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t follows that at equilibrium: mg of CuCl will exist in one liter of solution as a precipitate mg of CuCl will be dissolved in one liter of solution mg of precipitate and 41.1 mg of dissolved ions will be present in one lit easing the temperature would have no effect on solubiility

t follows that at equilibrium: mg of CuCl will exist in one liter of solution as a precipitate mg of CuCl will be dissolved in one liter of solution mg of precipitate and 41.1 mg of dissolved ions will be present in one lit easing the temperature would have no effect on solubiility

Chemistry for Engineering Students
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 12.92PAE: Consider the following system: 4NH3(g)+3O2(g)2N2(g)+6H2O(l)H=153.04kJ (a) How will the amount of...
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(Q46) Given that the molar solubility of copper (1) chloride (99.00 g/mol) at 25°C is 4.15 x 10-4 mol/L, it follows that at equilibrium: O 41.1 mg of CuCl will exist in one liter of solution as a precipitate 41.1 mg of CuCl will be dissolved in one liter of solution O 41.1 mg of precipitate and 41.1 mg of dissolved ions will be present in one liter of solution O Increasing the temperature would have no effect on solubiility O Diluting the solution would cause precipitation to begin
Transcribed Image Text:(Q46) Given that the molar solubility of copper (1) chloride (99.00 g/mol) at 25°C is 4.15 x 10-4 mol/L, it follows that at equilibrium: O 41.1 mg of CuCl will exist in one liter of solution as a precipitate 41.1 mg of CuCl will be dissolved in one liter of solution O 41.1 mg of precipitate and 41.1 mg of dissolved ions will be present in one liter of solution O Increasing the temperature would have no effect on solubiility O Diluting the solution would cause precipitation to begin
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