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.
ScanSolve AI Answer
Right Noh, let's go. d) i) Balance the equation and include state symbols. Step 1: Write the unbalanced equation. H_2SO_4 + NaOH → Na_2SO_4 + H_2O Step 2: Balance the sodium (Na) atoms. There are 2 Na atoms on the right, so place a coefficient of 2 in front of NaOH. H_2SO_4 + 2NaOH → Na_2SO_4 + H_2O Step 3: Balance the hydrogen (H) atoms. There are 2 (from H_2SO_4) + 2 (from 2NaOH) = 4 H atoms on the left. There are 2 H atoms in H_2O on the right. Place a coefficient of 2 in front of H_2O. H_2SO_4 + 2NaOH → Na_2SO_4 + 2H_2O Step 4: Check oxygen (O) atoms. There are 4 (from H_2SO_4) + 2 (from 2NaOH) = 6 O atoms on the left. There are 4 (from Na_2SO_4) + 2 (from 2H_2O) = 6 O atoms on the right. The equation is balanced. Step 5: Add state symbols. Sulfuric acid and sodium hydroxide are typically aqueous solutions, sodium sulfate is a soluble salt (aqueous), and water is a liquid. H_2SO_4(aq) + 2NaOH(aq) → Na_2SO_4(aq) + 2H_2O(l) ii) Calculate the mass of sodium sulfate produced. Step 1: Convert the volume of sulfuric acid from cm^3 to dm^3. Volume of H_2SO_4 = 50 cm^3 = (50)/(1000) dm^3 = 0.050 dm^3 Step 2: Calculate the moles of sulfuric acid (H_2SO_4). Moles of H_2SO_4 = Concentration × Volume Moles of H_2SO_4 = 0.2 mol/dm^3 × 0.050 dm^3 = 0.01 mol Step 3: Determine the moles of sodium sulfate (Na_2SO_4) produced using the mole ratio from the balanced equation. From the balanced equation: H_2SO_4 : Na_2SO_4 is 1:1. Moles of Na_2SO_4 = Moles of H_2SO_4 = 0.01 mol Step 4: Calculate the mass of sodium sulfate produced. Mass of Na_2SO_4 = Moles × RFM Mass of Na_2SO_4 = 0.01 mol × 142 g/mol = 1.42 g The mass of sodium sulfate produced is 1.42 g. Got more? Send 'em.