B, a weak base, can react with water in equilibrium into hydroxide ions and BH⁺ . Which of the following equation represents dissociation of B, a weak base, in water?

dissociation of weak acid, HA, is represented by following equation :

HA(aq) + H₂O(l) ⇌ H₃O⁺(aq) + A^-(aq)

The equilibrium constant for this reaction is represented by K_a . Which of the following equation represents expression of equilibrium constant, K_a?

the following equation represents the equilibrium reaction between weak base, B, with water :

B(aq) + H₂O(l) ⇌ BH⁺(aq) + OH^-(aq)

The equilibrium constant for this reaction is represented by K_b . Which of the following equation represents expression of equilibrium constant, K_b?

Which one IS TRUE about dissociation of weak acid in water ?

1.[H⁺] ions > [OH^-] ions in weak acid-containing solution

2.The numerical value of Equilibrium constant of dissociation of weak acid, K_a, increase as the temperature decrease

3.It makes light bulb glow very bright

4.pOH > 7 in weak acid-containing solution

Which one IS TRUE about dissociation of weak base in water ?

1.[H⁺] ions = [OH^-] ions in weak base-containing solution

2.The numerical value of Equilibrium constant of dissociation of weak base, K_b, decrease as the temperature decrease

3.Weak base are less dissociated in solution as the amount of concentration of common-ion OH^- in solution increase

4.pH > 7 in weak base-containing solution

calculate the Ka of a solution with a pKb of 3.38

calculate the pKb of solution with a pKa of 6.9

Calculate the Kb of a solution that has a pKb of 4.2

How would you calculate K_b for the formate ion (HCOO^–), given that the K_a for formic acid (HCOOH) is 1.8 × 10^–4? (K_w=1.0 × 10^–14)

Using the data in the table, which of the conjugate bases below is the weakest base?

Using the data in the table, which of the conjugate acids below is the weakest acid?