Question
#Practical.
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:
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
GPT-4o mini
To prepare calcium carbonate (CaCO₃) from calcium oxide (CaO) and carbon dioxide (CO₂), you can follow the method below.
### a) Method:
**Materials Needed:**
- Calcium oxide (CaO) (also known as quicklime)
- Carbon dioxide (CO₂) (can be sourced from a gas cylinder or using a reaction that produces CO₂)
- Beaker or flask
- Stirring rod
- Heat source (if necessary)
- Weighing balance
- Safety gear (gloves, goggles, etc.)
**Procedure:**
1. **Weighing:** Measure a specific amount of calcium oxide (for example, 10 grams).
2. **Reaction Setup:** Place the weighed calcium oxide into a clean, dry beaker or flask.
3. **Carbon Dioxide Introduction:** Introduce carbon dioxide gas into the beaker containing calcium oxide. This can be done by bubbling CO₂ through the solid, or by exposing the solid to the gas from a gas cylinder.
4. **Stirring:** Stir the mixture using a stirring rod to ensure thorough mixing and reaction of the gas with the solid.
5. **Formation of Calcium Carbonate:** As CO₂ reacts with CaO, calcium carbonate will form. You may observe the formation of a white precipitate.
6. **Drying:** If you need the calcium carbonate in powdered form, filter the precipitate formed (if necessary) and allow it to dry. You can warm the product slightly to remove any residual moisture.
7. **Collection:** Collect the dried calcium carbonate powder into a labeled container for use.
### b) Balanced Equation for the Reaction:
The balanced chemical equation for the reaction between calcium oxide and carbon dioxide to form calcium carbonate is:
\[ \text{CaO (s)} + \text{CO}_2 \text{(g)} \rightarrow \text{CaCO}_3 \text{(s)} \]
### c) Net Ionic Equation:
In this reaction, there are no spectator ions, as the reactants form a solid product. Therefore, the net ionic equation is essentially the same as the balanced equation:
\[ \text{Ca}^{2+} \text{(aq)} + \text{CO}_3^{2-} \text{(aq)} \rightarrow \text{CaCO}_3 \text{(s)} \]
This assumes that the initial reaction involves the dissolution of CaO in water to produce Ca²⁺ ions, which are then reacted with CO₂.
### d) Observations:
- **Before Reaction:** The calcium oxide (CaO) appears as a white powder (if dry).
- **During Reaction:** Upon the introduction of CO₂, you may observe bubbling (effervescence) and possibly some cloudiness as calcium carbonate begins to form.
- **After Reaction:** A white precipitate of calcium carbonate forms, which may settle at the bottom of the beaker or flask. If filtered, the solid will remain as a fine white powder.
- **Final Product:** After drying, the calcium carbonate will appear as a fine, white, dry powder.
**Note:** Always conduct the experiment following proper lab safety protocols and dispose of chemicals responsibly.
### a) Method:
**Materials Needed:**
- Calcium oxide (CaO) (also known as quicklime)
- Carbon dioxide (CO₂) (can be sourced from a gas cylinder or using a reaction that produces CO₂)
- Beaker or flask
- Stirring rod
- Heat source (if necessary)
- Weighing balance
- Safety gear (gloves, goggles, etc.)
**Procedure:**
1. **Weighing:** Measure a specific amount of calcium oxide (for example, 10 grams).
2. **Reaction Setup:** Place the weighed calcium oxide into a clean, dry beaker or flask.
3. **Carbon Dioxide Introduction:** Introduce carbon dioxide gas into the beaker containing calcium oxide. This can be done by bubbling CO₂ through the solid, or by exposing the solid to the gas from a gas cylinder.
4. **Stirring:** Stir the mixture using a stirring rod to ensure thorough mixing and reaction of the gas with the solid.
5. **Formation of Calcium Carbonate:** As CO₂ reacts with CaO, calcium carbonate will form. You may observe the formation of a white precipitate.
6. **Drying:** If you need the calcium carbonate in powdered form, filter the precipitate formed (if necessary) and allow it to dry. You can warm the product slightly to remove any residual moisture.
7. **Collection:** Collect the dried calcium carbonate powder into a labeled container for use.
### b) Balanced Equation for the Reaction:
The balanced chemical equation for the reaction between calcium oxide and carbon dioxide to form calcium carbonate is:
\[ \text{CaO (s)} + \text{CO}_2 \text{(g)} \rightarrow \text{CaCO}_3 \text{(s)} \]
### c) Net Ionic Equation:
In this reaction, there are no spectator ions, as the reactants form a solid product. Therefore, the net ionic equation is essentially the same as the balanced equation:
\[ \text{Ca}^{2+} \text{(aq)} + \text{CO}_3^{2-} \text{(aq)} \rightarrow \text{CaCO}_3 \text{(s)} \]
This assumes that the initial reaction involves the dissolution of CaO in water to produce Ca²⁺ ions, which are then reacted with CO₂.
### d) Observations:
- **Before Reaction:** The calcium oxide (CaO) appears as a white powder (if dry).
- **During Reaction:** Upon the introduction of CO₂, you may observe bubbling (effervescence) and possibly some cloudiness as calcium carbonate begins to form.
- **After Reaction:** A white precipitate of calcium carbonate forms, which may settle at the bottom of the beaker or flask. If filtered, the solid will remain as a fine white powder.
- **Final Product:** After drying, the calcium carbonate will appear as a fine, white, dry powder.
**Note:** Always conduct the experiment following proper lab safety protocols and dispose of chemicals responsibly.