Final answer:
In a high school chemistry assignment involving gravimetric analysis, the percentage yield of a precipitated AgCl from a reaction between BaCl2 and AgNO3 is calculated by comparing actual mass obtained to the theoretical mass.
Step-by-step explanation:
The question involves a gravimetric analysis in chemistry where the mass of a precipitate formed in a chemical reaction is used to calculate the percentage yield or the concentration of a substance in a mixture. The balanced equation for the reaction between barium chloride (BaCl2) and silver nitrate (AgNO3) which results in a precipitate of silver chloride (AgCl) is:
BaCl2 (aq) + 2AgNO3 (aq) → 2AgCl (s) + Ba(NO3)2 (aq)
To calculate the percentage yield, you must first calculate the theoretical yield and then compare it to the actual yield. Using the molarity and volume of BaCl2, the moles of AgCl that should form can be determined. The theoretical yield (mass) of AgCl is then found by using the molar mass of AgCl.
The percentage yield is the actual mass of AgCl obtained divided by the theoretical mass of AgCl, times 100%. Given that the actual yield is 2.01 g, and assuming that the theoretical yield can be calculated to be 2.1255 g (you need to do this step with the provided molarities and volumes), the percentage yield is (2.01 g / 2.1255 g) × 100% = 94.5%.