2 pH Questions...help!?

Question

Looks simple enough yet I can't come up with the correct answers. Help please! Please show steps...any help appreciated!

1. What is the pH (to nearest 0.01 pH unit) of a solution prepared by mixing 54.0 mL of 0.0397 M NaOH and 67.0 mL of 0.0203 M Ba(OH)2?

2. What is the pH (to nearest 0.01 pH unit) of a solution prepared by mixing 83.0 mL of 0.526 M HCl and 78.0 mL of 0.595 M NaOH?

Link to acid/base table: http://www.webassign.net/wertz/caqs/html/resource/acidbase_pka.html

Answer 1

For both sodium and barium hydroxide, they are totally ionized. Then you can compute the total hydroxide moles and divide by the sum of volumes. Then you can find the corresponding [H+] from [H+][OH-]=10x10-15.

Here you figure the initial moles of [H+] and [OH-],
moles= volume x molarity. Subtract the smaller from the larger, this will give you the remaining moles of the larger. Divide by 0.161 L to get concentration.

Answer 2

i kn othat ph times 54.0 ml over 0.0397 m to the y axis of the x unit then u divede the constant and add the lower number when u get that anwser which is 0.oo3954 u will subtrct ph millimeter 0.1 and go after the higher nimber the ph is 599.6 rememebr u have to think about the scientifc method