Question
#Practical.
Material used:
1.0 M solutions of calcium chloride, sodium carbonate, magnesium nitrate, sodium hydroxide, sulphuric acid, sodium sulphates, ammonium sulphate, barium chloride, magnesium powder or ribbon,test tube and rack , filter paper, funnel, beakers, Bunsen burner or hot plate and evaporating dish.
1) .Preparing of calcium carbonate.
A calcium carbonate is a white insoluble solid occuring naturally as chalk , limestone, marble and calcite.It is a useful building material.Devise a way of making some calcium carbonate from the substance provided.Obtain it as a power.
a). Write a method.
b) Write balanced equation for the reaction used.
c) Net ionic equation:
d). observations:
Material used:
1.0 M solutions of calcium chloride, sodium carbonate, magnesium nitrate, sodium hydroxide, sulphuric acid, sodium sulphates, ammonium sulphate, barium chloride, magnesium powder or ribbon,test tube and rack , filter paper, funnel, beakers, Bunsen burner or hot plate and evaporating dish.
1) .Preparing of calcium carbonate.
A calcium carbonate is a white insoluble solid occuring naturally as chalk , limestone, marble and calcite.It is a useful building material.Devise a way of making some calcium carbonate from the substance provided.Obtain it as a power.
a). Write a method.
b) Write balanced equation for the reaction used.
c) Net ionic equation:
d). observations:
Answers
Answered by
GPT-4o mini
### 1) Preparation of Calcium Carbonate
#### a) Method:
**Materials Needed:**
- 1.0 M sodium carbonate solution (Na2CO3)
- 1.0 M calcium chloride solution (CaCl2)
- Test tube
- Beakers
- Stirring rod
**Procedure:**
1. Set up a clean work area and gather all necessary materials.
2. Measure 10 mL of the 1.0 M calcium chloride solution (CaCl2) in a clean test tube.
3. In another container, measure 10 mL of the 1.0 M sodium carbonate solution (Na2CO3).
4. Slowly add the sodium carbonate solution to the calcium chloride solution in the test tube while stirring gently with a stirring rod.
5. A white precipitate of calcium carbonate (CaCO3) will form upon mixing the two solutions.
6. Allow the mixture to stand for a few minutes to ensure complete precipitation.
7. Once precipitation is complete, use a filter paper and funnel to filter out the precipitate of calcium carbonate from the solution.
8. Rinse the precipitate with distilled water to remove any remaining impurities.
9. Transfer the collected calcium carbonate precipitate to an evaporating dish.
10. Dry the calcium carbonate in an oven or over a Bunsen burner until it becomes a fine white powder.
#### b) Balanced Equation for the Reaction Used:
The balanced chemical equation for the reaction between calcium chloride and sodium carbonate is:
\[ \text{CaCl}_2(aq) + \text{Na}_2\text{CO}_3(aq) \rightarrow \text{CaCO}_3(s) + 2\text{NaCl}(aq) \]
#### c) Net Ionic Equation:
To derive the net ionic equation, we first identify the ions in the reaction:
- Calcium ions: \(\text{Ca}^{2+}\)
- Chloride ions: \(\text{Cl}^-\)
- Sodium ions: \(\text{Na}^+\)
- Carbonate ions: \(\text{CO}_3^{2-}\)
The soluble ions (Na\(^+\) and Cl\(^-\)) do not participate in the precipitation reaction, and we can thus write the net ionic equation as follows:
\[ \text{Ca}^{2+}(aq) + \text{CO}_3^{2-}(aq) \rightarrow \text{CaCO}_3(s) \]
#### d) Observations:
- Upon mixing the two solutions (calcium chloride and sodium carbonate), a white precipitate of calcium carbonate (CaCO3) is immediately observed.
- The solution may appear cloudy due to the formation of the insoluble calcium carbonate.
- After filtration, the residual solid (calcium carbonate) collected on the filter paper is white and powdery.
- After drying, the calcium carbonate powder has a fine, white appearance.
### Notes:
- Safety precautions must be taken when handling chemicals (wear gloves and goggles).
- Dispose of waste solutions and the calcium carbonate properly according to local regulations.
#### a) Method:
**Materials Needed:**
- 1.0 M sodium carbonate solution (Na2CO3)
- 1.0 M calcium chloride solution (CaCl2)
- Test tube
- Beakers
- Stirring rod
**Procedure:**
1. Set up a clean work area and gather all necessary materials.
2. Measure 10 mL of the 1.0 M calcium chloride solution (CaCl2) in a clean test tube.
3. In another container, measure 10 mL of the 1.0 M sodium carbonate solution (Na2CO3).
4. Slowly add the sodium carbonate solution to the calcium chloride solution in the test tube while stirring gently with a stirring rod.
5. A white precipitate of calcium carbonate (CaCO3) will form upon mixing the two solutions.
6. Allow the mixture to stand for a few minutes to ensure complete precipitation.
7. Once precipitation is complete, use a filter paper and funnel to filter out the precipitate of calcium carbonate from the solution.
8. Rinse the precipitate with distilled water to remove any remaining impurities.
9. Transfer the collected calcium carbonate precipitate to an evaporating dish.
10. Dry the calcium carbonate in an oven or over a Bunsen burner until it becomes a fine white powder.
#### b) Balanced Equation for the Reaction Used:
The balanced chemical equation for the reaction between calcium chloride and sodium carbonate is:
\[ \text{CaCl}_2(aq) + \text{Na}_2\text{CO}_3(aq) \rightarrow \text{CaCO}_3(s) + 2\text{NaCl}(aq) \]
#### c) Net Ionic Equation:
To derive the net ionic equation, we first identify the ions in the reaction:
- Calcium ions: \(\text{Ca}^{2+}\)
- Chloride ions: \(\text{Cl}^-\)
- Sodium ions: \(\text{Na}^+\)
- Carbonate ions: \(\text{CO}_3^{2-}\)
The soluble ions (Na\(^+\) and Cl\(^-\)) do not participate in the precipitation reaction, and we can thus write the net ionic equation as follows:
\[ \text{Ca}^{2+}(aq) + \text{CO}_3^{2-}(aq) \rightarrow \text{CaCO}_3(s) \]
#### d) Observations:
- Upon mixing the two solutions (calcium chloride and sodium carbonate), a white precipitate of calcium carbonate (CaCO3) is immediately observed.
- The solution may appear cloudy due to the formation of the insoluble calcium carbonate.
- After filtration, the residual solid (calcium carbonate) collected on the filter paper is white and powdery.
- After drying, the calcium carbonate powder has a fine, white appearance.
### Notes:
- Safety precautions must be taken when handling chemicals (wear gloves and goggles).
- Dispose of waste solutions and the calcium carbonate properly according to local regulations.