Author: Anonymous

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 [equil1] mL of NaOH and the Second Equivalence point occurs at [equil2] mL of NaOH. The First pKa value for this acid is [pka1] and the second is [pka2].  

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

The solubility of calcium carbonate (CaCO3) in water at 25°C is g/L. What is the Ksp of this sparingly soluble salt?

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

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 of the following substances is never a Brønsted-Lowry base in an aqueous solution?