What is the mass of the precipitate formed when 50ml of 16.9% solution of AgNO3 is mixed with 50ml of 5.8% nacl solution? Explain plz....

We assume that you mean percentage by VOLUME....

Explanation:

And so we got ………..

#50*mLxx16.9%*g*mL^-1=8.45*g*AgNO_3#..

And #50*mLxx5.8%*g*mL^-1=2.90*g*NaCl#..

#n_"silver nitrate"=(8.45*g)/(169.87*g*mol^-1)-=0.050*mol#

#n_"sodium chloride"=(2.90*g)/(58.44*g*mol^-1)-=0.050*mol#

And the molar equivalence makes me suspect that we have got the terms of the question right....

And silver ion reacts with chloride ion as follows...

#Ag^+ + Cl^(-) rarr AgCl(s)darr#

And silver chloride is as soluble as a brick, and crashed out of solution as a curdy white precipitate... And thus we should get a mass with respect to the silver salt of...…

#0.050*molxx143.32*g*mol^-1=7.11*g#

You happy with this spray? We used the relationship

...

#"Concentration"="moles of solute"/"volume of solution"#...by taking the product...#"volume"xx"concentration"# we are able to get #"moles of solute"# ……...