Na2CO3 powder, explain how 0.150mol of Na2CO3 can be practically be obtained in the lab
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To obtain 0.150 mol of Na2CO3 powder in the lab, you can follow these steps:
1. Determine the molecular weight of Na2CO3:
- 2 mol of sodium (Na) weighs 2 x 23.0 g/mol = 46.0 g/mol
- 1 mol of carbon (C) weighs 1 x 12.0 g/mol = 12.0 g/mol
- 3 mol of oxygen (O) weighs 3 x 16.0 g/mol = 48.0 g/mol
- The molecular weight of Na2CO3 is 46.0 g/mol + 12.0 g/mol + 48.0 g/mol = 106.0 g/mol
2. Calculate the mass of Na2CO3 needed:
- Amount of Na2CO3 in mol = 0.150 mol
- Mass of Na2CO3 = Amount (in mol) x Molecular weight
- Mass of Na2CO3 = 0.150 mol x 106.0 g/mol = 15.9 g
3. Set up a balanced chemical equation to determine the reactants needed to produce Na2CO3:
- Sodium hydroxide (NaOH) + Carbon dioxide (CO2) → Sodium carbonate (Na2CO3) + Water (H2O)
4. Choose a suitable method to react the appropriate reactants to obtain Na2CO3:
- One common method is to react sodium hydroxide (NaOH) with carbon dioxide (CO2) gas in the presence of water to produce sodium carbonate (Na2CO3) and water (H2O).
5. Prepare the reaction mixture:
- Weigh out the calculated mass (15.9 g) of Na2CO3 powder. This is the theoretical yield.
6. Carry out the reaction:
- Dissolve the measured Na2CO3 powder in water to form a solution.
7. Filter and dry the product:
- Use a suitable filter to separate any insoluble impurities from the solution.
- Carefully evaporate the water from the filtered solution to obtain the solid Na2CO3 powder.
8. Weigh and verify the yield:
- Weigh the obtained solid Na2CO3 powder and compare it to the theoretical yield (15.9 g) to determine the percent yield.
Note: It is important to follow appropriate lab safety procedures and guidelines while performing chemical reactions in the laboratory.
To obtain 0.150 mol of Na2CO3 powder in the lab, you will need to follow these steps:
1. Calculate the molar mass of Na2CO3: Na has a molar mass of 22.99 g/mol, C has a molar mass of 12.01 g/mol, and O has a molar mass of 16.00 g/mol. So, the molar mass of Na2CO3 is (2 * 22.99) + 12.01 + (3 * 16.00) = 105.99 g/mol.
2. Determine the mass of Na2CO3 needed: Since the molar mass of Na2CO3 is 105.99 g/mol and you want to obtain 0.150 mol, you can calculate the mass using the formula: mass = molar mass * moles. Therefore, the required mass is 105.99 g/mol * 0.150 mol = 15.8985 g.
3. Weigh the required mass of Na2CO3: Use a balance to measure out the exact amount of Na2CO3 needed, which is 15.8985 g. Make sure to use proper safety precautions when handling chemicals in the lab.
4. Dissolve the Na2CO3 in a suitable solvent: Often, Na2CO3 is dissolved in water to form a solution. Add the weighed Na2CO3 powder to a suitable container and add enough water to dissolve it completely. Stir the mixture until the powder is fully dissolved.
5. Evaporate the solvent: If you need to obtain the Na2CO3 powder, you will need to evaporate the water or the solvent you used to dissolve the compound. This can typically be done by gently heating the solution in a suitable container, such as an evaporating dish or a beaker, until all the water has evaporated, leaving behind the Na2CO3 powder.
6. Collect the Na2CO3 powder: Once all the water has evaporated, you will be left with solid Na2CO3 powder. You can collect it using a spatula or a scraper, making sure to handle it safely and avoid any contamination.
By following these steps, you can practically obtain 0.150 mol of Na2CO3 powder in the lab.