RESULTS:

Volume and molarity of $Pb(N{O}_3{)}_2$ solution

Volume and molarity of $H_{2}S{O}_4$ solution

$15mL$&$0\mathrm{.}5M$

$15mL$&$0\mathrm{.}5M$

Mass of crucible

Mass of crucible $+$ plumbum sulphate

$(1^{st}$ Weigh $-$ before heating$)$

Mass of crucible $+$ plumbum sulphate

$(2^{nd}$ Weigh $-$ after heating$)$

Mass of crucible $+$ plumbum sulphate

$(3^{rd}$ Weigh$)$

Mass of plumbum sulphate precipitates formed

$(1$ mark$)$

QUESTIONS:

Write the balanced equation for the reaction.

$(1$ mark$)$

Assume that the experiment is conducted ideally with both reactants fully reacted. Determine which reactant is the limiting and excess, if any.

$(4$ marks$)$

Based on the same ideal condition set in Question $2,$ will the mass of plumbum sulphate increases if you use $20mLPb(N{O}_3{)}_2$ solution? Why?

$(2$ marks$)$

Based on your calculation in Question $2,$ how much plumbum sulphate you should actually get? Explain one $(1)$ possible reason why the mass that you calculated is different than the collected one.

$(3$ marks$)$

What is the percentage yield for plumbum sulphate in this experiment?

$(1$ mark$)$

If you use $Mg(N{O}_3{)}_2$ instead of $Pb(N{O}_3{)}_2,$ do you think the experiment may proceed accordingly using the same lab procedure? Explain. $($Hint: Check their solubility$)$

$(3$ marks$)$

The precipitate is required to be rinsed several times before filtration. Briefly discuss the reason$($s$)$ rinsing is required and whether the timing of rinsing $($before or during filtration$)$ makes any difference to the obtained precipitate.

$(2$ marks$)$

Discuss the pros and cons of burning the filter paper to obtain the precipitate versus drying it in the drying cabinet.

$(2$ marks$)$