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SAT II Chemistry : pH

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Example Question #1 : Reaction Types

A scientist makes a solution by adding 0.2 grams of NaOH $\displaystyle NaOH$ to enough water so that the resulting solution has a volume of 10 liters. What, approximately, is the pH of this solution?

Possible Answers:

$\displaystyle 11$

$\displaystyle 3$

$\displaystyle 2$

$\displaystyle 10$

$\displaystyle 12$

Correct answer:

$\displaystyle 11$

Explanation:

NaOH $\displaystyle NaOH$ has a molar mass of approximately 40 g/mol, meaning that there is 0.01 mol of it in the solution. Sodium hydroxide is a strong base and completely dissociates in water. Its concentration in the solution is $\frac{0.01}{10}=10^{-3}$ $\displaystyle \frac{0.01}{10}=10^{-3}$ $\frac{mol}{L}$ $\displaystyle \frac{mol}{L}$. This means that the concentration of H^+ $\displaystyle H^+$ ions is $\frac{10^{-14}}{10^{-3}}=10^{-11}$ $\displaystyle \frac{10^{-14}}{10^{-3}}=10^{-11}$ and $-\log (10^{-11}) = 11$ $\displaystyle -\log (10^{-11}) = 11$. Thus, the pH of the solution is 11.

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SAT II Chemistry : pH

Study concepts, example questions & explanations for SAT II Chemistry

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Example Question #1 : Reaction Types

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