Question

g When aqueous solutions of and are mixed, a solid forms. Determine the mass of solid formed when 140.7 mL of 0.1000 M is mixed with an excess of an aqueous solution of .

Answer 1

The question is incomplete, the complete question is:

When aqueous solutions of NaCl and
`Pb(NO_3)_2` are mixed, a solid forms. Determine the mass of solid formed when 140.7 mL of 0.1000 M NaCl is mixed with an excess of an aqueous solution of

Answer: The mass of lead chloride produced is 1.96 g

Step-by-step explanation:

Molarity is defined as the amount of solute expressed in the number of moles present per liter of solution. The units of molarity are mol/L. The formula used to calculate molarity:

`\text{Molarity of solution}=\frac{\text{Moles of solute}* 1000}{ \text{Volume of solution (mL)}}` .....(1)

Given values:

Molarity of NaCl = 0.1000 M

Volume of the solution = 140.7 mL

Putting values in equation 1, we get:

`0.1000=\frac{\text{Moles of NaCl}* 1000}{140.7}\\\\\text{Moles of NaCl}=(0.1000* 140.7)/(1000)=0.01407mol`

The chemical equation for the reaction of NaCl and lead nitrate follows:

`Pb(NO_3)_2(aq)+2NaCl(aq)\rightarrow PbCl_2(s)+2NaNO_3(aq)`

By the stoichiometry of the reaction:

If 2 moles of NaCl produces 1 mole of lead chloride

So, 0.01407 moles of NaCl will produce =
`(1)/(2)* 0.01407=0.007035mol` of lead chloride

The number of moles is defined as the ratio of the mass of a substance to its molar mass.

The equation used is:

`\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}` ......(2)

Molar mass of lead chloride = 278.1 g/mol

Plugging values in equation 2:

`\text{Mass of lead chloride}=(0.007035mol* 278.1g/mol)=1.96g`

Hence, the mass of lead chloride produced is 1.96 g