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) rightarrow AgCl(s) + NaNO3(aq) What mass of silver chloride can be produced from 2.00L of a 0.119 M solution of silver nitrate? Express your answer with the appropriate units. The reaction described in Part A required 3.39L of sodium chloride. What is the concentration of this sodium chloride solution? Express your answer with the appropriate units.

Explanation / Answer

(a) Molality = number of moles of AgNO3/ Weight of Solution ===> number of moles of AgNO3 = Weight of water X Molality = 2 * 0.119 = 0.238 moles ===> number of moles of AgCl = 0.238 ; We know that the Molar mass of AgCl = 143.32 g / mol ===> Weight of AgCl = number of moles of AgCl X Molar mass of AgCl = 143.32 * 0.238 = 34.11 g (b) Given Volume of solution = 3.39 L ===> Concentration of the AgCl Solution = number of moles of AgCl / Volume of solution = 0.238 / 3.39 = 0.07 mol/L ===> Concentration of the AgCl Solution = 0.07 mol/L

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