General Chemistry 2: Acids and Bases

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

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$^{-5}$

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$^{-8}$

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

Find the concentration of HS$^-$, S$^{2-}$ and H$_3$O$^+$ in a 0.075 M solution of H$_2$S

H$_2$S + H$_2$O $\longrightarrow$ HS$^-$ + H$_3$O$^+$, K$_{a1}$ = 1.0 x 10$^{-7}$

HS$^-$ + H$_2$O $\longrightarrow$ S$^2-$ + H$_3$O$^+$, K$_{a2}$ = 1.0 x 10$^{-19}$

Calculate the pH and concentration of all species of a 3.0 M solution of phosphoric acid, H$_3$PO$_4$

Find the equilibrium concentrations of the species H$_2$SO$_4$, HSO$_4^-$, SO$_4^{2-}$, and H$^{+}$ given a 1.0 M solution of H$_2$SO$_4$.

Find the pH of the buffer solution consisting of 0.60 M HF and 1.0 M KF (K$_a$ of HF = 7.2 x 10$^{-4}$)

A buffer solution consisting of 0.60 M HF and 1.0 M KF (Ka of HF = 7.2 x 10$^-4$) is titrated by 0.2 mol HCl. After the HCl is added, there is 1 L of solution. Find the pH of the solution.

Find the pH of the buffer solution consisting of 0.100 M HONH$_2$ and 0.100 M HONH$_3^+$ (K$_b$ of HONH$_2$ = 1.1 x 10$^{-8}$), after .02 moles HCl is added to the buffer solution? (assume the final volume of the solution is 1 L)

10.00 mL of an unknown H$_2$CO$_3$ solution is titrated with 0.0500 M NaOH and it requires 15.67 mL to reach the end point. What is the concentration of the H$_2$CO$_3$ ?

H$_2$CO$_3$ + 2 NaOH $\longrightarrow$ Na$_2$CO$_3$ + 2 H$_2$O

Sketch the titration curve for 50.0 mL 0.1 M CH$_3$COOH, K$_a$ = 1.8 x 10$^{-5}$ with 0.1 M NaOH. Include points on your graph and an example calculation for the initial pH, the pH at half way to the equivalence point, the pH at the equivalence point and the pH after the equivalence point.