Question

What is the pH of a 1.00 M solution of disodium sulfate (Na₂SO₄)?
You can calculate the Kb from the Ka values given in the question 1. (K_a1 = large
K_a2 = 1.2 x 10^-2)

1. 7.94
2. 8.02
3. 6.01
4. 7.96

Answer 1

Na₂SO₄ ( aq ) $\rightarrow$ 2 Na⁺ ( aq ) + SO₄^2- ( aq )

SO₄^2- ( aq ) + H₂O ( l ) $\rightleftharpoons$ HSO₄^- ( aq ) + OH^- ( aq )

K_b ( SO₄^2- ) = K_w / K_a2 = 10^–14 / 1.2 x 10^-2 = 8.33 x 10^-13

_calculations

So, (aq) + H₂O = HSO i to the tre (1-x) ta tre -13 Kp = 8.33 810 = 2 x I- 1 - 2 = [01] =9.12 68 x 10 mg = -109 (9.1268 X10 ) -6.04 pa = 14-6.0% = 7.96