The solubility of ammonium formate, NH4HCO2, in 100. g of water is 102 g at 0 °C and 546 g at 80 °C. A solution is prepared by dissolving NH4HCO₂ in 235 g of water until no more will dissolve at 80 °C. The solution is then cooled to 0 °C. What mass of NH4HCO2 precipitates? (Assume that no water evaporates and that the solution is not supersaturated.) Mass= 9

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**Solubility of Ammonium Formate**

The solubility of ammonium formate (\( \text{NH}_4\text{HCO}_2 \)) in 100 grams of water is as follows:
- 102 grams at 0°C
- 546 grams at 80°C

A solution is prepared by dissolving \(\text{NH}_4\text{HCO}_2\) in 235 grams of water until no more will dissolve at 80°C. The solution is then cooled to 0°C. Determine the mass of \(\text{NH}_4\text{HCO}_2\) that precipitates under these conditions.

**Assumptions:**
- No water evaporates
- The solution is not supersaturated

**Calculate the Precipitation Mass:**
Mass = [Input field for the answer]

**Options:**
- Submit Answer
- Try Another Version (2 attempts remaining)

This activity involves calculating how much of the solute will precipitate out of solution as temperature decreases from 80°C to 0°C, based on changes in solubility.
Transcribed Image Text:**Solubility of Ammonium Formate** The solubility of ammonium formate (\( \text{NH}_4\text{HCO}_2 \)) in 100 grams of water is as follows: - 102 grams at 0°C - 546 grams at 80°C A solution is prepared by dissolving \(\text{NH}_4\text{HCO}_2\) in 235 grams of water until no more will dissolve at 80°C. The solution is then cooled to 0°C. Determine the mass of \(\text{NH}_4\text{HCO}_2\) that precipitates under these conditions. **Assumptions:** - No water evaporates - The solution is not supersaturated **Calculate the Precipitation Mass:** Mass = [Input field for the answer] **Options:** - Submit Answer - Try Another Version (2 attempts remaining) This activity involves calculating how much of the solute will precipitate out of solution as temperature decreases from 80°C to 0°C, based on changes in solubility.
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