Answer :
### 1. Calculate the mass of CuSO4.5H2O needed to make a 100ml of a 0.755M solution.
To prepare a 100ml (0.1 liters) solution with a concentration of 0.755M (Molar), we need to determine the mass of CuSO4.5H2O required. The molar mass of CuSO4.5H2O is 249.68 g/mol.
First, we calculate the number of moles of CuSO4.5H2O required:
[tex]\[ \text{Moles} = \text{Concentration (M)} \times \text{Volume (L)} \][/tex]
[tex]\[ \text{Moles} = 0.755 \, \text{M} \times 0.1 \, \text{L} \][/tex]
[tex]\[ \text{Moles} = 0.0755 \, \text{mol} \][/tex]
Next, we convert moles to mass using the molar mass:
[tex]\[ \text{Mass} = \text{Moles} \times \text{Molar Mass (g/mol)} \][/tex]
[tex]\[ \text{Mass} = 0.0755 \, \text{mol} \times 249.68 \, \text{g/mol} \][/tex]
[tex]\[ \text{Mass} \approx 18.85 \, \text{g} \][/tex]
So, the mass of CuSO4.5H2O needed is approximately 18.85 grams.
### 2. Determine the volume of 0.1M H2SO4 needed to dilute the acid to a concentration of 0.0002M with a final volume of 100ml.
To achieve a final concentration of 0.0002M from a 0.1M H2SO4 solution with a final volume of 100ml, we use the dilution formula [tex]\( C_1 V_1 = C_2 V_2 \)[/tex].
Given:
[tex]\[ C_1 = 0.1 \, \text{M} \][/tex]
[tex]\[ C_2 = 0.0002 \, \text{M} \][/tex]
[tex]\[ V_2 = 100 \, \text{ml} \][/tex]
Rearranging to solve for [tex]\( V_1 \)[/tex]:
[tex]\[ V_1 = \frac{C_2 \times V_2}{C_1} \][/tex]
[tex]\[ V_1 = \frac{0.0002 \, \text{M} \times 100 \, \text{ml}}{0.1 \, \text{M}} \][/tex]
[tex]\[ V_1 = \frac{0.02 \, \text{ml}}{0.1} \][/tex]
[tex]\[ V_1 = 0.2 \, \text{ml} \][/tex]
So, 0.2 ml of 0.1M H2SO4 is needed.
### 3. List all the equipment and glassware that will be used in this experiment.
- Beakers
- Graduated Cylinders
- Volumetric Flasks
- Pipettes
- Balance
- Stirring Rods
- Measuring Scoops
- Droppers
- Distilled Water
### 4. Write a paragraph on solution and solution preparation.
To prepare a 0.755M solution of CuSO4.5H2O, start by calculating the required mass of the compound using its molar mass along with the desired volume and concentration. Measure out 18.85 grams of CuSO4.5H2O and dissolve it in a 100ml volumetric flask filled with distilled water. Stir the solution thoroughly until the compound fully dissolves to ensure a homogeneous solution.
For the dilution of H2SO4, calculate the necessary volume of the 0.1M H2SO4 stock solution needed to achieve a final concentration of 0.0002M in a total volume of 100ml using the formula [tex]\( C_1V_1 = C_2V_2 \)[/tex]. Accurately measure out 0.2ml of the 0.1M H2SO4 and dilute it to 100ml with distilled water in a volumetric flask.
The equipment necessary for this experiment includes beakers, graduated cylinders, volumetric flasks, pipettes, a balance, stirring rods, measuring scoops, droppers, and distilled water. Each piece of equipment is essential to ensure precision and accuracy during the solution preparation process.
To prepare a 100ml (0.1 liters) solution with a concentration of 0.755M (Molar), we need to determine the mass of CuSO4.5H2O required. The molar mass of CuSO4.5H2O is 249.68 g/mol.
First, we calculate the number of moles of CuSO4.5H2O required:
[tex]\[ \text{Moles} = \text{Concentration (M)} \times \text{Volume (L)} \][/tex]
[tex]\[ \text{Moles} = 0.755 \, \text{M} \times 0.1 \, \text{L} \][/tex]
[tex]\[ \text{Moles} = 0.0755 \, \text{mol} \][/tex]
Next, we convert moles to mass using the molar mass:
[tex]\[ \text{Mass} = \text{Moles} \times \text{Molar Mass (g/mol)} \][/tex]
[tex]\[ \text{Mass} = 0.0755 \, \text{mol} \times 249.68 \, \text{g/mol} \][/tex]
[tex]\[ \text{Mass} \approx 18.85 \, \text{g} \][/tex]
So, the mass of CuSO4.5H2O needed is approximately 18.85 grams.
### 2. Determine the volume of 0.1M H2SO4 needed to dilute the acid to a concentration of 0.0002M with a final volume of 100ml.
To achieve a final concentration of 0.0002M from a 0.1M H2SO4 solution with a final volume of 100ml, we use the dilution formula [tex]\( C_1 V_1 = C_2 V_2 \)[/tex].
Given:
[tex]\[ C_1 = 0.1 \, \text{M} \][/tex]
[tex]\[ C_2 = 0.0002 \, \text{M} \][/tex]
[tex]\[ V_2 = 100 \, \text{ml} \][/tex]
Rearranging to solve for [tex]\( V_1 \)[/tex]:
[tex]\[ V_1 = \frac{C_2 \times V_2}{C_1} \][/tex]
[tex]\[ V_1 = \frac{0.0002 \, \text{M} \times 100 \, \text{ml}}{0.1 \, \text{M}} \][/tex]
[tex]\[ V_1 = \frac{0.02 \, \text{ml}}{0.1} \][/tex]
[tex]\[ V_1 = 0.2 \, \text{ml} \][/tex]
So, 0.2 ml of 0.1M H2SO4 is needed.
### 3. List all the equipment and glassware that will be used in this experiment.
- Beakers
- Graduated Cylinders
- Volumetric Flasks
- Pipettes
- Balance
- Stirring Rods
- Measuring Scoops
- Droppers
- Distilled Water
### 4. Write a paragraph on solution and solution preparation.
To prepare a 0.755M solution of CuSO4.5H2O, start by calculating the required mass of the compound using its molar mass along with the desired volume and concentration. Measure out 18.85 grams of CuSO4.5H2O and dissolve it in a 100ml volumetric flask filled with distilled water. Stir the solution thoroughly until the compound fully dissolves to ensure a homogeneous solution.
For the dilution of H2SO4, calculate the necessary volume of the 0.1M H2SO4 stock solution needed to achieve a final concentration of 0.0002M in a total volume of 100ml using the formula [tex]\( C_1V_1 = C_2V_2 \)[/tex]. Accurately measure out 0.2ml of the 0.1M H2SO4 and dilute it to 100ml with distilled water in a volumetric flask.
The equipment necessary for this experiment includes beakers, graduated cylinders, volumetric flasks, pipettes, a balance, stirring rods, measuring scoops, droppers, and distilled water. Each piece of equipment is essential to ensure precision and accuracy during the solution preparation process.
