$[$You will need to look up $K_a,K_b,K_{sp}$ values; on the exam, these would be given to you$]$

SALTS

Determine if each anion acts as a weak base in aqueous solution. For the anions that are basic,

write an equation that shows how the anion acts as a base:

$B{r}^{-}$

$Cl{O}^{-}$

$C{N}^{-}$

$C{l}^{-}$

Determine if each cation is acidic or $pH$ neutral in aqueous solution. For the cations that are acidic,

write an equation that shows how the cation acts as an acid:

$N{H}_4^{+}$

$N{a}^{+}(aq)$

$C{o}^{3+}(aq)$

$C{H}_{3}N{H}_3^{+}$

Determine if each salt will form a solution that is acidic, basic or neutral:

$Al(N{O}_3{)}_3$

$C_2{H}_{5}N{H}_{3}N{O}_3$

$K_{2}C{O}_3$

Rbl

$N{H}_4$ClO

LEWIS ACIDS$/$BASES

Classify each species as a Lewis acid or Lewis base:

$F{e}^{3+}$

$B{H}_3$

$N{H}_3$

$F^{-}$

$BeC{l}_2$

$O{H}^{-}$

$B(OH{)}_3,C{N}^{-}$

COMMON ION$/$BUFFERS

A formic acid $(HCH{O}_2)$ solution has a $pH$ of $3\mathrm{.}25.$ Which of these substances raises the $pH$ of the

solution upon addition? Explain.

$HCl$

NaBr

$NaCH{O}_2$

$KCl$

Solve an equilibrium problem $($i$.$e$.$ use an ICE table$)$ to calculate the $pH$ of each solution:

a solution that is $0\mathrm{.}20M$ in $HCH{O}_2$ and $0\mathrm{.}15M$ in $NaCH{O}_2$

a solution that is $0\mathrm{.}16M$ in $N{H}_3$ and $0\mathrm{.}22M$ in $N{H}_{4}Cl$

Calculate the percent ionization of a $0\mathrm{.}13MHCH{O}_2$ solution in pure water and also in a solution

containing $0\mathrm{.}11MKCH{O}_2.$ Explain the difference in percent ionization in the two solutions.

Use the Henderson$-$Hesselbalch equation to calculate the $pH$ of each solution in problem $7$