Asked by Allison
If you have 0.2 M of NaC7H4ClO2 with a pH of 8.65, what is the pH of 0.2 M of HC7H4ClO2?
Answers
Answered by
DrBob222
Let's just call this acid HA. It's the salt that is hydrolyzing, so
A^- + HOH ==> HA + OH^-
Kb = Kw/Ka = (HA)(OH^-)/(A^-)
You know Kw, Ka is what you want, (HA)=(OH^-) and you can get the OH from the pH. After you find Ka, use that as you would a weak acid ionization.
HA ==> H^+ + A^-
Ka = (H^+)(A^-)/(HA)
Do an ICE chart for the HA and solve for H^+ and pH. Post your work if you get stuck.
A^- + HOH ==> HA + OH^-
Kb = Kw/Ka = (HA)(OH^-)/(A^-)
You know Kw, Ka is what you want, (HA)=(OH^-) and you can get the OH from the pH. After you find Ka, use that as you would a weak acid ionization.
HA ==> H^+ + A^-
Ka = (H^+)(A^-)/(HA)
Do an ICE chart for the HA and solve for H^+ and pH. Post your work if you get stuck.
Answered by
Allison
im sorry i don't understand could you please go into a little more detail.. i broke it up into NaC7H4ClO2 --> Na+ and C7H4ClO2
then did C7H4ClO2 + H2O --> ?
then did C7H4ClO2 + H2O --> ?
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