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1 Name: Class: Date: Unit 4 Practice Test Multiple Choice Identify the choice that best completes the statement or answers the question. 1) The balanced molecular equation for complete neutralization of H 2 SO 4 by KOH in aqueous solution is. A) 2H + (aq) + 2OH (aq) 2H 2 O (l) B) 2H+ (aq) + 2KOH (aq) 2H 2 O (l) + 2K + (aq) C) H 2 SO 4 (aq) + 2OH (aq) 2H 2 O (l) + SO 2 4 (aq) D) H 2 SO 4 (aq) + 2KOH (aq) 2H 2 O (l) + K 2 SO 4 (s) E) H 2 SO 4 (aq) + 2KOH (aq) 2H 2 O (l) + K 2 SO 4 (aq) 2) Aqueous potassium chloride will react with which one of the following in an exchange (metathesis) reaction? A) calcium nitrate B) sodium bromide C) lead nitrate D) barium nitrate E) sodium chloride 3) Aqueous solutions of a compound did not form precipitates with Cl, Br, I, SO 2 4, CO 2 3, PO 3 4, OH, or S 2. This highly water-soluble compound produced the foul-smelling gas H 2 S when the solution was acidified. This compound is. A) Pb(NO 3 ) 2 B) (NH 4 ) 2 S C) KBr D) Li 2 CO 3 E) AgNO 3 4) The net ionic equation for formation of an aqueous solution of NiI 2 accompanied by evolution of CO 2 gas via mixing solid NiCO 3 and aqueous hydriodic acid is. A) 2NiCO 3 (s) + HI (aq) 2H 2 O (l) + CO 2 (g) + 2Ni 2+ (aq) B) NiCO 3 (s) + I (aq) 2H 2 O (l) + CO 2 (g) + Ni 2+ (aq) + HI (aq) C) NiCO 3 (s) + 2H + (aq) H 2 O (l) + CO 2 (g) + Ni 2+ (aq) D) NiCO 3 (s) + 2HI (aq) 2H 2 O (l) + CO 2 (g) + NiI 2 (aq) E) NiCO 3 (s) + 2HI (aq) H 2 O (l) + CO 2 (g) + Ni 2+ (aq) + 2I (aq) 5) The net ionic equation for formation of an aqueous solution of Al(NO3)3 via mixing solid Al(OH)3 and aqueous nitric acid is. A) Al(OH) 3 (s) + 3HNO 3 (aq) 3H 2 O (l) + Al(NO 3 ) 3 (aq) B) Al(OH) 3 (s) + 3NO 3 (aq) 3OH (aq) + Al(NO 3 ) 3 (aq) C) Al(OH) 3 (s) + 3NO 3 (aq) 3OH (aq) + Al(NO 3 ) 3 (s) D) Al(OH) 3 (s) + 3H + (aq) 3H 2 O (l) + Al 3+ (aq) E) Al(OH) 3 (s) + 3HNO 3 (aq) 3H 2 O (l) + Al 3+ (aq) + NO 3 (aq) 1

2 Name: 6) The net ionic equation for the reaction between aqueous nitric acid and aqueous sodium hydroxide is. A) H + (aq) + HNO 3 (aq) + 2OH (aq) 2H 2 O (l) + NO 3 (aq) B) HNO 3 (aq) + NaOH (aq) NaNO 3 (aq) + H 2 O (l) C) H + (aq) + OH (aq) H 2 O (l) D) HNO 3 (aq) + OH (aq) NO 3 (aq) + H 2 O (l) E) H + (aq) + Na + (aq) + OH (aq) H 2 O (l) + Na + (aq) 7) Which one of the following is a diprotic acid? A) nitric acid B) chloric acid C) phosphoric acid D) hydrofluoric acid E) sulfuric acid 8) Which one of the following is a weak acid? A) HNO 3 B) HCl C) HI D) HF E) HClO 4 9) Sodium does not occur in nature as Na (s) because. A) it is easily reduced to Na B) it is easily oxidized to Na + C) it reacts with water with great difficulty D) it is easily replaced by silver in its ores E) it undergoes a disproportionation reaction to Na and Na + 10) A M K 2 SO 4 solution is produced by. A) dilution of ml of 1.00 M K 2 SO 4 to 1.00 L B) dissolving 43.6 g of K 2 SO 4 in water and diluting to a total volume of ml C) diluting 20.0 ml of 5.00 M K 2 SO 4 solution to ml D) dissolving 20.2 g of K 2 SO 4 in water and diluting to ml, then diluting 25.0 ml of this solution to a total volume of ml E) dilution of 1.00 ml of 250 M K 2 SO 3 to 1.00 L 11) You are given two clear solutions of the same unknown monoprotic acid, but with different concentrations. Which statement is true? A) There is no chemical method designed to tell the two solutions apart. B) It would take more base solution (per milliliter of the unknown solution) to neutralize the more concentrated solution. C) A smaller volume of the less concentrated solution contains the same number of moles of the acid compared to the more concentrated solution. D) If the same volume of each sample was taken, then more base solution would be required to neutralize the one with lower concentration. E) The product of concentration and volume of the less concentrated solution equals the product of concentration and volume of the more concentrated solution. 2

