1. For titration of 20.00 ml of the analyzed solution containing iron(III)salt, 18.50 ml of EDTA solution with a molar concentration of 0.02500mol/L and a correction factor of 0.9800 were spent . Calculate the weight of iron (in grams).

Question

1. For titration of 20.00 ml of the analyzed solution containing iron(III)salt, 18.50 ml of EDTA solution with a molar concentration of 0.02500mol/L and a correction factor of 0.9800 were spent . Calculate the weight of iron (in grams).

Answer 1

To calculate the weight of iron in the analyzed solution, we need to follow these steps:1. Calculate the moles of EDTA used in the titration.2. Use the stoichiometry of the reaction between iron(III) salt and EDTA to find the moles of iron.3. Convert the moles of iron to grams.Given information:- Volume of the analyzed solution: 20.00 mL- Volume of EDTA solution used: 18.50 mL- Molar concentration of EDTA solution: 0.02500 mol/L- Correction factor for EDTA: 0.9800Step 1: Calculate the moles of EDTA used in the titration.Moles of EDTA = Volume of EDTA solution × Molar concentration of EDTAMoles of EDTA = 18.50 mL × 0.02500 mol/L × 0.001 L/mLMoles of EDTA = 0.0004625 molStep 2: Use the stoichiometry of the reaction between iron(III) salt and EDTA to find the moles of iron.The reaction between iron(III) salt and EDTA is a 1:1 molar ratio.Moles of iron = Moles of EDTAMoles of iron = 0.0004625 molStep 3: Convert the moles of iron to grams.Weight of iron = Moles of iron × Molar mass of ironWeight of iron = 0.0004625 mol × 55.845 g/molWeight of iron = 0.0258 gTherefore, the weight of iron in the analyzed solution is 0.0258 grams.

Вопрос

1. For titration of 20.00 ml of the analyzed solution containing iron(III)salt, 18.50 ml of EDTA solution with a molar concentration of 0.02500mol/L and a correction factor of 0.9800 were spent . Calculate the weight of iron (in grams).

Решения

Ответ