General Chemistry 2: Acids and Bases

Define acids and bases according to the Bronsted-Lowry and Lewis theories.

Rank the following in terms of acidity: HClO, IOH, and HBrO. Explain the trend.

Rank the following in terms of acidity: HClO, HClO$_2$, HClO$_3$, HClO$_4$. Explain the trend.

Rank the following in terms of basicity:

HCN K$_a$ = 4.8 x 10$^{-10}$

HSO$_4^-$ K$_a$ = 1.2 x 10$^{-2}$

HS$^-$ K$_a$ = 7.1 x 10$^{-15}$

H$_2$CO$_3$ K$_a$ = 4.3 x 10$^{-7}$

The percent ionization of NH$_3$ is found to be 4.2% in a solution, find the concentration of NH$_3$.

NH$_3$ (aq) + H$_2$O $\leftrightharpoons$ NH$_4^+$ + OH$^-$ , K$_b$ = 1.8 x 10$^{-5}$

Calculate the pH of a 0.2 M solution of NH$_4$Br, K$_a$ = 5.6 x 10$^{-10}$

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$_4^{3-}$.

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.

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.