3 Name: 12) is an oxidation reaction. A) Ice melting in a soft drink B) Table salt dissolving in water for cooking vegetables C) Rusting of iron D) The reaction of sodium chloride with lead nitrate to form lead chloride and sodium nitrate E) Neutralization of HCl by NaOH 13) What are the spectator ions in the reaction between KOH (aq) and HNO 3 (aq)? A) K + and H + B) H + and OH C) K + and NO 3 D) H + and NO 3 E) OH only 14) The balanced net ionic equation for precipitation of CaCO 3 when aqueous solutions of Na 2 CO 3 and CaCl 2 are mixed is. A) 2Na + (aq) + CO 2 3 (aq) Na 2 CO 3 (aq) B) 2Na + (aq) + 2Cl (aq) 2NaCl (aq) C) Na + (aq) + Cl (aq) NaCl (aq) D) Ca + (aq) + CO 2 3 (aq) CaCO 3 (s) E) Na 2 CO 3 (aq) + CaCL 2 (aq) 2NaCl (aq) + CaCO 3 (s) 15) The spectator ions in the reaction between aqueous chloric acid and aqueous barium hydroxide are. A) OH and ClO 3 B) H +, OH, ClO 3, and Ba 2+ C) H + and OH D) H + and Ba 2+ E) ClO 3 and Ba 2+ 16) The spectator ions in the reaction between aqueous hydrofluoric acid and aqueous barium hydroxide are. A) OH, F, and Ba 2+ B) F and Ba 2+ C) OH and F D) Ba 2+ only E) H +, OH, F, and Ba 2+ 17) Of the following elements, is the only one that cannot be found in nature in its elemental form. Cu Hg Au Ag Na A) Cu B) Hg C) Au D) Ag E) Na 3

4 Name: 18) Of the following elements, is the most easily oxidized. oxygen fluorine nitrogen aluminum gold A) oxygen B) fluorine C) nitrogen D) aluminum E) gold 19) How many moles of K + are present in 343 ml of a 1.27 M solution of K 3 PO 4? A) B) 1.31 C) D) 3.70 E) ) Calculate the concentration (M) of sodium ions in a solution made by diluting 50.0 ml of a M solution of sodium sulfide to a total volume of ml. A) B) 4.37 C) D) E) ) The concentration (M) of an aqueous methanol produced when L of a 2.00 M solution was diluted to L is. A) B) C) D) E) ) How many grams of sodium chloride are there in 55.0 ml of a 1.90 M aqueous solution of sodium chloride? A) B) 6.11 C) 3.21 D) E) ) The molarity of a solution prepared by diluting ml of M aqueous K 2 Cr 2 O 7 to 500. ml is. A) 57.2 B) C) D) E)

5 Name: 24) A 17.5 ml sample of an acetic acid (CH 3 CO 2 H) solution required 29.6 ml of M NaOH for neutralization. The concentration of acetic acid was M. A) B) C) 134 D) 6.88 E) ) With which of the following will the Potassium ion form an insoluble salt? A) Phosphate B) Sulfate C) Sulfide D) Iodide E) Potassium will form soluble salts with all choices. 26) There are mol of bromide ions in L of a M solution of AlBr 3. A) B) C) D) E) ) What volume (ml) of a 5.45 M lead nitrate solution must be diluted to ml to make a 1.41 M solution of lead nitrate? A) 212 B) 6310 C) 3170 D) E) ) How many milliliters of a stock solution of 11.7 M HNO 3 would be needed to prepare L of M HNO 3? A) B) 21.4 C) 2.93 D) 46.8 E) ) Pure acetic acid (HC 2 H 3 O 2 ) is a liquid and is known as glacial acetic acid. Calculate the molarity of a solution prepared by dissolving ml of glacial acetic acid at 25 C in sufficient water to give ml of solution. The density of glacial acetic acid at 25 C is 1.05 g/ml. A) B) 42.0 C) D) E)

