Chemistry: Problems/ solutions on pH and pOH Solutions - Answer

1) What is the pH of the solution with a hydronium concentration [H₃O⁺] 1.47 x 10^-4?
     What is the pOH of this solution?
     pH = -log (1.47 x 10^-4) = 3.83
      pOH = 14 - pH = 14 - 3.83 = 10.17
2) What is the pOH of the solution with a hydroxyl concentration [OH-] 2.98 x 10^-2?
     What is the hydronium concentration [H₃O⁺] of this solution?
     pOH = -log (2.98 x 10^-2) = 1.53
     hydronium concentration [H₃O⁺] =      1 x 10^-14     = 3.37 x 10^-13
                                                               2.98 x 10^-2
      OR   pH = 14- pOH = 14 - 1.53 = 12.47
    hydronium concentration [H₃O⁺] = antilog -12.47 = 3.38 x 10^-13
3) What is the hydronium concentration [H₃O⁺] of a solution with a pH of 7.84?
     What is the hydroxyl concentration [OH-] of this solution?
     hydronium concentration [H₃O⁺] = antilog -7.84 = 1.45 x 10^-8
     hydroxyl concentration [OH-] =     1 x 10^-14     = 6.90 x 10^-7
                                                          1.45 x 10^-8
     OR pOH = 14-pH = 14 - 7.84 = 6.16
      hydroxyl concentration [OH-] = antilog -6.16 = 6.9 x 10^-7
4) What is the hydroxyl concentration [OH-] of a solution with a pH of 3.76?
     pOH = 14 - pH = 14 - 3.76 = 10.24
     hydroxyl concentration [OH-] = antilog -10.24 = 5.75 x 10^-11
5) What is the hydronium concentration [H₃O⁺] of a solution with a pOH of 2.47?
     pH = 14 - pOH = 14 - 2.47 = 11.53
     hydronium concentration [H₃O⁺] = antilog -11.53 = 2.95 x 10^-12