You have a solution of silver nitrate with an unknown concentration. To determine the concentration, you devise a method of adding an excess of calcium metal to 100.0 cm3 of solution and collecting the silver by filtration.2AgNO3(aq)+Ca(s)→Ca(NO3)2(aq)+2Ag(s)2AgNO3(aq)+Ca(s)→Ca(NO3)2(aq)+2Ag(s)If 0.201 g of silver was collected, calculate the concentration of the silver nitrate solution in mol dm−3.Answer with the numerical value of the concentration to three significant figures, but do not include the units.

To calculate the concentration of the silver nitrate solution, we first need to determine the number of moles of silver (Ag) that were collected.

1. Calculate the molar mass of silver (Ag). From the periodic table, the molar mass of Ag is approximately 107.87 g/mol.

2. Calculate the number of moles of silver (Ag) collected. The number of moles is calculated by dividing the mass of the substance by its molar mass. So, the number of moles of Ag collected is 0.201 g / 107.87 g/mol = 0.00186 mol.

3. According to the balanced chemical equation, 2 moles of AgNO3 produce 2 moles of Ag. Therefore, the number of moles of AgNO3 in the 100.0 cm3 solution is also 0.00186 mol.

4. Convert the volume of the solution from cm3 to dm3. 1 dm3 = 1000 cm3, so 100.0 cm3 = 0.100 dm3.

5. Calculate the concentration of the AgNO3 solution. Concentration is calculated by dividing the number of moles of solute by the volume of the solution in dm3. So, the concentration of the AgNO3 solution is 0.00186 mol / 0.100 dm3 = 0.0186 mol/dm3.

To three significant figures, the concentration of the silver nitrate solution is 0.0186 mol/dm3.