Answer to Question #203003 in General Chemistry for Mickayla

General Chemistry

Question #203003

The pH of a 0.01M solution of a weak base is 10.65. What is the value of K_b for this base?

1)2.0 x 10^-5

2)5.0 x 10^-4

3)5.0 x 10^-20

4)0.073

Expert's answer

Kb-the degree of dissociation of the solution into ions

Right variant: 4

Learn more about our help with Assignments: Chemistry

Comments

No comments. Be the first!

Leave a comment

Related Questions

1. The pH of a 0.55M solution of hypobromous acid, HOBr, is 4.48. Calculate the value of Ka.1)3.0 x 10
2. Calculate the pH of a buffer solution prepared by dissolving 0.20 mole of cyanic acid (HCNO) and 0.8
3. What is the pH of a 0.65M sodium carbonate solution? (Kb = 1.8 x 10-4)1)10.22)123)3.94)2.0
4. What is the pH of a 1.3M butyric acid solution? (Ka = 1.54 x 10-5)1)4.72)5.03)2.34)2.5
5. In the reactionHSO3- + HClO2 ↔ H2SO3 + ClO2-The Bronsted bases are:1)HSO3- + HClO22)HSO3- +
6. An indicator is weak acid (or base) having a conjugate base (or acid) with a significantly different
7. An acid HA has Ka = 2.28 x 10 -4. The % ionisation of this acid in a 0.170 M solution of the acid