Question
Write a laboratory report on mass and mole relationship in a chemical reaction including aim and objective, apparatus/chemicals, procedures, observations, conclusions and results
Answers
GPT-4o mini
# Laboratory Report on Mass and Mole Relationship in a Chemical Reaction
### Aim and Objective
The aim of this experiment is to investigate the relationship between mass and moles in a chemical reaction, specifically the reaction between sodium bicarbonate (NaHCO₃) and hydrochloric acid (HCl). The objective is to determine the molar mass of sodium bicarbonate by measuring the changes in mass during the reaction and to verify the stoichiometric ratios from the balanced chemical equation.
### Apparatus and Chemicals
**Apparatus:**
- Analytical balance
- Beakers (100 mL and 250 mL)
- Graduated cylinder
- Stirring rod
- Weighing paper
- Burette
- Pipette
- Safety goggles
- Gloves
**Chemicals:**
- Sodium bicarbonate (NaHCO₃) - 5g
- Hydrochloric acid (HCl) solution (1M) - 50 mL
- Distilled water
### Procedures
1. **Preparation of Sodium Bicarbonate:**
- Weigh 5 g of sodium bicarbonate using an analytical balance. Record the mass.
2. **Preparation of Hydrochloric Acid:**
- Using a graduated cylinder, measure 50 mL of 1M hydrochloric acid and transfer it into a 250 mL beaker.
3. **Conducting the Reaction:**
- Slowly add the weighed sodium bicarbonate into the hydrochloric acid solution in the beaker.
- Stir gently with a stirring rod to ensure complete reaction and observe the reaction.
4. **Measuring Changes in Mass:**
- Before adding the sodium bicarbonate, measure the combined mass of the beaker and hydrochloric acid.
- After adding sodium bicarbonate and ensuring the reaction is complete, measure the combined mass again.
5. **Recording Data:**
- Record all observations during the reaction, including any gas evolution (bubbles) and the change in mass of the system.
### Observations
- Upon the addition of sodium bicarbonate, vigorous bubbling was observed indicating the release of carbon dioxide gas (CO₂).
- The initial mass of the beaker with hydrochloric acid was recorded as X grams.
- After the reaction, the final mass of the beaker and the resulting solution was Y grams.
- The difference in mass (X - Y) indicated the mass of carbon dioxide gas released during the reaction.
### Results
- **Initial Mass of Beaker + HCl:** X grams
- **Final Mass of Beaker + Solution:** Y grams
- **Mass of CO₂ Released:** X - Y = Z grams
Using the balanced chemical equation:
\[ \text{NaHCO}_3 (s) + \text{HCl} (aq) \rightarrow \text{NaCl} (aq) + \text{H}_2\text{O} (l) + \text{CO}_2 (g) \]
- 1 mole of NaHCO₃ reacts with 1 mole of HCl to produce 1 mole of CO₂.
- The molar mass of NaHCO₃ = 84 g/mol.
We can calculate the moles of NaHCO₃ used:
\[
\text{Moles of NaHCO}_3 = \frac{5 \text{ g}}{84 \text{ g/mol}} \approx 0.0595 \text{ moles}
\]
Assuming complete reaction, the moles of CO₂ produced will also be approximately 0.0595 moles.
### Conclusions
The experiment successfully demonstrated the mass-mole relationship in the chemical reaction between sodium bicarbonate and hydrochloric acid. The decrease in mass observed due to the escape of carbon dioxide gas was consistent with the stoichiometry of the reaction. The calculated moles of sodium bicarbonate used matched the theoretical predictions based on the balanced chemical equation, validating the relationship between mass and moles in chemical reactions. Further experiments could involve varying concentrations of HCl to study their effect on the rate and extent of the reaction.
### Aim and Objective
The aim of this experiment is to investigate the relationship between mass and moles in a chemical reaction, specifically the reaction between sodium bicarbonate (NaHCO₃) and hydrochloric acid (HCl). The objective is to determine the molar mass of sodium bicarbonate by measuring the changes in mass during the reaction and to verify the stoichiometric ratios from the balanced chemical equation.
### Apparatus and Chemicals
**Apparatus:**
- Analytical balance
- Beakers (100 mL and 250 mL)
- Graduated cylinder
- Stirring rod
- Weighing paper
- Burette
- Pipette
- Safety goggles
- Gloves
**Chemicals:**
- Sodium bicarbonate (NaHCO₃) - 5g
- Hydrochloric acid (HCl) solution (1M) - 50 mL
- Distilled water
### Procedures
1. **Preparation of Sodium Bicarbonate:**
- Weigh 5 g of sodium bicarbonate using an analytical balance. Record the mass.
2. **Preparation of Hydrochloric Acid:**
- Using a graduated cylinder, measure 50 mL of 1M hydrochloric acid and transfer it into a 250 mL beaker.
3. **Conducting the Reaction:**
- Slowly add the weighed sodium bicarbonate into the hydrochloric acid solution in the beaker.
- Stir gently with a stirring rod to ensure complete reaction and observe the reaction.
4. **Measuring Changes in Mass:**
- Before adding the sodium bicarbonate, measure the combined mass of the beaker and hydrochloric acid.
- After adding sodium bicarbonate and ensuring the reaction is complete, measure the combined mass again.
5. **Recording Data:**
- Record all observations during the reaction, including any gas evolution (bubbles) and the change in mass of the system.
### Observations
- Upon the addition of sodium bicarbonate, vigorous bubbling was observed indicating the release of carbon dioxide gas (CO₂).
- The initial mass of the beaker with hydrochloric acid was recorded as X grams.
- After the reaction, the final mass of the beaker and the resulting solution was Y grams.
- The difference in mass (X - Y) indicated the mass of carbon dioxide gas released during the reaction.
### Results
- **Initial Mass of Beaker + HCl:** X grams
- **Final Mass of Beaker + Solution:** Y grams
- **Mass of CO₂ Released:** X - Y = Z grams
Using the balanced chemical equation:
\[ \text{NaHCO}_3 (s) + \text{HCl} (aq) \rightarrow \text{NaCl} (aq) + \text{H}_2\text{O} (l) + \text{CO}_2 (g) \]
- 1 mole of NaHCO₃ reacts with 1 mole of HCl to produce 1 mole of CO₂.
- The molar mass of NaHCO₃ = 84 g/mol.
We can calculate the moles of NaHCO₃ used:
\[
\text{Moles of NaHCO}_3 = \frac{5 \text{ g}}{84 \text{ g/mol}} \approx 0.0595 \text{ moles}
\]
Assuming complete reaction, the moles of CO₂ produced will also be approximately 0.0595 moles.
### Conclusions
The experiment successfully demonstrated the mass-mole relationship in the chemical reaction between sodium bicarbonate and hydrochloric acid. The decrease in mass observed due to the escape of carbon dioxide gas was consistent with the stoichiometry of the reaction. The calculated moles of sodium bicarbonate used matched the theoretical predictions based on the balanced chemical equation, validating the relationship between mass and moles in chemical reactions. Further experiments could involve varying concentrations of HCl to study their effect on the rate and extent of the reaction.