Question

The value for Kw is 1.0 x 10-14 at 298K, but this value is temperature dependent. Given what you know about Kw and acid/base chemistry, what will the pH of water be at 303K if the value for Kw is 1.47 x 10-14? Is this solution acidic, basic, or neutral?

Answer 1

6.92; neutral

Step-by-step explanation:

Kw = [H^+][OH^-] = 1.47 × 10^-14

pKw = pH + pOH = 13.83

At neutrality, [H^+] = [OH^-] and pH = pOH

2pH = 13.83

pH = 6.92

The pH will be 6.92.

At 303 K, this will be the neutral pH, because [H^+] = [OH^-]