**Question 4: Solubility of Silver Sulfate in Water**Silver sulfate is slightly soluble in water, represented by the following equilibrium reaction:\[ Ag_2SO_4(s) \leftrightarrow 2Ag^+(aq) + SO_4^{2-}(aq) \]The equilibrium constant, \( K_c \), at 298 K is \( 1.1 \times 10^{-5} \).**Problem Statement:**If 3.45 grams of silver sulfate is added to 1.75 liters of water, will it all dissolve? Show your work and explain your reasoning.**Solution Approach:**1. **Calculate the Molar Mass of Silver Sulfate (Ag_2SO_4):** \[ \text{Molar mass of } Ag = 107.87 \, \text{g/mol} \] \[ \text{Molar mass of } S = 32.07 \, \text{g/mol} \] \[ \text{Molar mass of } O = 16.00 \, \text{g/mol} \] \[ Molar\,mass\,of\,Ag_2SO_4 = (2 \times 107.87) + 32.07 + (4 \times 16.00) \] \[ = 215.74 + 32.07 + 64.00 \] \[ = 311.81 \, \text{g/mol} \]2. **Calculate the Number of Moles of Silver Sulfate (Ag_2SO_4):** \[ \text{Mass of Ag_2SO_4} = 3.45 \, \text{g} \] \[ \text{Moles of Ag_2SO_4} = \frac{3.45 \, \text{g}}{311.81 \, \text{g/mol}} \] \[ = 0.0111 \, \text{mol} \]3. **Determine the Solubility Product (K_sp) Expression:** The equilibrium expression for the solubility of Ag_2SO_4 is: \[ K_c = [Ag^+]^2 [SO_4^{2-}] \] Let \( x \) be the mol

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Answered: 298K). If 3.45g of silver sulfate is…

298K). If 3.45g of silver sulfate is added to 1.75L of water, will it l dissolve? Show your work/explain your reasoning.

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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