When solutions of silver nitrate and sodium chloride are mixed, silver chloride

Question

When solutions of silver nitrate and sodium chloride are mixed, silver chloride precipitates out of solution according to the equation AgNO3(aq)+NaCl(aq)AgCl(s)+NaNO3(aq)

Part A What mass of silver chloride can be produced from 1.40 L of a 0.180 M solution of silver nitrate? Express your answer with the appropriate units.

Part B The reaction described in Part A required 3.98 L of sodium chloride. What is the concentration of this sodium chloride solution? Express your answer with the appropriate units.

Explanation / Answer

AgNO3(aq) + NaCl(aq) AgCl(s) + NaNO3(aq)

Part A. Volume of AgNO3 = 1.40 L

Molarity of AgNO3 = 0.180 M

Moles of AgNO3 = Molarity * Volume

= 0.180 * 1.40

= 0.252 moles

From reaction it is clear that 1 mole of AgNo3 reacts with 1 mole of NaCl and produce 1 mole of AgCl.

So, moles of AgCl produced = 0.252 moles

Molar mass of AgCl = 143.32 g/mol

Mass of AgCl produced = Moles * Molar mass

= 0.252 * 143.32

= 36.11 g

Part B. Volume of NaCl required = 3.98 L

From part A we have,

Moles of NaCl = 0.252

Concentration of NaCl = Moles / Volume

= 0.252 / 3.98

= 0.063 M

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