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Pb(CIO4)2 + 2 Kcı → PbCl2 + 2 KCIOA A chemist mixes dilute solutions of lead (II) perchlorate and potassium chloride to precipitate lead (II) chloride (Ksp = 1.7 x 105). 4. Which of the following is the net ionic equation for the experiment described above? (A) (B) (C) (D) 2 CI' + Pb*2 → PBCI2(s) 2 K*1 + ClO.? → K½CIO«(s) 2 CIO,1 + Pb*2 → PbCl2(s) + 4 O2(g) 4 CI + Pb*4 → PBCI4(s)

Pb(CIO4)2 + 2 Kcı → PbCl2 + 2 KCIOA A chemist mixes dilute solutions of lead (II) perchlorate and potassium chloride to precipitate lead (II) chloride (Ksp = 1.7 x 105). 4. Which of the following is the net ionic equation for the experiment described above? (A) (B) (C) (D) 2 CI' + Pb*2 → PBCI2(s) 2 K*1 + ClO.? → K½CIO«(s) 2 CIO,1 + Pb*2 → PbCl2(s) + 4 O2(g) 4 CI + Pb*4 → PBCI4(s)

Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter4: Reactions In Aqueous Solution
Section: Chapter Questions
Problem 60QAP: Gold metal will dissolve only in aqua regia, a mixture of concentrated hydrochloric acid and...
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Pb(CIO4)2 + 2 KCI → PbCl2 + 2 KCIO4 A chemist mixes dilute solutions of lead (II) perchlorate and potassium chloride to precipitate lead (II) chloride (Ksp = 1.7 x 105). 4. Which of the following is the net ionic equation for the experiment described above? (A) (B) (C) (D) 2 CI' + Pb*2 → PbCl2(s) 2 K*1 + ClO, ? → K2CIOA(s) 2 ClO,1 + Pb+2 → PbCl2(s) + 4 02(g) 4 CI + Pb*4 → PbCla(s) 5. Within a factor of 10, what is the approximate molar solubility of PbCl2 in a solution of 0.20 M CI1 ions? 1.6 x 102 M (A) (B) (C) (D) 1.7 x 10$ M 5.0 x 103 M 4.0 x 10-4 M 6. Ethanoic acid (CH3COOH) has a much lower vapor pressure than ethanol (CH3CH2OH). What is the most reasonable explanation? (A) The polarizability of two oxygen atoms increases the London forces of attraction in ethanoic acid compared with ethanol. (B) Hydrogen bonding in ethanoic acid is the strongest attractive force and is mainly responsible for the observed data. (C) Both ethanol and ethanoic acid have an - OH, so the difference is the dipole of the second oxygen that increases the attractive forces. (D) Ethanol has an – OH group and can hydrogen bond; therefore, the London forces must cause the effect.
Transcribed Image Text:Pb(CIO4)2 + 2 KCI → PbCl2 + 2 KCIO4 A chemist mixes dilute solutions of lead (II) perchlorate and potassium chloride to precipitate lead (II) chloride (Ksp = 1.7 x 105). 4. Which of the following is the net ionic equation for the experiment described above? (A) (B) (C) (D) 2 CI' + Pb*2 → PbCl2(s) 2 K*1 + ClO, ? → K2CIOA(s) 2 ClO,1 + Pb+2 → PbCl2(s) + 4 02(g) 4 CI + Pb*4 → PbCla(s) 5. Within a factor of 10, what is the approximate molar solubility of PbCl2 in a solution of 0.20 M CI1 ions? 1.6 x 102 M (A) (B) (C) (D) 1.7 x 10$ M 5.0 x 103 M 4.0 x 10-4 M 6. Ethanoic acid (CH3COOH) has a much lower vapor pressure than ethanol (CH3CH2OH). What is the most reasonable explanation? (A) The polarizability of two oxygen atoms increases the London forces of attraction in ethanoic acid compared with ethanol. (B) Hydrogen bonding in ethanoic acid is the strongest attractive force and is mainly responsible for the observed data. (C) Both ethanol and ethanoic acid have an - OH, so the difference is the dipole of the second oxygen that increases the attractive forces. (D) Ethanol has an – OH group and can hydrogen bond; therefore, the London forces must cause the effect.
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