Question

In: Chemistry

81.5 mL of a 3.30 M sodium chloride solution were used to react completely with 89.0...

81.5 mL of a 3.30 M sodium chloride solution were used to react completely with 89.0 mL of an aqueous lead (II) nitrate solution. What is the molarity of the lead (II) nitrate solution?

Solutions

Expert Solution

Reaction

2NaCl+ Pb(NO3)2​ --------------->PbCl2 + 2NaNO3

molarity of Sodium chloride = (number of moles of sodium chloride)(1000)÷(volume of solution)

3.30M = (number of moles of sodium chloride)(1000)÷81.5

Number of moles of sodium chloride = 3.30M×81.5÷1000

Number of moles of sodium chloride = 0.26895mol

From the stoichiometry of the reaction

2 mole sodium chloride completely react with 1 mole of lead(ll) nitrate

So 1mole of sodium chloride completely react with 1/2 mole of lead (ll) nitrate

Hence 0.26895 mole of sodium chloride completely react with (1×0.26895)/2 mole of lead (ll) nitrate

Number of moles of lead (ll) nitrate = 1×0.26895/2

Number of moles of lead (ll) nitrate = 0.134475 mole

Molarity of Pb(NO3) = {number of moles of Pb(No3)}×1000÷volume of solution

Molarity of Pb(NO3) = (0.134475mol)×1000÷89.0

Molarity of Pb(NO3) = 1.5109M


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