Answer part C only. Thank you. Review I Constants I Periodic TablePart ABarium can be analyzed by precipitating it as BaSO4 and weighing the precipitate. When a 0.265 g sample of a bariumcompound was treated with excess H2SO4 8.60x10-2 g of BaSO4 formed. What is the percentage of barium in the compound?19.1SubmitPrevious Answersv CorrectPart B-What is the percentage of sodium in pure table salt?Report your answer as a pecenteage to three significant figures.39.3SubmitPrevious AnswersV CorrectPart CAn impure sample of table salt that weighed 0.8571 g when dissolved in water and treated with excess AgNO3 formed 2.031 gof AgCl. What percentage of NaCl is in the impure sample?Show All4-tvAONMacBook ProG Search or type URL

Given: Mass of table salt sample = 0.8571 g. And mass of AgCl precipitates formed = 2.031 g. Molar mass of AgCl = Atomic mass of Ag + Atomic mass of Cl = 108 + 35.5 = 143.5 g/mol. Hence moles of AgCl produced = MassMolar mass = 2.031143.5 = 0.0141533 mol approx. Since all the Cl present in the table salt sample i.e. NaCl sample will convert into the AgCl on treating with the AgNO3. And moles of Cl present in NaCl = moles of NaCl present. And moles of Cl present in AgCl = moles of AgCl. Therefore the moles of NaCl = moles of AgCl produced = 0.0141533 mol. Molar mass of NaCl = Atomic mass of Na + Atomic mass of Cl = 23 + 35.5 = 58.5 g/mol. Hence mass of NaCl = moles × molar mass = 0.0141533 × 58.5 = 0.82797 g approx.Therefore the percentage of NaCl in the sample = Mass of NaClMass of sample × 100 = 0.827970.8571 × 100 = 96.6% approx. Therefore the answer is 96.6 % NaCl approx.