1. The solution gives no apparent reaction with dilute hydrochloric acid
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1 Which of the following would have to be absent for the following statement to be true: (A) CO 3 (B) Cr 2 O 7 (C) NH 4 (D) Ba 2 (E) Al 3 1. The solution gives no apparent reaction with dilute hydrochloric acid 2. No odor can be detected when a sample of the solution is added drop by drop to a warm solution of sodium hydroxide. 3. No precipitate is formed when a dilute solution of H 2 SO 4 is added to a sample of the solution. 4. The net ionic equation for the reaction between silver carbonate and hydrochloric acid is: (A) Ag 2 CO 3 2 H 2Cl - 2AgCl H 2 O CO 2 (B) 2 Ag CO 3 2 H 2Cl - 2AgC; H 2 O CO 2 (C) CO 3 2H H 2 O CO 2 (D) Ag Cl - AgCl 5. Metallic copper is heated strongly with concentrated sulfuric acid. The products of this reaction are (A) CuSO 4 and H 2 (B) Cu 2, SO 2 and H 2 O (C) Cu 2, H 2, H 2 O (D) CuSO 4, H 2, and SO 2 (E) Cu 2. SO 3, and H 2 O 6. When 70 ml of 3 M Na 2 CO 3 is added to 30 ml of 1 M NaHCO 3, the resulting concentration of Na is: (A) 2 M (B) 2.4 M (C) 4 M (D) 4.5 M (E) 7 M 7. The net ionic equation for the reaction that occurs during the titration of nitrous acid with sodium hydroxide is: (A) HNO 2 Na OH - NaNO 2 H 2 O (B) HNO 2 NaOH Na - NO 2 H 2 O (C) H OH - H 2 O (D) HNO 2 H 2 O NO - 2 H 3 O (E) HNO 2 OH - NO - 2 H 2 O
2 8. A 20 ml sample of 0.2 M K 2 CO 3 solution is added to 30 ml of 0.4 M Ba(NO 3 ) 2 solution. Barium carbonate precipitates. The concentration of barium ion, Ba 2, in solution after reaction is: (A) 0.15M (B) 0.16 M (C) 0.2 M (D) 0.24M (E) M 9. What is the net ionic equation for the reaction that occurs when aqueous copper(ii) sulfate is added to excess 6 M ammonia? (A) Cu 2 SO 4 2 NH 4 2OH - (NH 4 ) 2 SO 4 Cu(OH) 2 (B) Cu 2 4NH 3 4 H 2 O Cu(OH) 4 4 NH 4 (C) Cu 2 2NH 3 2H 2 O Cu(OH) 2 2 NH 4 (D) Cu 2 2 2NH 3 H 2 O Cu(NH 3 ) Which of the following does not behave as an electrolyte when it is dissolved in water? (A) CH 3 OH (B) K 2 CO 3 (C) NH 4 Br (D) HI (E) CH 3 COONa 11. The metal calcium reacts with molecular hydrogen to form a compound. All of the following statements concerning this compound are true except: (A) Its formula if CaH 2 (B) It is ionic. (C) It is a solid at room temperature. (D) When added to water, it reacts to produce H 2 gas (E) When added to water, it forms an acidic solution. 12. The test for the presence of Ag in an unknown solution involves the treatment of the silver-ammonia complex with dilute hydrochloric acid. The appearance of a white precipitate at this point indicates the presence of silver ion in the original sample. The net ionic equation that represents this test is: (A) Ag(NH 4 ) 4 4H Ag 4NH 4 (B) Ag(NH 4 ) 4 Cl - AgCl 4NH 4 (C) Ag(NH 3 ) 4 Cl - AgCl 2NH 4 3Cl - (D) Ag(NH 3 ) 2 2H Cl - AgCl 2NH A white solid is observed to be insoluble in water, insoluble in excess ammonia solution, and soluble in dilute HCl. Which of the following compounds could the solid be? (A) CaCO 3 (B) BaSO 4 (C) Pb(NO 3 ) 2 (D) AgCl (E) Zn(OH) How many moles of solid Ba(NO 3 ) 2 should be added to 300 ml of 0.2 M Fe(NO 3 ) 3 to increase the concentration of NO 3 - ion to 1 M? (A) 0.06 (B) 0.12 (C) 0.24 (D) 0.30 (E) 0.40
