**Question:**For which of the mixtures will Ag₂SO₄(s) precipitate?**Options:**1. 150.0 mL of 0.10 M Na₂SO₄(aq) and 5.0 mL of 0.20 M AgNO₃(aq)2. 150.0 mL of 0.10 M Na₂SO₄(aq) and 5.0 mL of 0.30 M AgNO₃(aq)3. 150.0 mL of 0.10 M Na₂SO₄(aq) and 5.0 mL of 0.40 M AgNO₃(aq)4. 150.0 mL of 0.10 M Na₂SO₄(aq) and 5.0 mL of 0.50 M AgNO₃(aq)**Explanation for Educational Context:**The question aims to determine in which of the listed mixtures a precipitation reaction will occur, resulting in the formation of solid silver sulfate (Ag₂SO₄). This involves the interaction of sodium sulfate (Na₂SO₄) and silver nitrate (AgNO₃) in aqueous solutions, which can lead to the formation of a precipitate if the concentrations exceed the solubility product (Ksp) of Ag₂SO₄. Each option provides different molarities and volumes of the reactants, which students must evaluate to predict whether precipitation will occur.

First we have to write the equation of precipitation of Ag2SO4

Answered: For which of the mixtures will…

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Chemistry

For which of the mixtures will Ag,SO4(s) precipitate?

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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