pH and pOH Calculations
1) Determine the pH of a 0.00340 M HNO3 solution.
2) Determine the pOH of a 0.00340 M HNO3 solution.
3) Determine the pH of a 4.30 x 10-4 M NaOH solution.
4) If a solution is created by adding water to 2.30 x 10-4 moles of NaOH and 4.50 x 10-6 moles of HBr until the
final volume is 1.00 L, what is the pH of this solution?
5) Why would we say that a solution with a H3O+ concentration of 1.00 x 10-7 M is said to be neutral. If it
contains acid, shouldn’t it be acidic?
6) What is the pH of a solution that contains 25 grams of hydrochloric acid (HCl) dissolved in 1.5 liters of
water?
7) What is the pH of a solution that contains 1.32 grams of nitric acid (HNO3) dissolved in 750.0 mL of water?
8) What is the pH of a solution that contains 1.20 moles of nitric acid (HNO3) and 1.70 moles of hydrochloric
acid (HCl) dissolved in 1000. liters of water?
9) If a solution has a [H3O+] concentration of 4.50 x 10-7 M, is this an acidic or basic solution? Explain.
10) An acidic solution has a pH of 4.00 If I dilute 10.0 mL of this solution to a final volume of 1000.0 mL, what
is the pH of the resulting solution?
