Question

An aqueous solution is 40.0% by mass silver nitrate, AgNO3, and has a density of 1.47 g/mL.

The molarity of silver nitrate in the solution is
M.

Answer 1

Molarity = 3.46 M

Step-by-step explanation:

Given data:

Percentage of silver nitrate = 40.0%

Density of AgNO₃ = 1.47 g/mL

Molarity of solution = ?

Solution:

40% means out of 100g we have 40 g of AgNO₃ and 60g solvent.

Number of moles of silver nitrate = mass /molar mass

Number of moles = 40 g/ 170 g/mol

Number of moles = 0.235 mol

Volume of solution:

Total mass of solution = 100 g

density = 1.47 g/mL which means there are 1.47 gram into 1 mL.

100 g/1 × 1mL/ 1.47 g × 1 L / 1000 mL

0.068 L

Molarity:

Molarity = number of moles / volume in L

Molarity = 0.235 mol / 0.068 L

Molarity = 3.46 M