Silver ions can be precipitated from aqueous solutions by the addition of aqueous chloride: (aq) + (aq) → AgCl(s) Silver chloride is virtually insoluble in water so that the reaction appears to go to completion. How many grams of solid NaCl must be added to 25.0 mL of 0.376 mol L^-1 solution to completely precipitate the silver?

Question

Quizplus · Accepted Answer

1. Write the balanced chemical equation:

AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq)

2. Calculate the amount of AgNO3 present in the given solution:

n = C x V = 0.376 mol/L x 0.0250 L = 0.0094 mol

3. Use the stoichiometry of the balanced equation to find the amount of NaCl needed to react with all the AgNO3:

From the equation, it can be seen that 1 mole of AgNO3 reacts with 1 mole of NaCl to form 1 mole of AgCl. Therefore, the amount of NaCl needed is also 0.0094 mol.

4. Calculate the mass of NaCl needed:

m = n x M = 0.0094 mol x 58.44 g/mol = 0.549 g

So the answer is B) 0.549 g.

Silver Ions Can Be Precipitated from Aqueous Solutions by the Addition