Final answer:
The maximum mass of AgCl precipitated is calculated by identifying the limiting reactant based on the molarity and volume of the reactants, using stoichiometry from the reaction AgNO3(aq) + Cl−(aq) → AgCl(s) + NaNO3(aq), and then multiplying the moles of the limiting reactant by the molar mass of AgCl.
Step-by-step explanation:
The question asks for the maximum mass of AgCl that can precipitate from a reaction between a 0.00350 M solution of Cl− ions and a 0.500 M solution of AgNO3. This type of reaction is a classic example of a precipitation reaction, where an insoluble compound forms from the mixture of two soluble salts. In this scenario, we would use the stoichiometry of the reaction, which is a 1:1 ratio of Ag+ to Cl−, to determine the limiting reactant and then calculate the mass of AgCl that could form.
To find the limiting reactant, you would compare the mole ratios based on the volumes and concentrations given. This will determine how much AgCl can be formed. Once the amount in moles of AgCl is determined, multiplying by the molar mass of AgCl (approximately 143.32 g/mol) will give the maximum possible mass of AgCl that can be precipitated from the reaction.