How do i do these? (1 Viewer)

Average Boreduser · Apr 17, 2023

I just need help w Part d)

jimmysmith560 · Apr 17, 2023

This is very similar to Question 23 (a) from the 2013 HSC exam. A difference is that the HSC paper's version of the question includes (aq) and (s) symbols for the species in the table, which this version of the question does not. Since my knowledge of chemistry is limited, I am unsure whether this affects the correct working/answers. However, I will still include the approach taken in the HSC exam, hoping that you find it useful.

$Pb\left(s\right)+2AgNO_3\left(aq\right)\:\rightarrow \: Pb\left(NO_3\right)_2\left(aq\right)+2Ag\left(s\right)$

$n_{Pb}=\frac{20.72\:g}{207.2\:g\:mol^{-1}}=0.1000\:mol$

$n_{Ag}=0.100\:L\:\times 1.00\:mol\:L^{-1}=0.100\:mol$

$\text{Mole ratio}\: Pb\::\:AgNO_3\:\text{is}\:1\::\:2$

$\therefore 0.100\:mol\:AgNO_3\:\text{and}\:0.0500\:mol\: Pb\:\text{used}$

Moles of remaining ions and solids:

$Pb^{2+}\left(aq\right)=0.0500\:mol$

$Ag^+\left(aq\right)=0\:mol$

$NO_3^{\:-}\left(aq\right)=0.100\:mol$

$Pb\left(s\right)=0.0500\:mol$

$Ag\left(s\right)=0.100\:mol$

I hope this helps!

Eagle Mum · Apr 18, 2023

Yes, it’s the same question. The ionic species are in dissolved in the aqueous solution and the solid state of each metal is uncharged.

How do i do these? (1 Viewer)

Average Boreduser

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Eagle Mum

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