AgNO3 solutions are often used to plate silver onto other metals. What is the maximum amount of silver in grams that can be plated out of 4.8 L of an AgNO3 solution containing 3.4% Ag by mass? (Assume that the density of the solution is 1.01 g/mL.)

Solution: Here, we are going to calculate the mass of silver that can be plated out of 4.8 L of an AgNO3 solution containing 3.4 % Ag by mass.

Step1:

The mass percentage of a component of a solution is defined as:

Mass of the component in the solution

Mass % of a component = ----------------------------------------------------- × 100 ---(1)

Total mass of the solution

Step2:

Again, density may be defined as mass per unit volume.

Thus,

d = m / v

Here, density of the solution = 1.01 g/mL

Volume of the solution = 4.8 L = 4.8 x 1000 mL = 4800 mL [1 L = 1000 mL]

Therefore, mass of the solution = density x volume

= (1.01 g/mL) x 4800 mL

= 4848 g

Step3:

Mass % of Ag in the solution = 3.4 %

Mass of the solution = 4848 g

Substituting the values in equation (1), we get,

3.4 = (mass of Ag in solution / 4848 g) x 100

3.4 / 100 = mass of Ag in solution / 4848 g

0.034 x 4848 g = mass of Ag in solution.

164.83 g = mass of Ag in solution.

Thus, 164.83 g of silver can be plated out of 4.8 L of an AgNO3 solution containing 3.4 % Ag by mass.

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