How can the student tell that every last trace of ammonia has evolved?
What colour is the solution in the conical flask before hydrochloric acid is added, and at the end-point?
From the burette diagrams, fill in the table, tick the most reliable titrations, and work out the mean volume of hydrochloric acid used.
Calculate the number of moles of hydrochloric acid in the average volume of $0.100\,\text{mol dm}^{-3}$ hydrochloric acid.
Using the equation $\text{HCl} + \text{NaOH} \rightarrow \text{NaCl} + \text{H}_2\text{O}$, deduce how many moles of sodium hydroxide are present in $25.0\,\text{cm}^3$ of $T$.
Calculate the number of moles of sodium hydroxide in $250\,\text{cm}^3$ of $T$.
Calculate the number of moles of sodium hydroxide in $50\,\text{cm}^3$ of $2.00\,\text{mol dm}^{-3}$ sodium hydroxide.
By subtracting your answer to (e)(ii) from your answer to (f), calculate the number of moles of sodium hydroxide that reacts with $25.0\,\text{cm}^3$ of $R$.
Calculate the mass of ammonia formed from the original $25.0\,\text{cm}^3$ sample of $R$.
Calculate the mass of ammonia formed from $1\,\text{dm}^3$ of $R$.
Using your answer to (h)(ii), calculate the concentration of ammonium sulfate in $R$. [$A_r$: N, $14$; H, $1$]