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) + NaN03(aq) What mass of silver chloride can be produced from 1.76L of a 0.280M solution of silver nitrate? Express your answer with the appropriate units. The reaction described in Part A required 3.43L of sodium chloride. What is the concentration of this sodium chloride solution? Express your answer with the appropriate units.

Explanation / Answer

from the reaction we can see , 1 mole of AgNO3 produces 1 mole of AgCl

moles of AgNO3 present = 1.76 *.28 = .4928

moles of AgCl formed = .4928

mass = .4928 *143.32 = 70.628 gm

similarly 1 mole of Nacl gives 1 mole AgCl

so moles of nacl present = .4928

so molarity = .4928/3.43 =.1437 M

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