State the formula of the dilute acid that reacts with a metal carbonate to produce a nitrate salt.
Why is it necessary to add the iron(II) carbonate in excess in step 2?
State two observations in step 2 that would indicate iron(II) carbonate was present in excess.
Describe what should be done in step 3 to achieve the highest possible crystal yield.
A saturated solution is produced in step 4. Describe what is meant by a saturated solution.
Name a different compound that could replace iron(II) carbonate to make hydrated iron(II) sulfate crystals from dilute sulfuric acid.
Work out the value of $x$ by following these steps: find the mass of one mole of FeSO$_4$; find the mass of H$_2$O in one mole of FeSO$_4\cdot$xH$_2$O; determine the value of $x$.
State the name of the method used to make salts in this way.
Give the observation the student would make in step 1.
Write the ionic equation for the reaction between aqueous silver nitrate and aqueous potassium bromide. Include state symbols.
Calculate the volume of chlorine gas, in cm$^3$, that reacts to produce 2.34 g of NaCl.
Explain this in terms of structure and bonding.
Name the product formed at the positive electrode when electricity is passed through molten sodium chloride.
State the type of change that occurs at the positive electrode in (ii). Explain your answer in terms of electron transfer.
Describe what else can be done to sodium chloride so that it can conduct electricity.