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.

2).Preparing of Magnesium hydroxide.
Magnesium hydroxide is a white insoluble solid that is used as an antacid to relieve upset stomachs.Obtain it as solid.
a). Write a method.
b) Write balanced equation for the reaction used.
c) Net ionic equation:
d). observations:

Answer 1

### 2) Preparing of Magnesium Hydroxide

**a) Method:**
1. **Preparation of Solutions:**
- In a beaker, prepare a solution of sodium hydroxide (NaOH) by dissolving a specific amount in distilled water to obtain a 1.0 M solution.
- In another beaker, prepare a solution of magnesium sulfate (MgSO₄) or magnesium nitrate (Mg(NO₃)₂) using the same concentration (1.0 M).

2. **Mixing the Solutions:**
- Carefully measure equal volumes (e.g., 25 mL) of the sodium hydroxide solution and the magnesium sulfate or magnesium nitrate solution using a graduated cylinder or pipette.
- Pour the sodium hydroxide solution into a clean test tube, and then slowly add the magnesium sulfate or magnesium nitrate solution to it while stirring.

3. **Formation of Precipitate:**
- As the two solutions are mixed, a white precipitate of magnesium hydroxide (Mg(OH)₂) will form. Continue stirring until no more precipitate appears.

4. **Filtration:**
- Set up a funnel and filter paper in another test tube or beaker.
- Pour the mixture through the filter paper to separate the magnesium hydroxide precipitate from the remaining solution.
- Rinse the collected precipitate on the filter paper with distilled water to remove any remaining impurities and unreacted reagents.

5. **Drying the Precipitate:**
- Allow the magnesium hydroxide to air-dry, or gently dry it using a low heat source, such as an evaporating dish over a hot plate.

6. **Collect the Solid:**
- Once dry, carefully collect the white solid magnesium hydroxide for further use.

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**b) Balanced Equation for the Reaction:**
The balanced chemical equation for the reaction forming magnesium hydroxide is as follows:

\[
\text{MgSO}_{4 (aq)} + 2 \text{NaOH}_{(aq)} \rightarrow \text{Mg(OH)}_2 (s) + \text{Na}_2\text{SO}_4 (aq)
\]

or

\[
\text{Mg(NO}_{3})_2 (aq) + 2 \text{NaOH}_{(aq)} \rightarrow \text{Mg(OH)}_2 (s) + 2 \text{NaNO}_3 (aq)
\]

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**c) Net Ionic Equation:**
To write the net ionic equation, we focus on the species that undergo a change during the reaction.

Starting from magnesium sulfate and sodium hydroxide, the net ionic equation will be:

\[
\text{Mg}^{2+} (aq) + 2 \text{OH}^{-} (aq) \rightarrow \text{Mg(OH)}_2 (s)
\]

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**d) Observations:**
1. **Mixing Solutions:** On mixing sodium hydroxide and magnesium sulfate/magnesium nitrate, a white precipitate (magnesium hydroxide) forms immediately.
2. **Precipitate Appearance:** The precipitate appears as a fine white solid, which may clump together or settle in the bottom of the test tube.
3. **Filtration Process:** During filtration, the remaining liquid (filtrate) may appear clear if the precipitate is completely removed.
4. **Final Product:** After drying, the magnesium hydroxide appears as a white powder.
5. **Reaction Characteristics:** There is no noticeable gas evolution, and the reaction occurs at room temperature without significant heat release or absorption.

These steps outline the practical method for preparing magnesium hydroxide and documenting the relevant chemical reactions and observations.