## HW 13.23

Julia Spaczai 2G
Posts: 19
Joined: Fri Sep 25, 2015 3:00 am

### HW 13.23

For part A of this problem, it asks you to sketch the titration curve for the titration of 5.00 mL .010 M NaOH with 0.005 M HCl and to indicate the pH of the initial and final solutions, as well as the pH at the stoichiometric point. I understand how to calculate the pH of the initial solution and that the pH at the stoichiometric point is 7 because it is a strong acid/strong base titration, but how would you calculate the pH of the final solution?

Chem_Mod
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### Re: HW 13.23

The final solution is after the stoich. point so as you continue to add HCl, it ionizes to form H3O+ and Cl-. Since you know the volume of acid added, you can calculate the mol of H3O+ in solution and solve for pH.

Rachael_1H
Posts: 31
Joined: Fri Sep 25, 2015 3:00 am

### Re: HW 13.23

How do you know the volume of acid added? Only the molarity of HCl, the acid, is given.

Camryn Marshall 1C
Posts: 37
Joined: Fri Sep 25, 2015 3:00 am

### Re: HW 13.23

You can calculate the volume because you know that at the stoichiometric point moles of sample is equal to the moles added so since you know molarity of the substance added you can do V=n/M for the substance added