What is the pH of a solution that is 0.046 M in HA and also 0.0026 M in NaA? (Ka = 7.1 × 10–6)

A 2.5 × 10–4 M solution of MnSO4 is gradually made more basic by adding NaOH. At what pH will manganese(II) hydroxide begin to precipitate? The Ksp of Mn(OH)2 is 2.0 × 10–13 and Kw = 1.01 × 10–14.

Arrange the following acids in order of decreasing acid strength in aqueous solution: HCl, HOCl, HOBr, and HOI.

Using the titration curve below, answer the following questions:    In this titration, the First Equivalence point occurs at mL of NaOH and the Second Equivalence point occurs at mL of NaOH. The First pKa value for this acid is and the second is .  

When a weak base is titrated with a strong acid, the pH at the equivalence point is _____.

What is the pOH of 0.037 M HI(aq) at 25 °C? (Kw = 1.01 × 10–14)?

The chemical equations below show the reaction of Al(OH)3 as a Lewis acid and as a Lewis base, respectively. Al(OH)3(s) + OH–(aq) Al(OH)4–(aq) Al(OH)3(s) + 3 H3O+(aq) Al3+(aq) + 3 H2O() Substances that can behave as either Lewis acids or bases are called ________ substances.

When mixed in appropriate amounts, each of the following mixtures can produce an effective buffer solution except _____.

What is the pH of a 0.31 M solution of methylamine (CH3NH2, Kb = 4.4 × 10–4) at 25oC? (Kw = 1.01 × 10-14)

Which acid–base reaction results in acidic solution?