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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To calculate the maximum mass of hydrated sodium sulfate crystals, we need to follow these steps: Step 1: Calculate the moles of sodium hydroxide (NaOH) used. The volume of NaOH is 25.0 cm^3, which needs to be converted to dm^3. Volume = 25.0 cm^3 × 1 dm^31000 cm^3 = 0.0250 dm^3 Now, calculate the moles of NaOH: Moles of NaOH = Concentration × Volume Moles of NaOH = 1.60 mol/dm^3 × 0.0250 dm^3 = 0.0400 mol Step 2: Determine the mole ratio from the balanced chemical equation and calculate the moles of hydrated sodium sulfate (Na_2SO_4 · 10H_2O) formed. The balanced equation is: 2NaOH(aq) + H_2SO_4(aq) + 8H_2O(l) → Na_2SO_4 · 10H_2O(s) From the equation, 2 moles of NaOH produce 1 mole of Na_2SO_4 · 10H_2O. Moles of Na_2SO_4 · 10H_2O = (1)/(2) × Moles of NaOH Moles of Na_2SO_4 · 10H_2O = (1)/(2) × 0.0400 mol = 0.0200 mol Step 3: Calculate the molar mass of hydrated sodium sulfate (Na_2SO_4 · 10H_2O). Using atomic masses: Na = 22.99 g/mol, S = 32.07 g/mol, O = 16.00 g/mol, H = 1.008 g/mol. Molar mass of Na_2SO_4 · 10H_2O = (2 × 22.99) + 32.07 + (4 × 16.00) + 10 × ((2 × 1.008) + 16.00) = 45.98 + 32.07 + 64.00 + 10 × (2.016 + 16.00) = 142.05 + 10 × 18.016 = 142.05 + 180.16 = 322.21 g/mol Step 4: Calculate the maximum mass of hydrated sodium sulfate crystals. Mass = Moles × Molar mass Mass of Na_2SO_4 · 10H_2O = 0.0200 mol × 322.21 g/mol Mass of Na_2SO_4 · 10H_2O = 6.4442 g Rounding to three significant figures (based on the given data 25.0 cm^3 and 1.60 mol/dm^3): Mass of Na_2SO_4 · 10H_2O = 6.44 g Send me the next one 📸