CHEM 1127Q Lecture Notes - Lecture 11: Solution, Sodium Hydroxide, Sodium Chloride

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4. Solubility Rules and Precipitation Reactions. Do both problems .4A Imagine you have a solution containing a mixture of Mg2+(aq), Ba2+ (aq), Ag+ (aq) and NO3 - (aq) dissolved in the solution. You have available to you 5 different solutions containing the ions shown: Solution 1. Na+ (aq) and Cl- (aq) Solution 2. Na+ (aq) and OH- (aq) Solution 3. Na+ (aq) and SO4 2- (aq) Solution 4. Na+ (aq) and PO4 3- (aq) Solution 5. Na+ (aq) and NO3 - (aq) a. Which of the five solutions could you use to remove the Ba2+ as an insoluble solid, but leave the Mg2+ and the Ag+ dissolved in solution? Explain why you decided on your answer. b. Which of the five solutions could you use to remove the Mg2+ and the Ag+ as insoluble solids, but leave the Ba2+ dissolved in solution? Explain why you decided on your answer. 4B. Phosphoric acid, H3PO4 is added to aluminum sulfate, Al2(SO4)3 in water. The products are sulfuric acid, H2SO4, and aluminum phosphote, AlPO4. Write and balance this reaction, and use the table of solubility to determine the physical states of all of the reactants and products.

1. (10)What ions and/or molecules are present in relatively large proportions in a solution of a weak acid, HF (aq)? Select all appropriate answers. H+ HF F- HF+ F+ F2+ H2- F2- H F 2. (10)What ions and/or molecules are present in relatively large proportions in a solution of a strong base NaOH (aq)? Select all appropriate answers. NaOH Na2+ OH2- OH- NaO+ OH+ Na Na+ OH 3. (10)What ions and/or molecules are present in relatively large proportions in a solution of a strong acid HClO3 (aq)? Select all appropriate answers. HClO3 ClO3- HCl+ Cl+ H+ ClO3+ O3- O32- HCl None of these is present in relatively large proportions 4. (10)What ions and/or molecules are present in relatively large proportions in a solution of the soluble ionic compound NiCl2 (aq)? Select all appropriate answers. Ni2+ NiCl2 Cl22- Cl2- Ni+ Cl2- Ni Cl Cl2 Cl- 5. (5)Which of the following equations represents the proper net ionic equation for the precipitation of an insoluble sulfide compound from ZnBr2(aq) and Na2S(aq). Na2S(aq) + ZnBr2(aq) ----> 2 NaBr(aq) + ZnS(s) Zn2+(aq) + S2-(aq) ----> ZnS(s) Na2S(aq) + 2 Br-(aq) ----> 2 NaBr(s) + S2-(aq) Br-(aq) + Na+(aq) ----> NaBr(s) S2-(aq) + ZnBr2(aq) ----> ZnS(s) + 2 Br-(aq) 3 S2-(aq) + 2 Zn3+(aq) ----> Zn2S3(s) Na2+(aq) + Br2-(aq) ----> Na2Br2(s) Na2S(aq) + ZnBr2(aq) ----> Na2Br2(aq) + ZnS(s) Zn+(aq) + S-(aq) ----> ZnS(s) 6. (5)Which of the following equations represents the proper net ionic equation for the complete neutralization reaction between the strong acid HI(aq) and the weak base NH3(aq)? H+ (aq) + NH3(aq) ----> NH4+ (aq) HI (aq) + OH- (aq) ----> H2O (l) + I- (aq) HI (aq) + NH3(aq) ----> NH4I (aq) I- (aq) + NH4+ (aq) ----> NH4I (aq) H+ (aq) + OH- (aq) ----> H2O (l) HI (aq) + OH- (aq) ----> H2IO (aq) H+ (aq) + NH4+ (aq) ----> NH5+ (aq) I- (aq) + OH- (aq) ----> HIO (aq) mark 7. (5)What are the spectator ions in the solution after completely precipitating an insoluble carbonate compound when mixing Ca(ClO3)2 (aq) and Na2CO3 (aq)? Ca2+ , ClO3- , Na+ , and CO32- Na+ and CO32- CO32- and ClO3- CO32- and Ca2+ Ca2+ and ClO3- Ca2+ and Na+ Na+ ClO3- ClO3- and Na+ Ca2+ 8. (5)What are the spectator ions in the solution after the complete neutralization reaction occurs when mixing the weak acid H2S (aq) and the strong base KOH (aq)? H+ , S2- , K+ , and OH- OH- and K+ H+ and OH- OH- and S2- K+ and S2- K+ and H+ S2- and H+ K+ S2-

