18. Aqueous Equilibrium

A 10.0 mL sample of 0.200 M hydrocyanic acid (HCN) is titrated with 0.0998 M NaOH. What is the pH at the equivalence point? For hydrocyanic acid, pKₐ = 9.31.

A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH. Determine the pH of the solution after the addition of 100.0 mL of KOH. The Ka of HF is 3.5 × 10^-4.

A 100.0 mL sample of 0.20 mol L⁻¹ HF is titrated with 0.10 mol L⁻¹ KOH. Determine the pH of the solution after the addition of 200.0 mL of KOH. The Kₐ of HF is 3.5 × 10⁻⁴.

A 25.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH. What is the pH of the solution after the addition of 15.0 mL of KOH? The Ka of HF is 3.5×10^-4.

A 30.0-mL volume of 0.50 M CH3COOH (Ka=1.8×10⁻⁵) was titrated with 0.50 M NaOH. Calculate the pH after the addition of 30.0 mL of NaOH at 25 °C.

A 30.00-mL sample of 0.125 M HCOOH is being titrated with 0.175 M NaOH. What is the pH after 11.2 mL of NaOH has been added? Ka of HCOOH = 1.8 × 10⁻⁴

A 30.00-mL sample of 0.125 M HCOOH is being titrated with 0.175 M NaOH. What is the pH after 15.0 mL of NaOH has been added? Ka of HCOOH = 1.8 × 10⁻⁴

A 30.00-mL sample of 0.125 M HCOOH is being titrated with 0.175 M NaOH. What is the pH after 21.4 mL of NaOH has been added? Ka of HCOOH = 1.8 × 10⁻⁴

A 30.00-mL sample of 0.125 M HCOOH is being titrated with 0.175 M NaOH. What is the pH after 23.0 mL of NaOH has been added? Ka of HCOOH = 1.8 × 10⁻⁴

A 30.00-mL sample of 0.125 M HCOOH is being titrated with 0.175 M NaOH. What is the pH after 30.0 mL of NaOH has been added? Ka of HCOOH = 1.8 × 10⁻⁴

What is the pH of a 35.0-mL sample of 0.150 M acetic acid (CH3COOH, Ka=1.8×10⁻⁵) before any 0.150 M NaOH solution is added?

A 35.0-mL sample of 0.150 M acetic acid (CH3COOH, Ka=1.8×10⁻⁵) is titrated with 0.150 M NaOH solution. Calculate the pH after 35.0 mL of the base have been added.

A student titrated a 100 mL sample of 0.100 M acetic acid with 0.050 M NaOH. (For acetic acid, Ka = 1.8 × 10^-5 at room temperature.) Calculate the pH after 50.0 mL of NaOH has been added.

Consider the titration of 100.0 mL of 0.016 M HOCl (Ka=3.5×10⁻⁸) with 0.0400 M NaOH. Calculate the pH after the addition of 10.0 mL of 0.0400 M NaOH.

Consider the titration of 25.00 mL of 0.150 M hydrazoic acid (Ka = 1.90 × 10^-5) with 0.200 M NaOH. What is the pH of the solution after the addition of 15.00 mL of NaOH solution?