Consider the sparingly soluble salt silver oxalate, Ag,C2O4. Assume a solution temperature of 25°C in all cases unless otherwise indicated. (a) Calculate the solubility, in mol·L of silver oxalate in distilled water at 25°C. You will need to look up the value of Ksp for silver oxalate in your textbook, the reference sheet from the previous solubility worksheet, or online. (b) Is the solubility of Ag,C,O4 at pH 3 expected to be greater than, less than, or equal to its solubility in distilled water at pH 7. Justify your answer using at least one chemical equation as part of your explanation. (c) Calculate the solubility, in mol·L of silver oxalate in the following solutions: (i) 0.200 M AgNO3 (ii) 0.150 M K2C2O4

Consider the sparingly soluble salt silver oxalate, Ag,C2O4. Assume a solution temperature of 25°C in all cases unless otherwise indicated. (a) Calculate the solubility, in mol·L of silver oxalate in distilled water at 25°C. You will need to look up the value of Ksp for silver oxalate in your textbook, the reference sheet from the previous solubility worksheet, or online. (b) Is the solubility of Ag,C,O4 at pH 3 expected to be greater than, less than, or equal to its solubility in distilled water at pH 7. Justify your answer using at least one chemical equation as part of your explanation. (c) Calculate the solubility, in mol·L of silver oxalate in the following solutions: (i) 0.200 M AgNO3 (ii) 0.150 M K2C2O4

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter15: Complex Ion And Precipitation Equilibria

Section: Chapter Questions

Problem 70QAP

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Question 1Consider the sparingly soluble salt silver oxalate, Ag2C2O4. Assume a solution temperature of 25°C in all cases unless otherwise indicated. (a) Calculate the solubility, in mol*L–1 of silver oxalate in distilled water at 25°C. You will need to look up the value of Ksp for silver oxalate in your textbook, the reference sheet from the previous solubility worksheet, or online. (b) Is the solubility of Ag2C2O4 at pH 3 expected to be greater than, less than, or equal to its solubility in distilled water at pH 7? Justify your answer using at least one chemical equation as part of your explanation. (c) Calculate the solubility, in mol*L–1 of silver oxalate in the following solutions: (i) 0.200 M AgNO3(ii) 0.150 M K2C2O4 Question 2Calculate the concentrations of all ions at equilibrium when 120.0 mL of 0.336 M Fe2(SO4)3 is mixed with 160.0 mL of 0.560 M KOH. You will need to identify the precipitate and look up the value of Ksp for that precipitate. Assume a temperature of at 25°C…
Hello I asked this question several times and your answers were wrong. please aware me if you do not know the answer. Calculate the solubility (in M) of cobalt(II) hydroxide, Co(OH)2(s) in H2O. Ksp = 1.00×10-16 at a specific temperature.
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