(a)[1]
Write down the molecular formula of sulfamic acid.
(b(i))[1]
Sulfamic acid is a weak acid. What does the term acid mean?
(b(ii))[2]
What is the distinction between a weak acid and a strong acid?
(c)[3]
What mass of sulfamic acid is needed to prepare $250\,\text{cm}^3$ of a $0.150\,\text{mol dm}^{-3}$ solution?
(d)[1]
In a titration, $0.00250$ moles of $\text{NaOH}$ are neutralised exactly by sulfamic acid with concentration $0.150\,\text{mol dm}^{-3}$. One mole of sodium hydroxide reacts with one mole of sulfamic acid. Calculate the volume, in $\text{cm}^3$, of sulfamic acid required for this titration.
(e)[2]
One mole of aqueous sulfamic acid yields one mole of hydrogen ions. Construct the equation to show how sulfamic acid reacts with magnesium.