A solution contains silver ions (Ag+). A student adds excess chloride ions (Cl-) to precipitate silver chloride $(\mathrm{AgCl})$. If the molar mass of silver chloride is $143.32 \mathrm{~g} / \mathrm{mol}$, calculate the mass of silver chloride formed when $100 \mathrm{~mL}$ of the solution is used. A solution contains silver ions ( $\mathrm{Ag}+$ ). A student adds excess chloride ions (Cl-) to precipitate silver chloride $(\mathrm{AgCl})$. If the molar mass of silver chloride is $143.32 \mathrm{~g} / \mathrm{mol}$, calculate the mass of silver chloride formed when $100 \mathrm{~mL}$ of the solution is used.

Question

Accepted Answer

∻Solution∻ ‖ 1 ⋮ **Determine the concentration of Ag+ ions**: To calculate the mass of AgCl precipitate formed, we first need the concentration of Ag+ ions in the solution. However, this information is not provided in the problem statement. Without the concentration of Ag+ ions, we cannot proceed with the calculation. ‖ ∻Answer∻ ⚹ The mass of silver chloride formed cannot be calculated without the concentration of silver ions (Ag+) in the solution. ⚹ ∻Key Concept∻ ⚹ Stoichiometry of a precipitation reaction ⚹ ∻Explanation∻ ⚹ To find the mass of a precipitate formed in a reaction, the stoichiometry of the reaction and the concentration of the reactants are required. In this case, the concentration of Ag+ ions is necessary to calculate the mass of AgCl precipitate. ⚹◊What is the molar mass of silver chloride (AgCl)?⍭ Generate me a similar question◊

Sia