Calculate the pH for an aqueous solution of pyridine that contains $2.15 \times 10 ^{- 4 }\mathrm {~mol} \mathrm {~L} ^ { - 1 }$ hydroxide ion. A)4.65 × 10^-11 B)2.15 × 10^-4 C)3.67 D)10.33

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Quizplus · Accepted Answer

The concentration of hydroxide ions is given, so we first calculate the pOH: $ \text{pOH} = -\log(2.15 \times 10^{-4}) \approx 3.67 $. Then, use the relation $ \text{pH} + \text{pOH} = 14 $ to find the pH: $ \text{pH} = 14 - 3.67 = 10.33 $.

Calculate the PH for an Aqueous Solution of Pyridine That 2.15×10−4 mol L−12.15 \times 10 ^{- 4 }\mathrm {~mol} \mathrm {~L} ^ { - 1 }2.15×10−4 mol L−1

Calculate the PH for an Aqueous Solution of Pyridine That $2.15 \times 10 ^{- 4 }\mathrm {~mol} \mathrm {~L} ^ { - 1 }$