3 15. A 1.0 L sample of an aqueous solution contains 0.1 mol of NaCl and 0.1 mole of CaCl 2. What is the minimum number of moles of AgNO 3 that must be added to the solution in order to precipitate all of the Cl - as AgCl?(assume that AgCl is insoluble.) (A) 0.1 mol (B) 0.2 mol (C) 0.3 mol (D) 0.4 mol (E) 0.6 mol 16. A 40.0 ml sample of 0.25 M KOH is added to 60.0 ml of 0.15 M Ba(OH) 2. What is the molar concentration of OH - (aq) in the resulting solution?(assume That the volumes are additive.) (A) 0.10M (B) 0.19M (C) 0.28M (D) 0.40 M (E) 0.55M 17. What is the final concentration of barium ions, Ba 2, in solution with 100 ml of 0.10 M BaCl 2 is mixed with 100 ml of 0.05M H 2 SO 4? (A) 0.00M (B) 0.012M (C) 0.025M (D) 0.075M (E) 0.10 M 18. When 100 ml of 1.0 M Na 3 PO 4 is mixed with 100 ml of 1.0 M AgNO 3, a yellow precipitate forms and Ag becomes negligibly small. Which of the following is the correct listing of the ions remaining in solution in order of increasing concentration? (A) PO 3-4 < NO - 3 < Na 3- (B) PO 4 < Na - < NO 3 (C) NO - 3 < PO 3-4 < Na (D) Na < NO < PO In a qualitative analysis for the presence of Pb 2, Fe 2. and Cu 2 ions in aqueous solution, which of the following will allow the separation of Pb 2 from the other ions at room temperature? (A) add Na 2 S (B) add HCl (C) add NaOH (D) add NH 3 (E) add HNO 3
4 For #20-23, refer to the reactions represented below. (A) H 2 SeO 4 (aq) 2Cl - (aq) 2H (aq) H 2 SeO 3 (aq) Cl 2 (g) H 2 O (l) (B) S 8 (s) 8O 2 (g) 8SO 2 (g) (C) 3Br 2 (aq) 6OH - (aq) 5Br - - (aq) BrO 3 (aq) 3H 2 O (l) (D) Ca 2 (aq) SO 4 (aq) CaSO 4 (s) (E) PtCl 4 (s) 2Cl - (aq) PtCl 6 (aq) 20.) A precipitation reaction 21.) A reaction that produces a coordination complex 22.) A reaction in which the reactant undergoes both oxidation and reduction. 23.) A combustion reaction. 24.) In the laboratory, H 2(g) can be produced by adding which of the following to 1M HCl (aq)? I. 1 M NH 3 (aq) II. Zn (s) III. NaHCO 3 (s) (A) I only (B) II only (C) III only (D) I & II only (E) I, II, & III 25.) 2NH 3 NH - 4 NH 2 In liquid ammonia, the reaction represented above occurs. In the reaction, NH 4 acts as (A) a catalyst (B) both an acid and a base (C) the conjugate acid of NH 3 (D) the reducing agent (E) the oxidizing agent 26.) A colorless solution is divided into three samples. The following tests were performed on samples of the solution. (1) Add H (aq) no change (2) Add NH 3 (aq) no change (3) Add SO 4 (aq) no change. Which of the following ions could be present in the solution at the concentration of 0.10 M? (a) Ni 2 (aq) (b) Al 3 (aq) (c) Ba 2 (aq) (d) Na (aq) (e) CO 3 (aq) 27.) A pure, white crystalline solid dissolves in water to yield a basic solution that liberates a gas when excess acid is added to it. On the basis of this information, the solid could be: (a) KNO 3 (b) K 2 CO 3 (c) KOH (d) KHSO 4 (e) KCl
5 Answers 1 A 2 C 3 D 4 A 5 B 6 D 7 E 8 B 9 D 10 A 11 E 12 D 13 A 14 A 15 C 16 C 17 C 18 A 19 B 20 D 21 E 22 C 23 B 24 B 25 C 26 D 27 - B
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