When solutions of silver nitrate and potassium chloride are mixed, silver chlori

Question

When solutions of silver nitrate and potassium chloride are mixed, silver chloride precipitates out of solution according to the equation AgNO_3(aq) + KCl(aq) rightarrow AgCl(s) + KNO_3(aq) What mass of silver chloride can be produced from 1.97 L of a 0.232 M solution of silver nitrate? Express your answer with the appropriate units. mass of AgCl = The reaction described in Part A required 3.65 L of potassium chloride. What is the concentration of this potassium chloride solution? Express your answer with the appropriate units.

Explanation / Answer

A)

mol of AgNO3 reacted = M*V

= 0.232 M * 1.97 L

= 0.457 mol

from reaction,

mol of AgCl formed = mol of AgNO3 reacted

= 0.457 mol

molar mass of AgCl = 143.3 g/mol

mass of AgCl = number of mol * molar mass

= 0.457 mol * 143.3 g/mol

=65.5 g

Answer: 65.5 g

B)

mol of AgNO3 reacted = M*V

= 0.232 M * 1.97 L

= 0.457 mol

from reaction,

mol of KCl formed = mol of AgNO3 reacted

= 0.457 mol

mol of KCl = M*V

0.457 = M * 3.65

M = 0.125 M

Answer: 0.125 M

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