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Construct the reaction table for mixing 25 mL of 0.12 M AgNO3 and 85 mL of 0.24 M K₂CrO4. (See the Selected Solubility Product Constants.) cation + anion mmol 65 mmol 5349 mmol mmol Reaction Table initial change final 0 X,X°→=← 2 Ag+ (aq) + CrO2 (aq) = Ag₂ CrO4(s) 2 Ag+ (aq) + CrO2(aq) = Ag2CrO4(s) 2 Ag^+(aq) + CrO_4^2-(aq) <=> Ag_2CrO_4(s) Correct. Greek mmol (a) What mass of precipitate forms? X g mmol 0 (b) What is the concentration of the excess reactant at equilibrium? M precipitate Enter the net ionic equation. (Use the lowest possible whole number coefficients. Include states-of-matter under the given conditions in your answer.) chemPad Help mmol x mmol X mmol (c) What is the concentration of the limiting reactant at equilibrium? (Base your answer on the solubility of the precipitate, not the stoichiometry of the reaction.) M

Construct the reaction table for mixing 25 mL of 0.12 M AgNO3 and 85 mL of 0.24 M K₂CrO4. (See the Selected Solubility Product Constants.) cation + anion mmol 65 mmol 5349 mmol mmol Reaction Table initial change final 0 X,X°→=← 2 Ag+ (aq) + CrO2 (aq) = Ag₂ CrO4(s) 2 Ag+ (aq) + CrO2(aq) = Ag2CrO4(s) 2 Ag^+(aq) + CrO_4^2-(aq) <=> Ag_2CrO_4(s) Correct. Greek mmol (a) What mass of precipitate forms? X g mmol 0 (b) What is the concentration of the excess reactant at equilibrium? M precipitate Enter the net ionic equation. (Use the lowest possible whole number coefficients. Include states-of-matter under the given conditions in your answer.) chemPad Help mmol x mmol X mmol (c) What is the concentration of the limiting reactant at equilibrium? (Base your answer on the solubility of the precipitate, not the stoichiometry of the reaction.) M

Chemistry
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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reaction table and part a-c

