# What is the mass of the precipitate formed when 50 mL of 16.9% solution of AgNO_(3) is mixed with 50 mL of 5.8% NaCl solution?

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What is the mass of the precipitate formed when 50 mL of 16.9% solution of AgNO_(3) is mixed with 50 mL of 5.8% NaCl solution?
A. 7 g
B. 14 g
C. 28 g
D. 3.5 g

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16.9% solution of AgNO_(3) implies that every 100 mL of solution contain 16.9 gAgNO_(3). Thus, 50 mL of solution will contain 8.45 g AgNO_(3).
Similarly, 5.8% NaCl solution implies that every 100 mL of solution contains 5.8 g NaCl. Thus, 50 mL of solution will contain 2.9 g NaCl.
n_(AgNO_(3))=(mass_(AgNO_(3)))/("molar mass"_(AgNO_(3)))
=(8.45 g)/(170 g mol^(-1))=0.049 mol
n_(NaCl)=(mass_(NaCL))/("molar mass"_(NaCl))
=(2.9 g)/(5.85" g "mol^(-1))=0.049 mol
According to the balanced chemical equation
AgNO_(3)(aq)+NaCl(aq) rarr AgCl(s)+NaNO_(3)(aq)

Mass_(AgCl)" precipitated"=(n//AgCl)("molar mass"_(AgCl))
=(0.049 mol)(143.5 g mol^(-1))
=7.0 g