Question

For each of the following solutions, calculate the initial pH and the final pH after adding 0.010 mol
of HCℓ.
a) 500.0 mL of pure water
i'm not sure how to do this question..
would the equation be
h20+h30 equilibrium arrows h30+h20

Answer 1

You are supposed to recognize that HCl is a strong acid (meaning it ionizes 100%) so pure water is pH of 7. Then you add 0.01 mol HCl which adds to 500 mL water. That 0.01 mol becomes 0.01/0.5 L = ?? and convert that to pH.