**Problem Statement:**If the end point of the titration was calculated to have occurred at a volume of 17.32 mL and the concentration of the LiCl solution is 0.00387 M, calculate the moles of lithium chloride that reacted.**Solution:**To find the moles of lithium chloride (LiCl) that reacted, use the formula:\[\text{Moles of LiCl} = \text{Concentration (M)} \times \text{Volume (L)}\]**Given:**- Concentration of LiCl = 0.00387 M- Volume of solution = 17.32 mL = 0.01732 L (converted from mL to L)**Calculation:**\[\text{Moles of LiCl} = 0.00387 \, \text{M} \times 0.01732 \, \text{L} = 0.0000669 \, \text{moles}\]Therefore, the moles of lithium chloride that reacted are 0.0000669 moles. (5) If the concentration of AgNO₃ is 0.00503 M and the concentration of the LiCl solution is 0.00387 M, use the stoichiometry of your equation to predict the volume of lithium chloride needed to react with 9.98 mL of the silver nitrate solution.

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(4) If the end point of the titration was calculated to have occurred at a volume of 17.32 mL and the concentration of the LiCI solution is 0.00387 M, calculate the moles of lithium chloride that reacted

(4) If the end point of the titration was calculated to have occurred at a volume of 17.32 mL and the concentration of the LiCI solution is 0.00387 M, calculate the moles of lithium chloride that reacted

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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