Part A. Titration of Pure Saturated Ca(OH)2 Solutionsnip Trial 1 Trial 2 Volume of Ca(OH)2 solution used, mL Final HCl buret reading, mL Initial HCl buret reading, mL Volume of HCl solution used, mL Concentration of HCl solution used, M 25.0 25.0 21.3 40.5 0.0 21.3 21.3 19.2 0.05 0.05 Moles of HCl used 1.065 0.96 Moles of Ca(OH)2 solution Concentration of Ca(OH)2 solution, M Concentration of Ca2+ ions, M Concentration of OH- ions, M Ksp value for Ca(OH)2 Average Ksp value for Ca(OH)2 Sample Calculations: Moles = molarity X volume Moles = (21.3)(0.05) = 1.065

Part A. Titration of Pure Saturated Ca(OH)2 Solutionsnip Trial 1 Trial 2 Volume of Ca(OH)2 solution used, mL Final HCl buret reading, mL Initial HCl buret reading, mL Volume of HCl solution used, mL Concentration of HCl solution used, M 25.0 25.0 21.3 40.5 0.0 21.3 21.3 19.2 0.05 0.05 Moles of HCl used 1.065 0.96 Moles of Ca(OH)2 solution Concentration of Ca(OH)2 solution, M Concentration of Ca2+ ions, M Concentration of OH- ions, M Ksp value for Ca(OH)2 Average Ksp value for Ca(OH)2 Sample Calculations: Moles = molarity X volume Moles = (21.3)(0.05) = 1.065

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 74QAP: Fifty cm3 of 1.000 M nitrous acid is titrated with 0.850 M NaOH. What is the pH of the solution (a)...

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Fifty cm3 of 1.000 M nitrous acid is titrated with 0.850 M NaOH. What is the pH of the solution (a) before any NaOH is added? (b) at half-neutralization? (c) at the equivalence point? (d) when 0.10 mL less than the volume of NaOH to reach the equivalence point is added? (e) when 0.10 mL more than the volume of NaOH to reach the equivalence point is added? (f) Use your data to construct a plot similar to that shown in Figure 14.10 (pH versus volume NaOH added).
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