(i) State how the student knew the reaction had ended in step 1. (ii) Name the residue from step 2. (iii) A saturated solution is made in step 3. What is a saturated solution? (iv) Explain why magnesium sulfate crystals are formed in step 4.
(i) Calculate the moles of water removed. (ii) Calculate the moles of anhydrous magnesium sulfate left in the crucible. The $M_r$ of anhydrous magnesium sulfate is 120. (iii) Calculate the ratio of moles of anhydrous magnesium sulfate : moles of water. Give your answer as whole numbers. (iv) Suggest the formula of hydrated magnesium sulfate crystals.
Describe how you would obtain a pure dry sample of lead(II) sulfate crystals from lead(II) nitrate solution and sodium sulfate solution. Include the main steps in your answer.
Write the ionic equation for the reaction between lead(II) nitrate solution and sodium sulfate solution. Include state symbols.