When equal molar amounts of these sets of compounds are mixed in aqueous solution, which will form a buffer solution? (A) HCl with NaCl (B) HCl with NaOH (C) NaOH with Na_2 CO_3 (D) NH_3 with NH_4 Cl The pH of a 0.0100 M solution of a weak acid, HA, is 3.76. What is the percent ionization of HA for this solution? (A) 0.017% (B) 0.58% (C) 1.7% (D) 5.8% Which is the most prevalent species in a 0.25 M aqueous solution of phosphoric acid, H_3 PO_4? (A) H_3 PO_4 (B) H_2 PO_4^- (C) HPO_4^2- (D) H_3 O^+ Which titration has an equivalence point with a basic pH? (A) titrating NH_3(aq) with HCl(aq) (B) titrating HNO_3(aq) with KOH(aq) (C) titrating HNO_2(aq) with KOH(aq) (D) titrating HClO_4 (aq) with Ca(OH)_2 (aq) Which figure best represents a concentrated aqueous solution of HI? (Water molecules are not shown.) A current of 0.150 A is passed through an aqueous CuSO_4 solution for 10.0 minutes. What mass of Cu is plated out? (Assume 100% yield.) (A) 0.000494 g (B) 0.0592 g (C) 0.0296 g (D) 0.0148 g The oxidation number of carbon changes from _____ in this redox reaction: 2NnO_4^- (aq) + 3C_2 O_4^2- (aq) + 4OH^- (aq) 2MNO_2 (s) + 6CO_3^2 (aq) + 2H O(I) (A) +6 to +4 (B) +4 and +3 (C) +3 to +4 (D) +3 to +6 Which species is the most powerful reducing agent at standard conditions? Na^+ (aq) + e^- rightarrow Na(s) E degree = -2.71 V Fe^2+ (aq) + 2e^- rightarrow Fe(s) E degree = -0.45 V O_2 (g) + 2H_2 O(l) + 4e^- rightarrow 4OH^- (aq) E degree = 0.40 V I_2 (s) + 2e^- rightarrow 2I^- (aq) E degree = 0.54 V (A) Na(s) (B) Fe^2+ (aq) (C) OH^- (aq) (D) I_2 (s) For this galvanic cell reaction 3HNO_2 (aq) + BrO_3^- (aq) rightarrow 3H^+(aq) + 3NO_3^- (aq) + Br^- (aq) the Nernst equation implies that the galvanic cell will have a more negative voltage if you: (A) increase the pH. (B) decrease the Br^- concentration (C) increase the BrO_3^-, concentration. (D) increase the NO_3^- concentration. The reaction Zn(s) + Ni^2+ (aq) rightarrow Zn^2 (aq) + Ni(s) occurs in the galvanic cell shown. Which statement is true? (A) Electrons flow to the Zn electrode. Na^+ ions flow toward the Ni electrode. (B) Electrons flow to the Zn electrode. Na^+ ions flow toward the Zn electrode. (C) Electrons flow to the Ni electrode. Na^+ ions flow toward the Ni electrode. (D) Electrons flow to the Ni electrode. Na^+ ions flow toward the Zn electrode.

CHEM 1127Q Lecture Notes - Lecture 11: Solution, Sodium Hydroxide, Sodium Chloride

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