Acid–base titrations Knowledge-Based Practice

Questions

1. 1.

   A 30.0 mL sample of a 0.200 M diprotic acid, $\text{H}_2\text{A}$, is titrated with 0.150 M $\text{KOH}$. What total volume of the $\text{KOH}$ solution is required to reach the second equivalence point?

   • A) 40.0 mL
   • B) 80.0 mL
   • C) 60.0 mL
   • D) 120.0 mL
2. 2.

   A 0.512 g sample of an unknown monoprotic acid is completely neutralized by 25.0 mL of a 0.160 M NaOH solution. What is the molar mass of the unknown acid?

   • A) 32.0 g/mol
   • B) 64.0 g/mol
   • C) 256 g/mol
   • D) 128 g/mol
3. 3.

   A 40.0 mL sample of 0.100 M HCl is titrated with 0.100 M NaOH at 25 °C. What is the pH of the resulting solution after 60.0 mL of 0.100 M NaOH has been added?

   • A) 12.30
   • B) 1.70
   • C) 12.00
   • D) 7.00
4. 4.

   A 40.0 mL sample of 0.150 M NH3 ($K_{\mathrm{b}} = 1.8 \times 10^{-5}$) is titrated with 0.150 M HCl at 25 °C. What is the pH of the resulting solution after the addition of 20.0 mL of the titrant?

   • A) 4.74
   • B) 7.00
   • C) 9.26
   • D) 11.23
5. 5.

   A 25.0 mL sample of 0.100 M CH3COOH (Ka = 1.8 × 10−5) is titrated with 0.100 M NaOH at 25 °C. What is the pH of the resulting solution at the equivalence point?

   • A) 7.00
   • B) 8.72
   • C) 5.28
   • D) 9.26

Answers and step-by-step solutions appear after you finish the test.