Calculate the pH and the pOH of an aqueous solution that is 0.025 M in HCl(aq) and 0.075 M in HBr(aq) at 25°C.
3 answers
extremely easy. Sorry! pH=1 and pOH = 13
Nope. Tricky question.
Suppose you take 1 L of each. That gives you 1 L x 0.025 mol/L HCl = 0.025 mols.
1L x 0.075 mol/L HBr = 0.075 mols.
Total mols = 0.025+0.075 = 0.1 mol but what's the volume? The volume is 2L so
M = 0.1 mol/2.0L = 0.05 M for H^+. Take pH and pOH from that. I get about 1.3 and 12.7.
Suppose you take 1 L of each. That gives you 1 L x 0.025 mol/L HCl = 0.025 mols.
1L x 0.075 mol/L HBr = 0.075 mols.
Total mols = 0.025+0.075 = 0.1 mol but what's the volume? The volume is 2L so
M = 0.1 mol/2.0L = 0.05 M for H^+. Take pH and pOH from that. I get about 1.3 and 12.7.
the pH for this is the sum of the two concentrations so 0.025 M+ 0.075 M = 0.10 M H
then with the sum of the concentrations, we can find pH
pH= -log(0.10 M)= 1.0 and
pOH= 14 - pH = 13
I know the answer was given but maybe walking it thru might help someone else!
then with the sum of the concentrations, we can find pH
pH= -log(0.10 M)= 1.0 and
pOH= 14 - pH = 13
I know the answer was given but maybe walking it thru might help someone else!