Standardization of 0.10 M HCl 1. Take three (3) clean and properly labeled 250-mL Erlenmeyer flasks. Into the three flasks, weigh 0.1 g of the primary standard Na2CO3 to the nearest 0.1 mg. Record the weights of the primary standard. 2. Add about 75.0 mL of boiled distilled water and swirl to dissolve the solids. 3. Add 2 to 3 drops of phenolphthalein indicator. Record the initial burette reading and titrate with the prepared 0.10 M HCl solution until phenolphthalein endpoint. 4. Record the final burette reading for each titration in your data sheet Determination of Ksp and Molar Solubility 1. Add Ca(OH)2 to 250.0 mL distilled water with stirring until equilibrium is achieved. 2. Filter the undissolved precipitate. Measure out 50.0 mL of the supernate into a 250-mL Erlenmeyer flask using a pipette. 3. Add a few drops of phenolphthalein indicator and titrate with standardized HCl solution until endpoint is achieved. 4. Record the volume the HCl solution used. Perform two more trials. Standardization of Hydrochloric Acid Solution Answer the concentrations in 3 significant figure. Primary Standard Used: Na2CO3 Formula Mass of 1º standard: 105.99 g/mol %purity of 1º standard: 95% Trial 1 2 3 1º Standard weight, g 0.1005 0.1001 0.0997 Net volume of HCl, mL 9.30 9.00 8.90 M HCl 0.194 0.199 0.201 Average M HCl 0.198 Answer the Ksp of Ca(OH)2, Average solubility, Average Ksp Determination of Ksp and Solubility of Ca(OH)2 Answer the concentrations, solubility, and Ksp in 3 significant figure. Trial 1 2 3 Volume of filtrate (mL) 50 50 50 Net volume of HCl, mL 11.2 11.2 11.4 [OH-], M [Ca 2+], M Solubility of Ca(OH)2 Ksp of Ca(OH)2 Average solubility Average Ksp Theoretical Ksp 5.50e-6 % error
Standardization of 0.10 M HCl 1. Take three (3) clean and properly labeled 250-mL Erlenmeyer flasks. Into the three flasks, weigh 0.1 g of the primary standard Na2CO3 to the nearest 0.1 mg. Record the weights of the primary standard. 2. Add about 75.0 mL of boiled distilled water and swirl to dissolve the solids. 3. Add 2 to 3 drops of phenolphthalein indicator. Record the initial burette reading and titrate with the prepared 0.10 M HCl solution until phenolphthalein endpoint. 4. Record the final burette reading for each titration in your data sheet Determination of Ksp and Molar Solubility 1. Add Ca(OH)2 to 250.0 mL distilled water with stirring until equilibrium is achieved. 2. Filter the undissolved precipitate. Measure out 50.0 mL of the supernate into a 250-mL Erlenmeyer flask using a pipette. 3. Add a few drops of phenolphthalein indicator and titrate with standardized HCl solution until endpoint is achieved. 4. Record the volume the HCl solution used. Perform two more trials. Standardization of Hydrochloric Acid Solution Answer the concentrations in 3 significant figure. Primary Standard Used: Na2CO3 Formula Mass of 1º standard: 105.99 g/mol %purity of 1º standard: 95% Trial 1 2 3 1º Standard weight, g 0.1005 0.1001 0.0997 Net volume of HCl, mL 9.30 9.00 8.90 M HCl 0.194 0.199 0.201 Average M HCl 0.198 Answer the Ksp of Ca(OH)2, Average solubility, Average Ksp Determination of Ksp and Solubility of Ca(OH)2 Answer the concentrations, solubility, and Ksp in 3 significant figure. Trial 1 2 3 Volume of filtrate (mL) 50 50 50 Net volume of HCl, mL 11.2 11.2 11.4 [OH-], M [Ca 2+], M Solubility of Ca(OH)2 Ksp of Ca(OH)2 Average solubility Average Ksp Theoretical Ksp 5.50e-6 % error
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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Standardization of 0.10 M HCl
1. Take three (3) clean and properly labeled 250-mL Erlenmeyer flasks. Into the three flasks, weigh 0.1 g of
the primary standard Na2CO3 to the nearest 0.1 mg. Record the weights of the primary standard.
2. Add about 75.0 mL of boiled distilled water and swirl to dissolve the solids.
3. Add 2 to 3 drops of phenolphthalein indicator. Record the initial burette reading and titrate with the
prepared 0.10 M HCl solution until phenolphthalein endpoint.
4. Record the final burette reading for each titration in your data sheet
Determination of Ksp and Molar Solubility
1. Add Ca(OH)2 to 250.0 mL distilled water with stirring until equilibrium is achieved.
2. Filter the undissolved precipitate. Measure out 50.0 mL of the supernate into a 250-mL Erlenmeyer flask
using a pipette.
3. Add a few drops of phenolphthalein indicator and titrate with standardized HCl solution until endpoint
is achieved.
4. Record the volume the HCl solution used. Perform two more trials.
Standardization of Hydrochloric Acid Solution
Answer the concentrations in 3 significant figure.
Primary Standard Used: Na2CO3
Formula Mass of 1º standard: 105.99 g/mol
%purity of 1º standard: 95%
| Trial | 1 | 2 | 3 |
|---|---|---|---|
| 1º Standard weight, g | 0.1005 | 0.1001 | 0.0997 |
| Net volume of HCl, mL | 9.30 | 9.00 | 8.90 |
| M HCl | 0.194 | 0.199 | 0.201 |
| Average M HCl | 0.198 |
Answer the Ksp of Ca(OH)2, Average solubility, Average Ksp
Determination of Ksp and Solubility of Ca(OH)2
Answer the concentrations, solubility, and Ksp in 3 significant figure.
| Trial | 1 | 2 | 3 |
|---|---|---|---|
| Volume of filtrate (mL) | 50 | 50 | 50 |
| Net volume of HCl, mL | 11.2 | 11.2 | 11.4 |
| [OH-], M | |||
| [Ca 2+], M | |||
| Solubility of Ca(OH)2 | |||
| Ksp of Ca(OH)2 | |||
| Average solubility | |||
| Average Ksp | |||
| Theoretical Ksp | 5.50e-6 | ||
| % error |
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