Question

11. You have a mixture of 0.10M HCl and 0.10M HI. What is the pH of the resulting solution? a. 1.00 OHOL b. 2.00 dignos 926d Trelsviupassas 0.70 d. 0.20 noitulo tuoups ni noi3591 ir notanog muhdilupe si to su svertit e. Cannot determine with the information provided OH 1 00+ HOH 12. The autoionization of water is an endothermic reaction. This means at higher temperatures: a. pH of pure water > 7.00 Inigh art of zeil mundillope I > pod b. pH of pure water < 7.00 [H3O+] > 107

Answer 1

11. Option E is correct as the volume of each acid has to be given to calculate the total concentration of $H^{+}$ ions in the solution and hence the pH.

12. Option B is correct.

The autoionization of the water is like-
H20+ heat = H+ + OH-
., as the reaction is endothermic! So if you increase the temperature i.e you are actually supplying heat to the system, or you are supplying more reactants to the system and according to Le-Chatelier's principle, the forward reaction would be more favorable i.e more $H^{+}$ ions are generated so the pH at higher temperatures becomes low.