posted by .

Calculate the pH of an aqueous solution of 0.15 M potassium carbonate.

I know that pH = -log(H30+) but I am not sure how to start this problem.

Hydrolyze the CO3^2-.
CO3^- + HOH ==> HCO3^- + OH^-
Do an ICE chart, Kb = Kw/k2 for H2CO3.

so for kb I do 1e-14/.15?

No. Kb = 1E-14/k2 for H2CO3.

How do I set up an ice table when I only have .15M?

Similar Questions

1. Chemistry

Buffers- Common Ion effect IS this Correct Calculate the pH of a aqueous solution containing 0.15 M HNO2 and 0.20 M NaNO2 (aq). The Ka of nitrous acid is 4.0*10^-4. HNO2 + H20 <--> NaNO2- + H30^+ Inital 0.15 0.20 X Final 0.15 …
2. chemistry

Hi, The problem is: "Calculate the concentration of OH- and the pH value of an aqueous solution in which [H30+] is 0.014M at 25C. Is this solution acidic, basic, or neutral?

What is the [H3O+] for a neutral solution at 50 degrees celsius?

1) The Ka for acetic acid is 1.8e-5. What is the pH of a 3.18M solution of this acid?

What is the pH of a 5.06E-2 M aqueous solution of sodium acetate?
6. Chemistry

If you add 0.35grams NaF to 150mL of a 0.30M HF, what is the pH of the resulting solution?