**Precipitation Chemistry Problem****Question:**Will a precipitate be observed if 0.10 mol Ag⁺ and 0.001 mol SO₄²⁻ are added to make 1.0 L of solution? (Ksp = 1.4 × 10⁻⁵)**Options:**- ○ yes, because Q < Ksp- ○ no, because Q > Ksp- ○ no, because Q < KspWhen attempting to determine if a precipitate will form in a solution, it is essential to compare the ion product (Q) with the solubility product constant (Ksp). If Q > Ksp, a precipitate will form because the solution is supersaturated. If Q < Ksp, no precipitate will form because the solution is unsaturated. If Q = Ksp, the solution is at equilibrium and is saturated.**Calculation Process:**To solve this, first, determine the molar concentrations of Ag⁺ and SO₄²⁻ in the solution. Since the volume of the solution is 1.0 L:\[ [Ag^+] = \frac{0.10 \text{ mol}}{1.0 \text{ L}} = 0.10 \text{ M} \]\[ [SO₄²⁻] = \frac{0.001 \text{ mol}}{1.0 \text{ L}} = 0.001 \text{ M} \]Next, calculate the reaction quotient (Q) for the precipitation reaction:\[ Q = [Ag^+] \times [SO₄²⁻] \]\[ Q = (0.10 \text{ M}) \times (0.001 \text{ M}) \]\[ Q = 1.0 \times 10^{-4} \]Compare Q with the given Ksp:\[ Q = 1.0 \times 10^{-4} \]\[ Ksp = 1.4 \times 10^{-5} \]Since \( Q > Ksp \), the solution is supersaturated, and a precipitate will form. Therefore, the correct option is:- ○ no, because Q > Ksp

Here we are required to find whether precipitation will occur or not

Answered: Will a precipitate be observed if 0.10…

Will a precipitate be observed if 0.10 mol Ag* and 0.001 mol SO4²- are added to make 1.0 L of solution? (Ksp = 1.4 x 10-5) yes, because Q < Ksp no, because Q > Ksp no, because Q < Ksp

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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