Chapter 6 Laboratory: Separating Mixtures 119q: 3 The formula weight of anhydrous copper sulfate is 159.6 g/mol. How many moles of anhydrous copper sulfate were present in
your sample (line E of Table 6-7)?
q: 4 Would you expect the number of moles of hydrated copper sulfate and the number of moles of anhydrous copper sulfate to be
the same? Why or why not?
q: 5 Assuming that all of the mass loss (line F of Table 6-7) represented water of crystallization, how many moles of water are
present in hydrated copper sulfate for each mole of copper sulfate? (Hint: the formula weight of water is 18.015 g/mol. Divide the mass
loss by the formula weight of water to calculate the number of moles of water present in the hydrated sample. Divide that number by
the number of moles of copper sulfate to determine the proportion of water molecules to copper sulfate molecules and round the
result to the nearest whole number.)
q: 6 How closely did your experimental results correspond to the actual value of five molecules of water per molecule of copper
sulfate? Propose several explanations for any variation.