given acetic acid has a Ka= 1.8 x 10^(-5). Determine the pH at the following points in the titration of 25mL of 0.5M CH3COOH with 0.5M of NaOH solution.
CH3COOH + Na +OH ---> Na + CH3COO + H2O
1) before addition of any NaOH
2) after addition of 10.00ml of 0.5M NaOH
okay, so I believe I should use the ICE chart, but I'm thrown off by the equation being Na + OH , and the questions asking for NaOH. And then use -log(x) to find pH.
If you would help me set up the equation for both 1 & 2, I should be able to work from there. Thank you so much