Answered: Using the solubility product constant,…

Using the solubility product constant, calculate the minimum concentration of the sulfate ion needed to initiate the precipitation of calcium sulfate. (Calcium ion concentration is 0.30 M).

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Concept explainers

Ionic Equilibrium

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Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

Only 2 and 3 rd questions you have to solve as soon as possible

1. Write the complete chemical reaction with states and Ksp expressions for Ca+2 and Ag*
precipitated with sodium sulfate. (Hint, you must combine the cations with agents that leave
them soluble on the reactant side of the chemical reaction).
2. Using the solubility product constant, calculate the minimum concentration of the sulfate ion
needed to initiate the precipitation of calcium sulfate. (Calcium ion concentration is 0.30 M).
3. If a solution contains 0.30M Ca2 and 0.060 M Agt, what % of the calcium ion can be
precipitated out by the addition of sodium chloride, without co-precipitation occurring? (Hint:
you can try random percentages until you find your limit. That is, you can start a low or high
percentage and move upward or downward until you reach the co-precipitation limit).

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