 10##^{3}##
HSO##_4^-## + H##_2##O ##\longrightarrow## SO##_4^{2-}## + H##_3##O##^+##, K##_{a2}## = 1.2 x 10##^{-2}##

Calculate the pH of a 5.0 M H##_3##PO##_4## solution and the equilibrium concentrations of the species H##_3##PO##_4##, H##_2##PO##_4^-##, HPO##_4^{2-}##, and PO##_4^{3-}##.

Find the equilibrium concentrations of the species H##_2##SO##_4##, HSO##_4^-##, SO##_4^{2-}##, and H##^{+}## given a 1.0 M solution of H##_2##SO##_4##.

Find the pH of the buffer solution consisting of 0.60 M HF and 1.0 M KF (K##_a## of HF = 7.2 x 10##^{-4}##)

A buffer solution consisting of 0.60 M HF and 1.0 M KF (Ka of HF = 7.2 x 10##^-4##) is titrated by 0.1 mol NaOH. After the NaOH is added, there is 1 L of solution. Find the pH of the solution.

A buffer solution consisting of 0.60 M HF and 1.0 M KF (Ka of HF = 7.2 x 10##^-4##) is titrated by 0.2 mol HCl. After the HCl is added, there is 1 L of solution. Find the pH of the solution.

Find the pH of the buffer solution consisting of 0.100 M HONH##_2## and 0.100 M HONH##_3^+## (K##_b## of HONH##_2## = 1.1 x 10##^{-8}##), after .02 moles HCl is added to the buffer solution? (assume the final volume of the solution is 1 L)

10.00 mL of an unknown H##_2##CO##_3## solution is titrated with 0.0500 M NaOH and it requires 15.67 mL to reach the end point. What is the concentration of the H##_2##CO##_3## ?
H##_2##CO##_3## + 2 NaOH ##\longrightarrow## Na##_2##CO##_3## + 2 H##_2##O

Sketch the titration curve for 50.0 mL 0.1 M HCl, K##_a## = 1.8 x 10##^{-5}## with 0.1 M NaOH. Include points on your graph for the initial pH, the pH at half way to the equivalence point, the pH at the equivalence point and the pH after the equivalence point.

Sketch the titration curve for 50.0 mL 0.1 M CH##_3##COOH, K##_a## = 1.8 x 10##^{-5}## with 0.1 M NaOH. Include points on your graph and an example calculation for the initial pH, the pH at half way to the equivalence point, the pH at the equivalence point and the pH after the equivalence point.

Find the pH of a 0.1 M solution of NH##_3##. If 50 ml of this solution is titrated by 50 ml of 0.1 M HCl, find the pH at the equivalence point. (K##_a## = 5.56 x 10##^{-10}## )