Question 1 Consider 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 1
Consider 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 2
Calculate 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 for all solutions.
Solve all parts in both questions. Ksp value for silver oxalate provided.
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