Acids and Bases

Calculate the pH of a mixture of equal parts 2.0 M HF and 1.0 M HOCl. Also find the concentration of OCl\(^-\) and F\(^-\) ions in the solution. The K\(_a\) of HF = 7.2 x 10\(^{-4}\), K\(_a\) of HOCl = 3.5 x 10\(^{-8}\)

Calculate the pH of 0.1 M NH\(_4\)Cl. The K\(_b\) of NH\(_3\) = 1.8 x 10\(^{-5}\)

Calculate the pH of 0.12 M KNO\(_2\). The K\(_a\) of HNO\(_2\) = 4.0 x 10\(^{-4}\)

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\(^{-19}\)