chloride did the sample contain? 4. FeCl_(3) weighs 5.95 g.The chloride converted to the hydrous oxide and ignited to Fe_(2)O_(3) The oxide weighs 2.62 g Calculate the percent Fe in the original mixture. Calculate the pH and pOH of the following strong base solutions: 0.14 M Ba(OH)_(2)

To calculate the percent Fe in the original mixture, we need to determine the amount of Fe in the final oxide ( ) and then calculate the percentage based on the initial weight of the chloride ( ).1. Calculate the molar mass of : - Molar mass of Fe = 55.85 g/mol - Molar mass of O = 16.00 g/mol - Molar mass of = (2 × 55.85) + (3 × 16.00) = 159.69 g/mol2. Calculate the moles of : - Moles of = Mass / Molar mass = 2.62 g / 159.69 g/mol = 0.0164 mol3. Calculate the moles of Fe in : - Moles of Fe = 2 × Moles of = 2 × 0.0164 mol = 0.0328 mol4. Calculate the mass of Fe in the original mixture: - Mass of Fe = Moles of Fe × Molar mass of Fe = 0.0328 mol × 55.85 g/mol = 1.83 g5. Calculate the percent Fe in the original mixture: - Percent Fe = (Mass of Fe / Initial weight of ) × 100% = (1.83 g / 5.95 g) × 100% = 30.6%Therefore, the percent Fe in the original mixture is 30.6%.To calculate the pH and pOH of the 0.14 M solution, we need to use the following formulas:pH = -log[H+]pOH = -log[OH-]1. Calculate the concentration of OH- ions in the solution: - dissociates into 2 OH- ions per molecule. - [OH-] = 2 × 0.14 M = 0.28 M2. Calculate the pOH of the solution: - pOH = -log[OH-] = -log(0.28) = 0.553. Calculate the pH of the solution: - pH = 14 - pOH = 14 - 0.55 = 13.45Therefore, the pH of the 0.14 M solution is 13.45, and the pOH is 0.55.