SAT II Chemistry : Acid-Base Reactions

Study concepts, example questions & explanations for SAT II Chemistry

varsity tutors app store varsity tutors android store

Example Questions

Example Question #1 : Identifying And Defining Acids And Bases

Which of the following cannot act as a Bronsted-Lowry base (proton recipient) in aqueous solution?

Possible Answers:

\displaystyle HCO_3^-

\displaystyle NH_3

\displaystyle OH^-

\displaystyle H_2O

\displaystyle NH_4^+

Correct answer:

\displaystyle NH_4^+

Explanation:

\displaystyle NH_4^+ cannot receive another proton \displaystyle (H^+) because then it would become \displaystyle NH_5^{2+}, which does not exist. All of the other answer choices are fine:

\displaystyle NH_3 \Rightarrow NH_4^+

\displaystyle HCO_3^-\Rightarrow H_2CO_3

\displaystyle H_2O\Rightarrow H_3O^+

\displaystyle OH^-\Rightarrow H_2O

Example Question #1 : Reaction Types

A scientist makes a solution by adding 0.2 grams of \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 12

\displaystyle 2

\displaystyle 10

\displaystyle 11

\displaystyle 3

Correct answer:

\displaystyle 11

Explanation:

\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 \displaystyle \frac{0.01}{10}=10^{-3} \displaystyle \frac{mol}{L}. This means that the concentration of \displaystyle H^+ ions is \displaystyle \frac{10^{-14}}{10^{-3}}=10^{-11} and \displaystyle -\log (10^{-11}) = 11. Thus, the pH of the solution is 11.

Learning Tools by Varsity Tutors