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VMariaS [17]
3 years ago
5

Calculate the mass of precipitate that forms when 250.0 mL of an aqueous solution containing 35.5 g of lead(II) nitrate reacts w

ith excess sodium iodide solution.
Chemistry
1 answer:
natulia [17]3 years ago
6 0
<h3><u>Answer;</u></h3>

= 49.42 g

<h3><u>Explanation;</u></h3>

The equation for the reaction between Lead (ii) nitrate and sodium iodide;

Pb(NO3)2(aq) + 2 NaI(aq) ---> 2NaNO3(aq) + PbI2(s)

The precipitate formed in this equation is Lead iodide

We first calculate the moles of lead nitrate;

Moles = mass/molar mass

           = 35.5 g/ 331.2 g/mol

           = 0.1072 moles

The mole ratio of Pb(NO3)2 : PbI2 is 1 : 1

Therefore; the number of moles of lead iodide is 0.1072 moles

Mass = moles × molar mass

         = 0.1072 moles × 461.01 g/mol

         <u>= 49.42 g</u>

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Answer:

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Explanation:

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Therefore we have the molecular formula:

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