At equilibrium, a 1.00 M OCl− solution has an [OH−] of 5.75 × 10−4 M. Which of the following is the correct pH of the solution?

3.24

3.3 × 10−7

14.00

10.76

Question

At equilibrium, a 1.00 M OCl− solution has an [OH−] of 5.75 × 10−4 M. Which of the following is the correct pH of the solution?

3.24

3.3 × 10−7

14.00

10.76

rushwr · Answer

$$[OH ^{-}] = 5.75 * 10^{-4}$$
we know pKw = 10 ^-14
$$[H ]= \frac{ Kw }{ [OH] } = \frac{ 10^{-14} }{ 5.75 * 10^{-4} }= 0.174 * 10^{-10}$$$$pH = -\log _{10} [H ^{+}]$$
pH = 10.76