6 Name: 30) What mass (g) of CaF 2 is formed when 30.4 ml of M NaF is treated with an excess of aqueous calcium nitrate? A) B) 1.04 C) 1040 D) E) ) A 24.5 ml aliquot of M H 2 SO 4 (aq) is to be titrated with M NaOH (aq). What volume (ml) of base will it take to reach the equivalence point? A) 156 B) C) 77.9 D) 39.0 E) 4430 Numeric Response 1) How many grams of CH 3 OH must be added to water to prepare 175 ml of a solution that is 1.0 M CH 3 OH? 2) There are mol of bromide ions in L of a M solution of AlBr 3. 3) How many moles of Co 2+ are present in L of a M solution of CoI 2? Short Answer 1) The solvent in an aqueous solution is. True/False Indicate whether the statement is true or false. 1) Ca(OH) 2 is a strong base. 2) The compound HClO 4 is a weak acid. 3) HNO 2 is a strong acid. 4) The compound NH 4 Cl is a weak acid. 5) Ammonia is a strong base. 6

7 Unit 4 Practice Test Answer Section MULTIPLE CHOICE 1) ANS: E PTS: 1 DIF: 1 REF: Page Ref: 4.2 2) ANS: C PTS: 1 DIF: 2 REF: Page Ref: 4.2 3) ANS: B PTS: 1 DIF: 3 REF: Page Ref: 4.2 4) ANS: C PTS: 1 DIF: 4 REF: Page Ref: 4.2 5) ANS: D PTS: 1 DIF: 4 REF: Page Ref: 4.2 6) ANS: C PTS: 1 DIF: 3 REF: Page Ref: 4.2 7) ANS: E PTS: 1 DIF: 2 REF: Page Ref: 4.3 8) ANS: D PTS: 1 DIF: 1 REF: Page Ref: 4.3 9) ANS: B PTS: 1 DIF: 2 REF: Page Ref: ) ANS: C PTS: 1 DIF: 3 REF: Page Ref: ) ANS: B PTS: 1 DIF: 2 REF: Page Ref: ) ANS: C PTS: 1 DIF: 2 REF: Page Ref: ) ANS: C PTS: 1 DIF: 2 REF: Page Ref: ) ANS: D PTS: 1 DIF: 3 REF: Page Ref: ) ANS: E PTS: 1 DIF: 3 REF: Page Ref: ) ANS: D PTS: 1 DIF: 2 REF: Page Ref: ) ANS: E PTS: 1 DIF: 2 REF: Page Ref: ) ANS: D PTS: 1 DIF: 3 REF: Page Ref: ) ANS: B PTS: 1 DIF: 3 REF: Page Ref: ) ANS: D PTS: 1 DIF: 2 REF: Page Ref: ) ANS: C PTS: 1 DIF: 2 REF: Page Ref: 4.5 1

8 22) ANS: B PTS: 1 DIF: 3 REF: Page Ref: ) ANS: C PTS: 1 DIF: 2 REF: Page Ref: ) ANS: B PTS: 1 DIF: 3 REF: Page Ref: 4.6 OBJ: 4.6; G4 25) ANS: E PTS: 1 DIF: 1 REF: Page Ref: ) ANS: C PTS: 1 DIF: 3 REF: Page Ref: ) ANS: A PTS: 1 DIF: 3 REF: Page Ref: ) ANS: B PTS: 1 DIF: 3 REF: Page Ref: ) ANS: D PTS: 1 DIF: 4 REF: Page Ref: ) ANS: A PTS: 1 DIF: 4 REF: Page Ref: 4.5 OBJ: 4.6; G4 31) ANS: A PTS: 1 DIF: 4 REF: Page Ref: 4.6 OBJ: 4.6; G4 NUMERIC RESPONSE 1) ANS: 5.6 PTS: 1 DIF: 3 REF: Page Ref: 4.5 2) ANS: PTS: 1 DIF: 3 REF: Page Ref: 4.5 3) ANS: PTS: 1 DIF: 3 REF: Page Ref: 4.5 SHORT ANSWER 1) ANS: water PTS: 1 DIF: 1 REF: Page Ref: 4.1 2

9 TRUE/FALSE 1) ANS: T PTS: 1 DIF: 1 REF: Page Ref: 4.3 2) ANS: F PTS: 1 DIF: 2 REF: Page Ref: 4.3 3) ANS: F PTS: 1 DIF: 1 REF: Page Ref: 4.3 4) ANS: T PTS: 1 DIF: 2 REF: Page Ref: 4.3 5) ANS: F PTS: 1 DIF: 1 REF: Page Ref: 4.3 3

10 Unit 4 Practice Test [Answer Strip] ID : A _ C 6) _ C 12) _ D 18) _ B 24) _ E 1) _ E 7) _ C 13) _ E 25) _ C 2) _ D 8) _ D 14) _ B 19) _ C 26) _ B 3) _ B 9) _ E 15) _ D 20) _ A 27) _ C 4) _ C 10) _ D 16) _ C 21) _ B 28) _ D 5) _ B 11) _ E 17) _ B 22) _ D 29) _ C 23)

11 Unit 4 Practice Test [Answer Strip] ID : A _ A 30) _ A 31) _ T 1) _ F 2) _ F 3) _ T 4) _ F 5)

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