A #10^-3 M# solution has been diluted to 100 times.Calculate the pH of the diluted solution?
1 Answer
Here's one possible answer.
Explanation:
Since you didn't specify the content of your solution, I will have to assume that you're dealing with a solution that contains a strong monoprotic acid like hydrochloric acid,
Hydrochloric acid ionizes in a
#["H"_3"O"^(+)] = 10^(-3)"M"#
Now, you dilute this solution by a factor of
This means that if you take
#["H"_3"O"^(+)] = n/V = 10^(-3)"M"-># for the initial solution
After the initial solution is diluted, its volume will be
#["H"_3"O"^(+)] = n/(100 * V) = 1/100 * n/V#
#["H"_3"O"^(+)] = 1/100 * 10^(-3)"M" = 10^(-5)"M"#
Now ll you have to do is use the equation
#color(blue)(|bar(ul(color(white)(a/a)"pH" = - log(["H"_3"O"^(+)])color(white)(a/a)|)))#
to find the pH of the dilutes solution. In your case, you will have
#"pH" = - log(10^(-5)) = color(green)(|bar(ul(color(white)(a/a)5color(white)(a/a)|)))#