Question

# When solutions of silver nitrate and potassium chloride are mixed, silver chloride precipitates out of solution...

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?

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

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

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