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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Step 1: Write the balanced chemical equation for the neutralization reaction. Sulfuric acid (H_2SO_4) reacts with sodium hydroxide (NaOH) to produce sodium sulfate (Na_2SO_4) and water (H_2O). H_2SO_4(aq) + 2NaOH(aq) Na_2SO_4(aq) + 2H_2O(l) From the balanced equation, 1 mole of H_2SO_4 reacts with 2 moles of NaOH. Step 2: Calculate the moles of sulfuric acid. Given: Volume of H_2SO_4 solution = 25 cm^3 = 0.025 L Concentration of H_2SO_4 solution = 0.05 M Moles of H_2SO_4 = Molarity × Volume (L) Moles of H_2SO_4 = 0.05 mol/L × 0.025 L Moles of H_2SO_4 = 0.00125 mol Step 3: Calculate the moles of sodium hydroxide required for neutralization. Using the mole ratio from the balanced equation (1 mole H_2SO_4 : 2 moles NaOH): Moles of NaOH = Moles of H_2SO_4 × 2 mol NaOH1 mol H_2SO_4 Moles of NaOH = 0.00125 mol × 2 Moles of NaOH = 0.0025 mol Step 4: Calculate the volume of sodium hydroxide solution required. Given: Concentration of NaOH solution = 0.1 M Volume of NaOH (L) = Moles of NaOHMolarity of NaOH Volume of NaOH (L) = 0.0025 mol0.1 mol/L Volume of NaOH (L) = 0.025 L Step 5: Convert the volume to cm^3 (optional, but consistent with given units). Volume of NaOH (cm^3) = 0.025 L × 1000 cm^31 L Volume of NaOH (cm^3) = 25 cm^3 The volume of 0.1 M sodium hydroxide solution required is 0.025 L or 25 cm^3.