If a solution contains 0.0100 mole of HCl in 10.0 mL aqueous solution.

Question

a.) What is its molarity? My answer is 1M (0.0100 mole/10.0 mL * 1000 mL/1L = 1M)
b.) What is H^+ ion concentration for this solution?
c.) What is the expected pH for this solution?
pls help i don't know how to answer the last 2 questions

Answer 1

You're batting 1000 on a. Just plug in the numbers for b and c.
b.
HCl is a strong acid (meaning it ionizes 100%) so HCl ==> H^+ + Cl^-

If HCl = 1.0 M then (H^+) must be 1.0 M (and Cl^- must be 1.0 M).

c.
pH = -log(H^+)
pH = -log(1.0)
pH = -(0)
pH = 0
(Note: I doubt it would read this on a pH meter).