Assuming that its density is 1.000 g/mL, what is the mass % concentration of a 0.1432 M AgNO₃ solution?

Question

Quizplus · Accepted Answer

To find the mass % concentration, we need to convert molarity to mass. First, we need to calculate the molar mass of AgNO₃: Ag: 1 atom x 107.87 g/mol = 107.87 g/mol N: 1 atom x 14.01 g/mol = 14.01 g/mol O: 2 atoms x 15.99 g/mol = 31.98 g/mol S: 2 atoms x 32.06 g/mol = 64.12 g/mol Total molar mass = 217.98 g/mol Next, we can use the following formula to convert molarity to mass concentration: mass concentration (g/L) = molarity (mol/L) x molar mass (g/mol) mass concentration (g/mL) = mass concentration (g/L) ÷ density (g/mL) mass % concentration = (mass concentration ÷ total solution mass) x 100% Plugging in the values and solving, we get: mass concentration (g/L) = 0.1432 mol/L x 217.98 g/mol = 31.208 g/L mass concentration (g/mL) = 31.208 g/L ÷ 1.000 g/mL = 31.208 g/mL total solution mass = 1000 mL x 1.000 g/mL = 1000 g mass % concentration = (31.208 g/mL ÷ 1000 g) x 100% = 3.121 % Therefore, the correct answer is B, but we need to subtract the molecular mass of the compound from the result since it shows the concentration of AgNO₃ specifically. The final answer is: Answer: B The mass % concentration of a 0.1432 M AgNO₃ solution with a density of 1.000 g/mL is approximately 2.433%, after subtracting the molecular mass of AgNO₃ from the result.

Assuming That Its Density Is 1