What is the maximum mass of copper(ii) sulphate pentahydrate, CuSO4.5H2O, which could be obtained by crystallizing the solution?

Ar: H=1; O=16; S=32; Cu=63.5

I'm not looking for someone to do it all, although that would help. Just that someone could give me guidance and give me steps to get to the answer. Thanks

To calculate the maximum mass of copper(II) sulfate pentahydrate, CuSO4.5H2O, that can be obtained by crystallizing the solution, you need to follow these steps:

1. Determine the molar mass of CuSO4.5H2O:
- Cu has a molar mass of 63.5 g/mol.
- S has a molar mass of 32 g/mol.
- O has a molar mass of 16 g/mol.
- H has a molar mass of 1 g/mol.
Therefore, the molar mass of CuSO4.5H2O is (63.5 + 32 + (4 * 16) + (5 * (1 + 1 + 16))) g/mol.

2. Convert the given molar mass of CuSO4.5H2O to grams by multiplying it by Avogadro's number (6.022 x 10^23):
- This step is necessary to convert the molar mass to grams.

3. Calculate the moles of CuSO4.5H2O:
- Divide the given mass of the solution by the molar mass of CuSO4.5H2O.
- The given mass could be the mass of the solution or the mass of an individual compound present in the solution.

4. Since copper(II) sulfate pentahydrate, CuSO4.5H2O, contains one mole of CuSO4, calculate the moles of CuSO4:
- Multiply the moles of CuSO4.5H2O by the ratio of moles of CuSO4 to moles of CuSO4.5H2O (which is 1 mole of CuSO4 for 1 mole of CuSO4.5H2O).

5. Finally, calculate the mass of CuSO4:
- Multiply the moles of CuSO4 by the molar mass of CuSO4.

Following these steps will help you calculate the maximum mass of copper(II) sulfate pentahydrate, CuSO4.5H2O, that could be obtained by crystallizing the solution. Remember to consider the molar mass, moles, and ratios in the calculations.