A chemist has 4.0 g of silver nitrate and needs to prepare 2.0 L of a 0.010 M solution. How many grams of solid silver nitrate will be left over after the solution is made?
molarity of a solution is defined as the number of moles of solute dissolved in 1 L solvent. The molarity required in the solution to be prepared - 0.010 M the volume of the solution to be prepared - 2.0 L In 1 L of solution there should be 0.010 mol Therefore in 2.0 L solution, number of moles required - 0.010 mol/L x 2.0 L the number of silver nitrate moles required - 0.020 mol Molar mass of silver nitrate - AgNO₃ - 169.9 g/mol Mass of silver nitrate needed to make solution - 0.020 mol x 169.9 g/mol Mass required - 3.4 g chemist had 4.0 g and 3.4 g needed to make the solution leftover solid AgNO₃ after the reaction is 4.0 - 3.4 = 0.6 g of AgNO₃
