what is the pH of a solution prepared by adding 0.50 mol KOH to 1.0 L of 0.30 M HNO3?
3 answers
How is there no answer to this...SOMEONE HELP PLEASE
its 13.30 and i only know that bc i saw the answer key
Since:
mol of HNO3 = 0.30 x 1 = 0.3 mol
And mol of KOH bigger than mol of HNO3
Then:
The solution has more OH therefore basic
POH = - log [OH]
[OH] = [OH] - [H]
POH = - log [0.2]
POH = 0.7
PH + POH = 14
PH = 14 - 0.7 = 13.3
mol of HNO3 = 0.30 x 1 = 0.3 mol
And mol of KOH bigger than mol of HNO3
Then:
The solution has more OH therefore basic
POH = - log [OH]
[OH] = [OH] - [H]
POH = - log [0.2]
POH = 0.7
PH + POH = 14
PH = 14 - 0.7 = 13.3
3 answers