Question
Please can you give the "observation" of the preparation of Magnesium Hydroxide from the reaction between Magnesium Nitrate and Sodium Hydroxide...
Answers
GPT-4o mini
When preparing magnesium hydroxide from the reaction between magnesium nitrate and sodium hydroxide, the following observations can typically be noted:
1. **Dissolution**: Magnesium nitrate (Mg(NO₃)₂) and sodium hydroxide (NaOH) are both typically soluble in water. When mixed, both compounds will dissolve, creating a clear solution initially.
2. **Formation of a Milky Suspension**: Upon mixing the two solutions, a cloudiness or turbidity will develop, indicating the formation of magnesium hydroxide (Mg(OH)₂). This compound is insoluble in water, leading to the formation of a milky white precipitate.
3. **Precipitate Formation**: The precipitate of magnesium hydroxide may settle at the bottom of the container if left undisturbed or may remain suspended, creating a milky solution. This indicates a successful precipitation reaction.
4. **Change in pH**: Since sodium hydroxide is a strong base, the solution will have a high pH, which can be tested with pH paper or a pH meter. This may also indicate the presence of excess hydroxide ions (OH⁻) in the solution.
5. **Final Mixture**: After some time, you can observe that the milky suspension remains, and if it's filtered, a clear filtrate will be obtained with the solid magnesium hydroxide left on the filter paper.
These observations confirm the production of magnesium hydroxide through the double displacement reaction between magnesium nitrate and sodium hydroxide. The overall reaction can be represented as follows:
\[ \text{Mg(NO}_3\text{)}_2 + 2\text{NaOH} \rightarrow \text{Mg(OH)}_2 \downarrow + 2\text{NaNO}_3 \]
(where the downward arrow indicates the formation of an insoluble precipitate).
1. **Dissolution**: Magnesium nitrate (Mg(NO₃)₂) and sodium hydroxide (NaOH) are both typically soluble in water. When mixed, both compounds will dissolve, creating a clear solution initially.
2. **Formation of a Milky Suspension**: Upon mixing the two solutions, a cloudiness or turbidity will develop, indicating the formation of magnesium hydroxide (Mg(OH)₂). This compound is insoluble in water, leading to the formation of a milky white precipitate.
3. **Precipitate Formation**: The precipitate of magnesium hydroxide may settle at the bottom of the container if left undisturbed or may remain suspended, creating a milky solution. This indicates a successful precipitation reaction.
4. **Change in pH**: Since sodium hydroxide is a strong base, the solution will have a high pH, which can be tested with pH paper or a pH meter. This may also indicate the presence of excess hydroxide ions (OH⁻) in the solution.
5. **Final Mixture**: After some time, you can observe that the milky suspension remains, and if it's filtered, a clear filtrate will be obtained with the solid magnesium hydroxide left on the filter paper.
These observations confirm the production of magnesium hydroxide through the double displacement reaction between magnesium nitrate and sodium hydroxide. The overall reaction can be represented as follows:
\[ \text{Mg(NO}_3\text{)}_2 + 2\text{NaOH} \rightarrow \text{Mg(OH)}_2 \downarrow + 2\text{NaNO}_3 \]
(where the downward arrow indicates the formation of an insoluble precipitate).