19. Select the correct name for the coordination compound with the formula: $\mathsf{K}_3[\mathsf{Fe}(\mathsf{C}_2\mathsf{O}_4)_3]$.
(A) Potassium trioxalate ferrate(III)
(B) Potassium tris(oxalato)iron(III)
(C) Potassium tris(oxalato)ferrate(III)
(D) Potassium trioxalate iron(III)
(E) Tripotassium tris(oxalato)ferrate(III)

20. An aqueous solution was prepared by dissolving 0.05 moles of aluminum sulfate in 1.00 kg of water. The freezing point of this solution is determined to be $-0.391^{\circ}\mathrm{C}$. (Kf for water is $1.86^{\circ}\mathrm{C} \cdot \mathrm{kg} / \mathrm{mol}$). Calculate the van't Hoff factor (i) for aluminum sulfate. (A) 5 (B) 4.2 (C) 3.6 (D) 2.1 (E) 1 

21. At $100^{\circ}\mathrm{C}$ and 1 atm, $100\mathrm{g}$ sodium azide (hint: a compound with a chemical formula of $\mathrm{NaN_7}$) was completely inflated, what is the volume (liters) of the nitrogen gas released from this sample? (A) >121 (B) 101-120 (C) 81-100 (D) 61-80 (E) 41-60 

22. Cerium(IV) ion is a strong oxidizing agent that accepts one electron to produce cerium(III) ion. A solution containing an unknown concentration of $Sn^{2+}$ ions was titrated with a solution containing $Ce^{4+}$ ions, which oxidize the $Sn^{2+}$ ions to $Sn^{4+}$ ions. In one titration $1.00\ \mathrm{L}$ of the unknown solution required $46.45\ \mathrm{mL}$ of a $0.1050\ \mathrm{M}\ Ce^{4+}$ solution to reach the stoichiometric point. $$ a\ Ce^{4+}(aq) + b\ Sn^{2+}(aq) \longrightarrow c\ Ce^{3+}(aq) + d\ Sn^{4+}(aq) $$ What is the closest concentration of $Sn^{2+}$ ions in the unknown solution? (A) $2.4 \times 10^{-3}$ (B) $2.4 \times 10^{-2}$ (C) $2.7 \times 10^{-3}$ (D) $2.7 \times 10^{-2}$ (E) $3.0 \times 10^{-3}$

23. For a $\mathrm{H}_2\mathrm{CO}_3$ solution at $25^{\circ}\mathrm{C}$, what is the fractions (in %) of HCO3- at pH 9.00?  H2CO3(aq)⇌H+(aq)+HCO3-(aq) Ka1=4.3×10-7 HCO3-(aq) ⇌H+(ag)+CO3-(aq)   Ka2 =4.8 x 10-11  (A) < 20 (B) 20-39 (C) 40-69 (D) 70-90 (E) >90

24. If $\mathrm{H}_3\mathrm{A}$ is a triprotic acid with $k_{a1} = 1 \times 10^{-4}$, $k_{a2} = 1 \times 10^{-8}$, $k_{a3} = 1 \times 10^{-14}$. What is the equilibrium concentrations of $[\mathrm{HA}^{2-}]$ in a $1.0\ \mathrm{M}\ \mathrm{H}_3\mathrm{A}$ aqueous solution? (A) $1 \times 10^{-7}$ (B) $1 \times 10^{-6}$ (C) $1 \times 10^{-10}$ (D) $1 \times 10^{-9}$ (E) $1 \times 10^{-8}$

25. A 50.0-mL sample of $0.10\ \mathrm{M}\ \mathrm{HCN}$ (if $K_a = 7 \times 10^{-10}$) is titrated with $0.10\ \mathrm{M}\ \mathrm{NaOH}$, what is the pH of the solution at the halfway point in the titration? (Select the closest pH) (A) $\sim 9$ (B) $\sim 10$ (C) $\sim 11$ (D) $\sim 12$ (E) $\sim 8$

26. What is the pH of a $1.0\ \mathrm{M}$ solution of $\mathrm{NaH_2PO_4}$? (For $\mathrm{H_3PO_4}$, $K_{a1} = 7.5 \times 10^{-3}$, $K_{a2} = 6.2 \times 10^{-8}$, and $K_{a3} = 4.8 \times 10^{-13}$). Select the closest pH. (A) $\sim 6$ (B) $\sim 5.5$ (C) $\sim 4$ (D) $\sim 4.5$ (E) $\sim 5$

27. What is the solubility (M) of solid AgCI in a 10.0 M NHs solution? AgCI(s)+2NH3(aq) ⇌Ag(NH3)2+ (aq)+CI -(aq) If K=2.8 X 10-3 Select the closest solubility (M). (A)~0.3 (B)~0.4 (C)〜0.5 (D)~0.6 (E)~0.7

28. For a reaction: A $\longrightarrow$ B(g) + C(g) was studied at two temperature and the following values of k were obtained. (Hint: Arrhenius equation: $ = A e?/RT). What is the value of Ea for this reaction? Select the closest Ea (in kJ/mol). (A) ~80 (B) ~100 (C) ~120 (D) ~140 (E) ~160

29. Select the right configuration assignment ($R$ or $S$) for the following two organic compounds.  (A) Compound I is S and compound II is R (B) Compound I is R and compound II is S (C) Compound I is R and compound II is R (D) Compound I is S and compound II is S (E) Can not determine

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