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Screenshot_2019-01-23_at_4.56.18_PM.png What is the mass of the precipitate formed when 50 mL of 16.9% solution of AgNO3 is mixed with 50 mL of 5.8% NaCl solution ?(Ag = 107.8, N = 14, O = 16, Na = 23, CI = 35.5)

Answers (1)

Mass percent of the solution -

Mass percent = ((mass of solute)/(mass of solution) ) X 100

 it is a mass of solute present in 100-gram solution.

16.9% solution of AgNO3 means 16.9g AgNO3 in 100ml solution.

\Rightarrow    50ml of solution contains \frac{16.9}{2}\:=\:8.45g

Similarly, 100ml of other solution contains 5.8g NaCl

50ml of other solution contains 2.9g NaCl

Mol of AgNO3 = \frac{8.45}{169.8}\:=\:0.049

Mol of NaCl = \frac{2.9}{58.5}\:=\:0.049

AgNO3    +      NaCl     \rightarrow      AgCl     +     NaNO3

0.049                   0.049                        0                          0                       

0                       0                      0.049                 0.049     

Mass of AgCl = 0.049 \times Molar mass of AgCl

                     = 0.049 \times 143.5 = 7g

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