how to prepare 100cm3 of 1.0moldm3 copper sulphate and from this prepare 100cm3 of 0.1 moldm3 solution.similarly use the 0.1moldm3 to prepare a 0.05 moldm3 ,and the 0.05moldm3 solution to prepare 0.01 moldm3 and 0.001moldm3solution.

To prepare the solutions as per your requirements, you will need to perform a series of dilutions. Here's a step-by-step guide:

Preparing 100 cm³ of 1.0 mol/dm³ Copper Sulphate Solution:
1. Start with 1.0 mol/dm³ copper sulphate solution.
2. Calculate the volume of the stock solution needed using the dilution formula: C1V1 = C2V2.
- C1 = initial concentration (1.0 mol/dm³)
- V1 = initial volume (unknown)
- C2 = final concentration (1.0 mol/dm³)
- V2 = final volume (100 cm³)

Since C1 = C2, the volume required will be 100 cm³.

Preparing 100 cm³ of 0.1 mol/dm³ Copper Sulphate Solution:
1. Take the 1.0 mol/dm³ copper sulphate solution prepared earlier.
2. Calculate the volume of the stock solution needed using the dilution formula.
- C1 = initial concentration (1.0 mol/dm³)
- V1 = initial volume (100 cm³)
- C2 = final concentration (0.1 mol/dm³)
- V2 = final volume (100 cm³)

Using the dilution formula: C1V1 = C2V2
(1.0 mol/dm³)(100 cm³) = (0.1 mol/dm³)(V2)
V2 = (1.0 mol/dm³)(100 cm³) / (0.1 mol/dm³)
V2 = 1000 cm³

So, you will need 1000 cm³ of the 1.0 mol/dm³ solution to prepare 100 cm³ of 0.1 mol/dm³ copper sulphate solution.

Preparing 100 cm³ of 0.05 mol/dm³ Copper Sulphate Solution:
1. Take the 0.1 mol/dm³ copper sulphate solution prepared earlier.
2. Calculate the volume of the stock solution needed using the dilution formula.
- C1 = initial concentration (0.1 mol/dm³)
- V1 = initial volume (100 cm³)
- C2 = final concentration (0.05 mol/dm³)
- V2 = final volume (100 cm³)

Using the dilution formula: C1V1 = C2V2
(0.1 mol/dm³)(100 cm³) = (0.05 mol/dm³)(V2)
V2 = (0.1 mol/dm³)(100 cm³) / (0.05 mol/dm³)
V2 = 200 cm³

So, you will need 200 cm³ of the 0.1 mol/dm³ solution to prepare 100 cm³ of 0.05 mol/dm³ copper sulphate solution.

Preparing 100 cm³ of 0.01 mol/dm³ Copper Sulphate Solution:
1. Take the 0.05 mol/dm³ copper sulphate solution prepared earlier.
2. Calculate the volume of the stock solution needed using the dilution formula.
- C1 = initial concentration (0.05 mol/dm³)
- V1 = initial volume (100 cm³)
- C2 = final concentration (0.01 mol/dm³)
- V2 = final volume (100 cm³)

Using the dilution formula: C1V1 = C2V2
(0.05 mol/dm³)(100 cm³) = (0.01 mol/dm³)(V2)
V2 = (0.05 mol/dm³)(100 cm³) / (0.01 mol/dm³)
V2 = 500 cm³

So, you will need 500 cm³ of the 0.05 mol/dm³ solution to prepare 100 cm³ of 0.01 mol/dm³ copper sulphate solution.

Preparing 100 cm³ of 0.001 mol/dm³ Copper Sulphate Solution:
1. Take the 0.01 mol/dm³ copper sulphate solution prepared earlier.
2. Calculate the volume of the stock solution needed using the dilution formula.
- C1 = initial concentration (0.01 mol/dm³)
- V1 = initial volume (100 cm³)
- C2 = final concentration (0.001 mol/dm³)
- V2 = final volume (100 cm³)

Using the dilution formula: C1V1 = C2V2
(0.01 mol/dm³)(100 cm³) = (0.001 mol/dm³)(V2)
V2 = (0.01 mol/dm³)(100 cm³) / (0.001 mol/dm³)
V2 = 1000 cm³

So, you will need 1000 cm³ of the 0.01 mol/dm³ solution to prepare 100 cm³ of 0.001 mol/dm³ copper sulphate solution.

Remember to perform each dilution carefully, measuring the volumes accurately and using appropriate containers.

To prepare different concentrations of copper sulphate solutions, you will need to use the concept of molarity (mol/dm³) and dilution.

1. Preparing 100 cm³ of 1.0 mol/dm³ Copper Sulphate Solution:
To make a 1.0 mol/dm³ solution, you will need the following steps:
- Calculate the amount of copper sulphate needed. Molarity (M) is defined as the number of moles (mol) of solute divided by the volume (dm³) of the solution.
- 1.0 mouldm³ means you have 1.0 mol of copper sulphate in 1.0 dm³ of solution.
- Therefore, you need to dissolve 1.0 mole of copper sulphate in 1.0 dm³ (1000 cm³) of water.
- Measure 1.0 mole of copper sulphate accurately on a balance, dissolve it in a small volume of water, and then dilute it to a final volume of 100 cm³ with distilled water in a volumetric flask.

2. Preparing 100 cm³ of 0.1 mol/dm³ Copper Sulphate Solution:
To prepare a 0.1 mol/dm³ solution from the 1.0 mol/dm³ solution, you will perform a dilution:
- Dilution involves taking a known volume of a more concentrated solution and diluting it with a solvent to reach the desired concentration.
- To prepare 0.1 mol/dm³ from 1.0 mol/dm³, you will need to dilute the 1.0 mol/dm³ solution by a factor of 10.
- Take 10 cm³ of the 1.0 mol/dm³ copper sulphate solution and add it to a 100 cm³ volumetric flask.
- Add distilled water to reach the 100 cm³ mark.

3. Preparing 100 cm³ of 0.05 mol/dm³ Copper Sulphate Solution:
Again, you will use the dilution method to prepare this solution:
- Take 10 cm³ of the 0.1 mol/dm³ copper sulphate solution prepared in the previous step and add it to a 100 cm³ volumetric flask.
- Add distilled water to reach the 100 cm³ mark.

4. Preparing 100 cm³ of 0.01 mol/dm³ Copper Sulphate Solution:
Continuing the dilution process:
- Take 10 cm³ of the 0.05 mol/dm³ copper sulphate solution obtained in the previous step and add it to a 100 cm³ volumetric flask.
- Add distilled water to reach the 100 cm³ mark.

5. Preparing 100 cm³ of 0.001 mol/dm³ Copper Sulphate Solution:
- Finally, take 10 cm³ of the 0.01 mol/dm³ copper sulphate solution prepared in the previous step and add it to a 100 cm³ volumetric flask.
- Add distilled water to reach the 100 cm³ mark.

Remember to label each solution clearly with its concentration to avoid confusion. Also, when performing dilutions, make sure to mix well to ensure an even distribution of solute throughout the solution.

I don't think you mean moldm3. I think you omitted the / mark and you should have written mol/dm^3

You want 1 mol/dm^3 CuSO4. If that is CuSO4 (and not CuSO4.5H2O) then take 15.96 g CuSO4 in 100 cc.
To use this soln to prepare 0.1 mol/cm^3, use 10 cc and dilute to 100 cc.

Answer to the ques