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What is the concentration of OH– in a 1.0 × 10–3 M Ba(OH)2 solution?

What is the concentration of OH– in a 0.083 M NaOH solution?

A 20.00-mL sample of 0.3000 M HBr is titrated with 0.15 M NaOH. What is the pH of the solution after 40.3 mL of NaOH have been added to the acid?

Calculate the pH of a buffer solution prepared by dissolving 0.20 mole of sodium cyanate (NaCNO) and 1.0 mole of cyanic acid (HCNO) in enough water to make 1.0 liter of solution.  [Ka(HCNO) = 2.0 × 10–4]

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

A CH3COOH/CH3COO– buffer can be produced by adding a strong acid to a solution of CH3COO– ions.

What is the conjugate base of sulfuric acid?

What is the concentration of OH– in a 1.0 × 10–3 M Ba(OH)2 solution?

What is the concentration of OH– in a 0.083 M NaOH solution?

Which of the following is the correct equilibrium expression for the autoionization of water?