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Rus_ich [418]
3 years ago
15

The balanced equation for the reaction of aqueous Pb(ClO3)2 with aqueous NaI is Pb(ClO3)2(aq)+2NaI(aq)⟶PbI2(s)+2NaClO3(aq) What

mass of precipitate will form if 1.50 L of concentrated Pb(ClO3)2 is mixed with 0.200 L of 0.210 M NaI? Assume the reaction goes to completion. mass of precipitate:
Chemistry
1 answer:
ryzh [129]3 years ago
6 0

Answer : The mass of PbI_2 precipitate produced will be, 9.681 grams.

Explanation : Given,

Molarity of NaI = 0.210 M

Volume of solution = 0.2 L

Molar mass of PbI_2 = 461.01 g/mole

First we have to calculate the moles of NaI.

\text{Moles of }NaI=\text{Molarity of }NaI\times \text{Volume of solution}=0.210M\times 0.2L=0.042moles

Now we have to calculate the moles of PbI_2.

The balanced chemical reaction is,

Pb(ClO_3)_2(aq)+2NaI(aq)\rightarrow PbI_2(s)+2NaClO_3(aq)

From the balanced reaction we conclude that

As, 2 moles of NaI react to give 1 mole of PbI_2

So, 0.042 moles of NaI react to give \frac{0.042}{2}=0.021 moles of PbI_2

Now we have to calculate the mass of PbI_2.

\text{Mass of }PbI_2=\text{Moles of }PbI_2\times \text{Molar mass of }PbI_2

\text{Mass of }PbI_2=(0.021mole)\times (461.01g/mole)=9.681g

Therefore, the mass of PbI_2 precipitate produced will be, 9.681 grams.

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