Selected Solubility Product Constants Substance Ksp at 25 °C Aluminum Al(OH)3 Barium Ba(OH)2 BaCO3 BaSO4 Ba3(PO4)2 Cadmium Cd(OH)2 CdCO3 CdS Calcium Ca(OH)2 CaCO3 Ca3(PO4)2 CaF2 Cr(OH)3 Cobalt Co(OH)2 COS Chromium Copper Cu(OH)2 Cu₂S CuCO3 CuS 1.9 × 10-33 Iron Fe(OH)2 FeS Fe(OH)3 FePO4 5.0 × 10-3 8.1 x 10-9 1.1 x 10-10 3.4 x 10-23 2.5 x 10-14 5.2 x 10-12 8.0 × 10-27 5.5 x 10-6 4.8 x 10-9 1.0 × 10-26 3.9 × 10-11 6.3 × 10-31 1.6 × 10-15 4.0 × 10-21 2.2 X10-20 1.6 x 10-48 1.4 x 10-10 6.3 × 10-36 8.0 × 10-16 6.3 × 10-18 2.5 x 10-39 9.9 × 10-29 Substance Lead Pb(OH)2 PbF2 PbCl₂ PbBr2 Pbl₂ PbCrO4 PbSO4 PbS Mg(OH)2 Magnesium Mn(OH)2 MnCO3 MnS Nickel Ni(OH)2 Silver Manganese AgCl AgBr AgI AgCN Ag2S Ag2 CrO4 Ksp at 25 °C Ag3PO4 Tin Sn(OH)2 SnS 2.8 × 10-16 3.7 x 10-8 1.7 x 10-5 6.3 x 10-6 6.5 x 10-⁹ 1.8 x 10-14 1.7 x 10-8 8.4 x 10-28 Zinc ZnCO3 Zn(OH)2 ZnS 1.8 x 10-11 1.9 × 10-13 8.8 × 10-11 5.6 x 10-16 1.6 × 10-14 1.8 × 10-10 5.0 × 10-13 8.3 x 10-17 1.2 × 10-16 6.3 x 10-50 1.1 x 10-12 2.6 x10-18 1.4 x 10-28 1.3 x 10-23 1.0 x 10-10 4.5 x 10-17 1.1 x 10-21
Transcribed Image Text:Selected Solubility Product Constants Substance Ksp at 25 °C Aluminum Al(OH)3 Barium Ba(OH)2 BaCO3 BaSO4 Ba3(PO4)2 Cadmium Cd(OH)2 CdCO3 CdS Calcium Ca(OH)2 CaCO3 Ca3(PO4)2 CaF2 Cr(OH)3 Cobalt Co(OH)2 COS Chromium Copper Cu(OH)2 Cu₂S CuCO3 CuS 1.9 × 10-33 Iron Fe(OH)2 FeS Fe(OH)3 FePO4 5.0 × 10-3 8.1 x 10-9 1.1 x 10-10 3.4 x 10-23 2.5 x 10-14 5.2 x 10-12 8.0 × 10-27 5.5 x 10-6 4.8 x 10-9 1.0 × 10-26 3.9 × 10-11 6.3 × 10-31 1.6 × 10-15 4.0 × 10-21 2.2 X10-20 1.6 x 10-48 1.4 x 10-10 6.3 × 10-36 8.0 × 10-16 6.3 × 10-18 2.5 x 10-39 9.9 × 10-29 Substance Lead Pb(OH)2 PbF2 PbCl₂ PbBr2 Pbl₂ PbCrO4 PbSO4 PbS Mg(OH)2 Magnesium Mn(OH)2 MnCO3 MnS Nickel Ni(OH)2 Silver Manganese AgCl AgBr AgI AgCN Ag2S Ag2 CrO4 Ksp at 25 °C Ag3PO4 Tin Sn(OH)2 SnS 2.8 × 10-16 3.7 x 10-8 1.7 x 10-5 6.3 x 10-6 6.5 x 10-⁹ 1.8 x 10-14 1.7 x 10-8 8.4 x 10-28 Zinc ZnCO3 Zn(OH)2 ZnS 1.8 x 10-11 1.9 × 10-13 8.8 × 10-11 5.6 x 10-16 1.6 × 10-14 1.8 × 10-10 5.0 × 10-13 8.3 x 10-17 1.2 × 10-16 6.3 x 10-50 1.1 x 10-12 2.6 x10-18 1.4 x 10-28 1.3 x 10-23 1.0 x 10-10 4.5 x 10-17 1.1 x 10-21
Construct the reaction table for mixing 25 mL of 0.12 M AgNO3 and 85 mL of 0.24 M K₂CrO4. (See the Selected Solubility Product Constants.) Reaction Table initial change final 0 cation Greek mmol mmol mmol 2- 2 Ag+ (aq) + CrO₂²- (aq) = Ag₂CrO4(s) 2 Ag+ (aq) + CrO2- (aq) = Ag₂CrO4(s) 4 2 Ag^+(aq) + CrO_4^2-(aq) <=> Ag_2CrO_4(s) Correct. 65 (a) What mass of precipitate forms? x g anion mmol mmol mmol Enter the net ionic equation. (Use the lowest possible whole number coefficients. Include states-of-matter under the given conditions in your answer.) chemPad Help X₁X² → ← precipitate (b) What is the concentration of the excess reactant at equilibrium? M mmol X mmol X mmol (c) What is the concentration of the limiting reactant at equilibrium? (Base your answer on the solubility of the precipitate, not the stoichiometry of the reaction.) M
Transcribed Image Text:Construct the reaction table for mixing 25 mL of 0.12 M AgNO3 and 85 mL of 0.24 M K₂CrO4. (See the Selected Solubility Product Constants.) Reaction Table initial change final 0 cation Greek mmol mmol mmol 2- 2 Ag+ (aq) + CrO₂²- (aq) = Ag₂CrO4(s) 2 Ag+ (aq) + CrO2- (aq) = Ag₂CrO4(s) 4 2 Ag^+(aq) + CrO_4^2-(aq) <=> Ag_2CrO_4(s) Correct. 65 (a) What mass of precipitate forms? x g anion mmol mmol mmol Enter the net ionic equation. (Use the lowest possible whole number coefficients. Include states-of-matter under the given conditions in your answer.) chemPad Help X₁X² → ← precipitate (b) What is the concentration of the excess reactant at equilibrium? M mmol X mmol X mmol (c) What is the concentration of the limiting reactant at equilibrium? (Base your answer on the solubility of the precipitate, not the stoichiometry of the reaction.) M
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