Practice Exam - Chapter 4 #1 PDF

Practice exam - Chapter 4 #1 1. When 1.00 mole of each compound below is dissolved in 10.0 L of water, which solution would most likely contain the least number of ions dissolved in solution? qqugaaoooo A. NH3 B. NaOH C. H2C2O...

Practice exam - Chapter 4 #1 1. When 1.00 mole of each compound below is dissolved in 10.0 L of water, which solution would most likely contain the least number of ions dissolved in solution? qqugaaoooo A. NH3 B. NaOH C. H2C2O4 D. CH3CH2OH E. Pb(ClO3)2 2. Choose the only correct statement below in choices A-E. A. All strong electrolytes are water-soluble ionic compounds B. All water-soluble molecular compounds are strong electrolytes in water C. All water-soluble ionic compounds are strong electrolytes in water i D. All ionic compounds are strong electrolytes in water E. All water-soluble compounds are strong electrolytes in water 3. Which of the compounds below behaves as weak acids in water, yielding a weakly electrolytic solution? i. Acetic acid (CH3COOH) ii. Nitric acid (HNO3) iii. Sulfuric acid (H2SO4) iv. Hypochlorous acid (HClO) v. Hydrofluoric acid (HF) A. ii, iii, v B. i, iv C. iii, v D. i, ii, iv E. i, iv, v 4. Which pair of compounds when mixed in water results in the formation of a precipitate? A. MgCl2 and NaOH B. Ba(NO3)2 and (NH4)2S C. Hg(NO3)2 and KCl D. Hg2(C2H3O2)2 and Ca(NO3)2 E. None of the above 5. Which electrolyte and acid-base property best describes NH4Cl when dissolved in water? A. Weak electrolyte, strong acid B. Non-electrolyte, non-acid or basenoeauaat C. Strong electrolyte, weak acid D. Strong electrolyte, strong base E. Weak electrolyte, weak base Dr. Kroner Practice exam - Chapter 4 #1 6. Consider the metathesis reaction between silver(I) nitrate and calcium chloride. If 1.0 L of 1.0 M AgNO3 and 1.0 L of 1.0 M CaCl2 are mixed together, what are the molarities of all ions in the solution once the reaction is complete? Assume the final volume of the solution is 2.0 L. A. No ions remain in solution B. [Ag+] = 1.0 M , [NO3-] = 1.0 M , [Ca2+] = 1.0 M, [Cl-] = 2.0 M C. [Ag+] = none , [NO3-] = none , [Ca2+] = 0.50 M, [Cl-] = 0.50 M D. [Ag+] = 0.50 M , [NO3-] = 0.50 M , [Ca2+] = none, [Cl-] = none E. [Ag+] = none , [NO3-] = 0.50 M , [Ca2+] = 0.50 M, [Cl-] = 0.50 M 7. Sodium nitrite when dissolved in water results in a __________ solution because __________. A. Strongly acidic, nitrite ion completely reacts with water to form H+ ions B. Strongly basic, nitrite ion completelyAtallah reacts with water to form OH- ions C. Weakly basic, nitrite ion partially reacts with water to form OH- ions D. Weakly acidic, nitrite ion partially reacts with water to form H+ ions E. Neither acidic nor basic, nitrite ion does not react with water to form H+ or OH- ions 8. 2.57 g Pb(NO3)2 and 2.28 g of KI are mixed in water and react according to the below reaction. What is the maximum amount of PbI2 that may precipitate (in g)? [Molecular weights (amu): Pb(NO3)2 =331.2; KI=166.0; PbI2=461.0; KNO3=101.1] Pb(NO3)2 + 2 KI → PbI2 + 2 KNO3 A. 6.33 g B. 3.17 g C. 3.58 g D. 3.97 g E. 4.44 g 9. Consider the following ionic compounds and determine how many are soluble in water? i. BaSO4 ii. AgBr iii. Sr(NO3)2 iv. PbS v. Na2CO3 A. All are soluble B. Four are soluble C. Three are soluble D. Two are soluble E. None are soluble Dr. Kroner Practice exam - Chapter 4 #1 10. The net ionic reaction for the reaction between potassium chloride and lead(II) nitrate in water is_______. A. Pb+ (aq) + Cl- (aq) → PbCl (s) B. K+ (aq) + Cl- (aq) → KCl (aq) C. K+ (aq) + Cl- (aq) + Pb+ (aq) + (NO3-) (aq) → PbCl (s) + K+ (aq) + (NO3-) (aq) D. Pb2+ (aq) + 2 Cl- (aq) → PbCl2 (s) E. 2KCl (aq) + Pb(NO3)2 (aq) → PbCl2 (s) + 2 KCl (aq) 11. A 5.00 mL sulfuric acid solution of unknown molarity and a couple drops of an acid-base indicator are titrated using 2.19 M NaOH. If 16.25 mL of the NaOH solution is required to cause a color change, what is the molarity of the sulfuric acid solution? 2 NaOH (aq) + H2SO4 (aq) → Na2SO4 (aq) + 2 H2O (l) A. 0.712 M B. 0.356 M C. 3.56 M D. 7.12 M E. 5.25 M 12. How much PbSO4 (MW=303.3 amu) can be produced (in g) by the addition of 25 mL of 0.50 M solution of aluminum sulfate to excess lead(II) nitrate according to the below reaction? 3 Pb(NO3)2 (aq) + Al2(SO4)3 (aq) → 3 PbSO4 (s) + 2 Al(NO3)3 (aq) A. 3.8 g B. 11.4 g C. 3.00 g D. 1.26 g E. 1.50 g 13. Write the balanced acid-base reaction between nitric acid and calcium hydroxide. How much 0.0250 M HNO3 solution is needed (in mL) to fully react with (or titrate) 12.5 mL of a 0.0100 M Ca(OH)2 solution? A. 15.0 mL B. 20.0 mL C. 12.5 mL D. 5.00 mL E. 10.0 mL Dr. Kroner Practice exam - Chapter 4 #1 14. Sodium hypochlorite (NaClO), the active ingredient in bleach, is synthesized by the below reaction. Balance the reaction and determine how much Cl2 (in g) is needed to react with 60.0 g of NaOH? __ NaOH + __ Cl2 → __ NaCl + __ NaClO + __ H2O A. 14.6 g B. 26.6 g C. 53.2 g D. 106 g E. 142 g 15. A chemist has a 3.50 M NaOH solution. If 25.00 mL of this solution is added to an empty 500.0 mL volumetric flask and the flask is filled to the line with water, what is the concentration of the final solution? A. It is still 3.50 M B. 0.175 M C. 0.0875 M D. 0.350 M E. 0.00875 M 16. What is the oxidation number of sulfur in Na2S2O8? A. 3 B. 4 C. 7 D. 8 E. 14 17. According to the activity series, which metal(s) below would dissolve in a solution of Ni(NO3)2? A. Copper B. Manganese C. Zinc D. b and c E. all of the above 18. Write and balance the oxidation-reduction reaction between aluminum metal and nitric acid. How much 0.500 M HNO3 (in L) is needed to fully dissolve 27.0 g of Al (s)? A. 0.500 L B. 6.00 L C. 1.50 L D. 0.167 L E. 0.250 L Dr. Kroner