Effect of Common Ions on the Solubility of Ca(OH)2 Answer the concentrations and solubility in 3 significant figure. [Ca2+]total = [Ca2+]from Ca(OH)2 + [Ca2+]from CaCl2 Assume that 0.01M CaCl2 medium is exact.
Ionic Equilibrium
Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
Arrhenius Acid
Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
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 |
Complete the table below:
Effect of Common Ions on the Solubility of Ca(OH)2
Answer the concentrations and solubility in 3 significant figure.
[Ca2+]total = [Ca2+]from Ca(OH)2 + [Ca2+]from CaCl2
Assume that 0.01M CaCl2 medium is exact.
| Trial | 1 | 2 | 3 |
|---|---|---|---|
| Volume of filtrate (mL) | 50 | 50 | 50 |
| Net volume of HCl (mL) | 9.1 | 9.0 | 9.1 |
| [OH-] | |||
| [Ca 2+]total | |||
| Solubility of Ca(OH)2 | |||
| Average solubility |
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