This physics problem tests your understanding of fundamental physical laws and their applications. The step-by-step solution below breaks down the problem using relevant equations and physical reasoning.
ScanSolve AI Answer
To calculate the molar mass of XOH, we need information about the concentrations and volumes involved in the titration. Since these are not provided in the current image, we will make reasonable assumptions based on typical titration problems. Assumptions: Concentration of H_2SO_4 (solution A) = 0.100 mol/dm^3. Volume of XOH (solution B) used in each titration = 25.00 cm^3. The average volume of H_2SO_4 (solution A) used from the previous step is 24.35 cm^3. Solution B was prepared by dissolving 2.72 g of XOH in 250 cm^3 of water. Step 1: Write the balanced chemical equation and determine the mole ratio. The reaction between sulfuric acid (H_2SO_4) and a metal hydroxide (XOH) is: H_2SO_4(aq) + 2XOH(aq) → X_2SO_4(aq) + 2H_2O(l) The mole ratio of H_2SO_4 : XOH is 1:2. Step 2: Calculate the moles of H_2SO_4 used. The concentration of H_2SO_4 (solution A) is 0.100 mol/dm^3. The average volume of H_2SO_4 used is 24.35 cm^3, which is 0.02435 dm^3. Moles of H_2SO_4 = Concentration × Volume Moles of H_2SO_4 = 0.100 mol/dm^3 × 0.0243