What is the mass of precipitate formed when 50ml of 16.9% solution of AgNO3 mixed with 50ml of 5.8% NaCl solution?

Question

(Ag=107.8u, N=14u, O=16u, Na=23u, Cl=35.5u)

Answer 1

Moles of AgNo3= 50x 16.9/100x169.8
                           = 0.05mole
Moles of NaCl = 50x5.8/100x58.5
                       =0.05mole
AgNo3 + NaCl ----> AgCl + NaNo3
mass of AgCl = mole x molar mass
                       =0.05 x 143.5
                       = 7.16 g

Comments

How did you decide that the precipitate is AgCl?

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AgCl precipitated out of solution because it's insoluble in water.

In this double-displacement reaction, all the states of the reactants are aqueous, meaning, they are dissolved in water. The insoluble precipitate, AgCl, is solid. NaNO3 is aqueous because it's soluble in water.

So, we write the complete ionic equation with the state symbols as:

AgNO3(aq) + NaCl(aq) ---> AgCl(s) + NaNO3(aq)

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Thank you, sir,
it was really helpful...