Copper $$ _{( ext {II })} $$ nitrate $$ _{(\mathrm{aq})}+ $$ sodium hydroxide $$ _{(\mathrm{aq})} ightarrow $$ copper(II) hydroxide $$ _{(\mathrm{s})}+ $$ sodium $$ ^{ ext {nitrate }}(\mathrm{aq}) $$ Observations:

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Copper $$ _{(	ext {II })} $$ nitrate $$ _{(\mathrm{aq})}+ $$ sodium hydroxide $$ _{(\mathrm{aq})} ightarrow $$ copper(II) hydroxide $$ _{(\mathrm{s})}+ $$ sodium $$ ^{	ext {nitrate }}(\mathrm{aq}) $$ Observations:

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When copper(II) nitrate aqueous solution reacts with sodium hydroxide aqueous solution to form copper(II) hydroxide and sodium nitrate, several observable changes occur. Here are the typical observations for this reaction:

**Balanced Chemical Equation:**
$$ \text{Cu(NO}_3\text{)}_2\,(\text{aq}) + 2\,\text{NaOH}\,(\text{aq}) \rightarrow \text{Cu(OH)}_2\,(\text{s}) + 2\,\text{NaNO}_3\,(\text{aq}) $$

**Observations:**

1. **Color Change:**
   - **Copper(II) Nitrate Solution:** Initially, the copper(II) nitrate solution is typically a vibrant blue color due to the presence of Cu²⁺ ions.
   - **Reaction Mixture:** Upon addition of sodium hydroxide, the bright blue color may start to change as the reaction progresses.

2. **Precipitate Formation:**
   - **Copper(II) Hydroxide:** A distinct blue precipitate forms immediately upon mixing the two aqueous solutions. Copper(II) hydroxide is insoluble in water, resulting in the formation of this solid.

3. **Solution Clarity:**
   - **Post-Reaction Solution:** The remaining solution, now containing sodium nitrate, remains clear and colorless, as sodium nitrate is highly soluble in water.

4. **Temperature Change:**
   - **Exothermic Nature:** The reaction may release a small amount of heat, making the solution feel slightly warmer to the touch.

5. **Effervescence:**
   - **Gas Evolution:** Typically, no gas is evolved in this reaction under standard conditions, so no bubbling or effervescence is observed.

6. **pH Indicator (if used):**
   - **Increase in pH:** The addition of sodium hydroxide increases the pH of the solution, making it more basic. If a pH indicator is present, a color change corresponding to a higher pH may be observed.

**Summary of Observations:**
- Formation of a blue precipitate (Cu(OH)₂) indicating the production of copper(II) hydroxide.
- The solution becomes clearer as sodium nitrate remains dissolved.
- Slight increase in temperature due to an exothermic reaction.

These observations help confirm the occurrence of the double displacement reaction between copper(II) nitrate and sodium hydroxide, resulting in the formation of copper(II) hydroxide and sodium nitrate.
When copper(II) nitrate and sodium hydroxide are mixed, a blue precipitate of copper(II) hydroxide forms, and the solution becomes clear as sodium nitrate dissolves. The reaction is exothermic, releasing a small amount of heat, and the pH increases, making the solution more basic.

Copper \( _{(\text {II })} \) nitrate \( _{(\mathrm{aq})}+ \) sodium hydroxide \( _{(\mathrm{aq})} \rightarrow \) copper(II) hydroxide \( _{(\mathrm{s})}+ \) sodium \( ^{\text {nitrate }}(\mathrm{aq}) \) Observations:

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