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
To solve this problem, crucial information regarding the concentration of solution W and the volume of solution W used in the titration is missing from the image. I will proceed by making reasonable assumptions for these values to demonstrate the calculation method. Assumptions: Concentration of solution W (C_W) = 0.100 mol/dm^3 Average volume of solution W used (V_W) = 20.00 cm^3 The reaction between W and the metal hydroxide (MOH) is a 1:1 mole ratio (e.g., if W is a monoprotic acid). --- a) Number of moles of solution W that reacted with each 25 cm^3 portion of solution L. Step 1: Calculate the moles of solution W. Moles of W = Concentration of W × Volume of W (in dm^3) Moles of W = 0.100 mol/dm^3 × 20.00 cm^31000 cm^3/dm^3 Moles of W = 0.100 × 0.02000 mol Moles of W = 0.00200 mol --- b) Calculate the: i) Number of moles of the metal hydroxide (MOH) in solution L that reacted with each portion of solution W. Step 2: Determine the moles of MOH. Based on the assumed 1:1 mole ratio between W and MOH, the moles of MOH that reacted are equal to the moles of W. Moles of MOH = Moles of W Moles of MOH = 0.00200 mol ii) Concentration of solution L. Step 3: Calculate the concentration of solution L. The volume of solution L used was 25 cm^3. Concentration of L = Moles of MOHVolume of L (in dm^3) Concentration of L = 0.00200 mol25.00 cm^31000 cm^3/dm^