General Chemistry 2: Acids and Bases

Define acids and bases according to the Bronsted-Lowry and Lewis theories.

What are the factors that affect the strength of an acid?

Rank the following in terms of acidity: HClO, IOH, and HBrO. Explain the trend.

Rank the following in terms of acidity: HClO, HClO##_2##, HClO##_3##, HClO##_4##. Explain the trend.

Rank the following in terms of basicity:
HCN K##_a## = 4.8 x 10##^{-10}##
HSO##_4^-## K##_a## = 1.2 x 10##^{-2}##
HS##^-## K##_a## = 7.1 x 10##^{-15}##
H##_2##CO##_3## K##_a## = 4.3 x 10##^{-7}##

In the below reactions, identify which reactant is the lewis acid and which is the lewis base.
NH##_3## + BF##_3## ##\leftrightharpoons## NH##_3##BF##_3##
KOH + CH##_3##Br ##\leftrightharpoons## KBr + CH##_3##OH

Hydrogen bromide is a gas at room temperature. It is soluble in water, forming hydrobromic acid. Identify the conjugate acid-base pairs.
HBr (aq) + H##_2##O (l) ##\longrightarrow##

Ammonia is a pungent gas at room temperature. Its main use is in the production of fertilizers and explosives. It is very soluble in water. It forms a basic solution that is used in common products, such as glass cleans. Identify the conjugate acid-base pairs in the reaction between aqueous ammonia and water.
NH##_3## (aq) + H##_2##O (l) ##\longrightarrow##

Predict the products for the following reaction
KHSO##_3## + NH##_3## ##\leftrightharpoons## ?
KHSO##_3## has K##a## = 6.2 x 10##^{-8}## K##b## = 1.0 x 10##^{-4}##
NH##_3## has K##a## = 7.8 x 10##^{-13}## K##b## = 1.8 x 10##^{-5}##

The percent ionization of NH##_3## is found to be 4.2% in a solution, find the concentration of NH##_3##.
NH##_3## (aq) + H##_2##O ##\leftrightharpoons## NH##_4^+## + OH##^-## , K##_b## = 1.8 x 10##^{-5}##

Lactic acid, HC##_3##H##_5##O##_3##, is a waste product that accumulates in muscle during exertion, leading to pain and a feeling of fatigue. In a 0.100 M aqueous solution, lactic acid is 3.7% dissociated. Calculate the value of K##_a## for this reaction.

Find the pH of 2.0 M HF, ( K##_a## = 7.1 x 10##^{-4}## )

Find the pH of 3.0 M NH##_3##, ( K##_b## = 1.8 x 10##^{-5}## )

Find the pH of a 0.100 M solution of HOCl, K##_a## = 3.5 x 10##^{-8}##

Calculate the pH of a 0.2 M solution of NH##_4##Br, K##_a## = 5.6 x 10##^{-10}##

Compare the concentration of H##_3##O##^+## in 1 M and 2 M solutions of HC##_2##H##_3##O##_2##, K##_a## = 1.8 x 10##^{-5}##. (doubling the concentration results in an increase of hydronium ions by what factor?)

A solution contains 0.5 M KOH and 0.75 M Cs(OH)##_2##, calculate the pOH of the solution

Calculate the pH of a mixture of equal parts 2.0 M HF and 1.0 M HOCl. Also find the concentration of OCl##^-## and F##^-## ions in the solution. The K##_a## of HF = 7.2 x 10##^{-4}##, K##_a## of HOCl = 3.5 x 10##^{-8}##

Calculate the pH of 0.1 M NH##_4##Cl. The K##_b## of NH##_3## = 1.8 x 10##^{-5}##

Calculate the pH of 0.12 M KNO##_2##. The K##_a## of HNO##_2## = 4.0 x 10##^{-4}##