General Chemistry 2

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$^{-4}$