What is the pH of a solution prepared by diluting 25.00mL of 0.020M barium hydroxide to a volume of 100.00mL?

Answer 1

Start with 0.020 M Ba(OH)2.
Calculate the (OH^-). Ba(OH)2 is 100% ionized.
Then dilute that by a factor of 25/100.
Then POH and pH from that. Post your work if you need more help.

Answer 2

Find the moles of Ba(OH)2 by .025L*.020M
Then divide answer by .100L to find new molarity
then find pOH=-log(OH-)
Then subtract from 14
pH=14-pOH