1. Determine the molar mass of \(Na_2SO_4.10H_2O\).
- The molar mass of \(Na_2SO_4\) is approximately 142.04 g/mol.
- The molar mass of \(H_2O\) is approximately 18.02 g/mol.
- The formula \(Na_2SO_4.10H_2O\) indicates that there are 10 molecules of water for every molecule of \(Na_2SO_4\).
- Therefore, the molar mass of \(Na_2SO_4.10H_2O\) is:
$$142.04 \text{ g/mol} \text{ (for }Na_2SO_4) + 18.02 \text{ g/mol (for 10 H}_2\text{O)} $$
$$142.04 \text{ g/mol} + 180.2 \text{ g/mol} $$
$$322.24 \text{ g/mol}$$
2. Calculate the mole ratio of salt to water.
- The mole ratio of salt to water is the number of moles of salt for every mole of water in the compound.
- In \(Na_2SO_4.10H_2O\), there is one mole of \(Na_2SO_4\) for every 10 moles of \(H_2O\).
- Therefore, the mole ratio of salt to water is 1:10.
So, the mole ratio of salt to water in \(Na_2SO_4.10H_2O\) is 1:10. This ratio indicates that for every one mole of \(Na_2SO_4\), there are 10 moles of water molecules associated with the salt in this hydrated compound.
