Question

When solutions of silver nitrate and potassium chloride are mixed, silver chloride precipitates out of solution according to the equation AgNO3(aq)+KCl(aq)→AgCl(s)+KNO3(aq).

A) What mass of silver chloride can be produced from 1.90 L of a 0.133 M solution of silver nitrate?

B) The reaction described in Part A required 3.67 L of potassium chloride. What is the concentration of this potassium chloride solution?

Please help!

Answer 1

A)

number of moles of AgNO3 = M(AgNO3)*V(AgNO3)

= 0.133 M * 1.90 L

= 0.2527 mol

from reaction,

mol of AgCl formed = mol of AgNO3 reacted

= 0.2527 mol

Molar mass of AgCl,

MM = 1*MM(Ag) + 1*MM(Cl)

= 1*107.9 + 1*35.45

= 143.35 g/mol

use:

mass of AgCl,

m = number of mol * molar mass

= 0.2527 mol * 1.434*10^2 g/mol

= 36.22 g

Answer: 36.2 g

B)

From reaction,

mol of KCl reacted = mol of AgNO3 formed

= 0.2527 mol

Now use:

mol of KCl = M(KCl)*V(KCl)

0.2527 mol = M(KCl) * 3.67 L

M(KCl) = 0.0689 M

Answer: 0.0689 M