Part 2: Molar Solubility of Calcium Hydroxide in the Presence of a Common Ion Exact Titrations (5 pts) Concentration of HCl solution (mol/L) pH of sat'd Ca(OH)2 with added CaCl2 solution (eg 2) no 0.115 m/L 11.58 OH 0003 Late To Ho Titration Data I noti Titration 1 Titration 2 Titration 3* Volume of sat'd Ca(OH)2 with added 25.0 25.0 CaCl2 solution (mL) Burette reading, initial (mL) Burette reading, final (mL) Volume of HCl used (mL) 8.3ulay *Do a 3rd titration when the difference between the titration volumes is more than 0.5 mL. 0 8:3 8.3 (ra) komil gay ito 8.3 Analysis and Calculations (15 pts) Moles of HCI used Moles of OH in sat'd solution (moles) Molarity of OH, [OH] (mol/L) Molar solubility of Ca(OH)2 with added CaCl2 solution (mol/L) Solubility of Ca(OH)2 with added CaCl2 solution (grams/L) Average Molar Solubility (mol/L) Average Solubility (grams/L) bas elavlanA 4 9.5×10 9510-4 bazu u to soloM Com) JoM (Nom) gidalo? slot samYA 10) to vidalo (Nerang) villogyA Show ALL calculations Ksp = [Ca2+] [OH-]² Ca(OH)2 Ca²+ +20H

Part 2: Molar Solubility of Calcium Hydroxide in the Presence of a Common Ion Exact Titrations (5 pts) Concentration of HCl solution (mol/L) pH of sat'd Ca(OH)2 with added CaCl2 solution (eg 2) no 0.115 m/L 11.58 OH 0003 Late To Ho Titration Data I noti Titration 1 Titration 2 Titration 3* Volume of sat'd Ca(OH)2 with added 25.0 25.0 CaCl2 solution (mL) Burette reading, initial (mL) Burette reading, final (mL) Volume of HCl used (mL) 8.3ulay *Do a 3rd titration when the difference between the titration volumes is more than 0.5 mL. 0 8:3 8.3 (ra) komil gay ito 8.3 Analysis and Calculations (15 pts) Moles of HCI used Moles of OH in sat'd solution (moles) Molarity of OH, [OH] (mol/L) Molar solubility of Ca(OH)2 with added CaCl2 solution (mol/L) Solubility of Ca(OH)2 with added CaCl2 solution (grams/L) Average Molar Solubility (mol/L) Average Solubility (grams/L) bas elavlanA 4 9.5×10 9510-4 bazu u to soloM Com) JoM (Nom) gidalo? slot samYA 10) to vidalo (Nerang) villogyA Show ALL calculations Ksp = [Ca2+] [OH-]² Ca(OH)2 Ca²+ +20H

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

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 14Q: Consider the following pH curves for 100.0 mL of two different acids with the same initial...

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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).
A 0.2481 M solution of KOH is used to titrate 30.00 mL of 0.269 M hydrobromic acid. Assume that volumes are additive. (a) Write a balanced net ionic equation for the reaction that takes place during the titration. (b) What are the species present at the equivalence point? (c) What volume of KOH is required to reach the equivalence point? (d) What is the pH of the solution 1. before any KOH is added? 2. halfway to the equivalence point? 3. at the equivalence point?
A buffer is prepared by dissolving 0.062 mol of sodium fluoride in 127 mL of 0.0399 M hydrofluoric acid. Assume no volume change after NaF is added. Calculate the pH of this buffer.
Malonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid w ith NaOH, stoichiometric points occur at pH = 3.9 and 8.8. A 25.00-mL sample of malonic acid of unknown concentration is titrated with 0.0984 M NaOH, requiring 31.50 mL of the NaOH solution to reach the phenolphthalein end point. Calculate the concentration of the initial malonic acid solution. (Sec Exercise 113.)
Consider the following pH curves for 100.0 mL of two different acids with the same initial concentration each titrated by 0.10 M NaOH. a. Which plot represents a pH curve of a weak acid, and which plot is for a strong acid? How can you tell? Cite three differences between the plots that help you decide. b. In both cases the pH is relatively constant before the pH changes greatly. Does this mean that at some point in each titration each solution was a buffered solution? c. True or false? The equivalence point volume for each titration is the same. Explain your answer. d. True or false? The pH at the equivalence point for each titration is the same. Explain your answer.
When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.
Sketch two pH curves, one for the titration of a weak acid with a strong base and one for a strong acid with a strong base. How are they similar? How are they different? Account for the similarities and the differences.
Potassium hydrogen phthalate, known as KHP (molar mass = 204.22 g/mol), can be obtained in high purity and is used to determine the concentration of solutions of strong bases by the reaction HP(aq)+OH(aq)H2O(l)+P2(aq) If a typical titration experiment begins with approximately 0.5 g KHP and has a final volume of about 100 mL, what is an appropriate indicator to use? The pKa for HP is 5.51.
A 0.4000 M solution of nitric acid is used to titrate 50.00 mL of 0.237 M barium hydroxide. (Assume that volumes are additive.) (a) Write a balanced net ionic equation for the reaction that takes place during titration. (b) What are the species present at the equivalence point? (c) What volume of nitric acid is required to reach the equivalence point? (d) What is the pH of the solution before any HNO3 is added? (e) What is the pH of the solution halfway to the equivalence point? (f) What is the pH of the solution at the equivalence point?