Analysis of ClA 0.4892 g sample of the chromium compound was dissolved in water and excess silver nitrate was added to precipitate AgCl. 1.0042 g of AgCl was obtained. Calculate the mass of Cland then % Cl- . Show work below. Answers: g Cl- % ClAnalysis of NH3 A 0.2502 g sample of the unknown chromium compound was dissolved in water, and 42.56 mL of 0.1089 M HCl was added, converting all the NH3 to NH4 with HCl left over. The excess HCl was titrated with 0.1022 M NaOH, requiring 10.28 mL Moles HCl added moles Moles NaOH added moles Moles HCl USED moles Moles NH3 moles Grams NH3 grams % NH3 % Determination of Empirical Formula Knowing % Cr3 , % NH3, and % Cl- , find the empirical formula. Show work below. Write the balanced equation for the preparation of the compound. Determine which of the original reagents was limiting and calculate the % yield. Show work below