This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
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You're on a roll — i) What mass of zinc Sulphate crystals would need to be taken to obtain this intake? Step 1: Convert the daily zinc intake from milligrams to grams. Daily zinc intake = 15 mg = 15 × 10^-3 g Step 2: Calculate the moles of zinc (Zn) required. The atomic mass of zinc (Zn) is 65 g/mol. Moles of Zn = Mass of ZnMolar mass of Zn Moles of Zn = 15 × 10^-3 g65 g/mol ≈ 0.00023077 mol Step 3: Determine the moles of hydrated zinc sulfate (ZnSO_4 · 7H_2O) needed. From the formula ZnSO_4 · 7H_2O, 1 mole of the hydrated salt contains 1 mole of zinc. Moles of ZnSO_4 · 7H_2O = Moles of Zn ≈ 0.00023077 mol Step 4: Calculate the molar mass of hydrated zinc sulfate (ZnSO_4 · 7H_2O). Atomic masses: Zn = 65, S = 32, O = 16, H = 1. Molar mass of ZnSO_4 = 65 + 32 + (4 × 16) = 161 g/mol Molar mass of 7H_2O = 7 × ((2 × 1) + 16) = 7 × 18 = 126 g/mol Molar mass of ZnSO_4 · 7H_2O = 161 + 126 = 287 g/mol Step 5: Calculate the mass of hydrated zinc sulfate crystals needed. Mass = Moles × Molar mass Mass = 0.00023077 mol × 287 g/mol ≈ 0.06630 g Converting to milligrams: Mass = 0.06630 g × 1000 mg/g = 66.3 mg The mass of zinc sulfate crystals needed is 66.3 mg. ii) Calculate the concentration of this solution in mol/dm^3 of the hydrated salt. Step 1: Identify the moles of hydrated zinc sulfate. From part (i), the moles of ZnSO_4 · 7H_2O are approximately 0.00023077 mol. Step 2: Convert the volume of the dose from millilitres to litres (dm^3). Volume = 5 ml = 5 cm^3 = 0.005 L = 0.005 dm^3 Step 3: Calculate the concentration of the solution. Concentration = Moles of hydrated saltVolume of solution (in dm^3) Concentration = 0.00023077 mol0.005 dm^3 ≈ 0.046154 mol/dm^3 Rounding to three significant figures: The concentration of the solution is 0.0462 mol/dm^3. What's next? Send 'em! 📸