1. The problem statement, all variables and given/known data "A 4.36-g sample of an unknown alkali metal hydroxide is dissolved in 100.0 mL of water. An acid-base indicator is added and the resulting solution is titrated with 2.50 M HCl (aq) solution. The indicator changes colour signaling that the equivalence point has been reached after 17.0 mL of the hydrochloric acid solution has been added." a) What is the molar mass of the metal hydroxide? b) What is the identity of the alkali metal cation: Li+, Na+, K+, Rb+, or Cs+? 2. Relevant equations Molarity = moles solute / volume of solution in liters 3. The attempt at a solution First, I found the moles for HCl: moles solute / volume of solution in liters = molarity moles solute = molarity (volume of solution in liters) 0.0425 mol HCl = 2.5(0.017) Now I guessed that 0.0425 mol of HCl is supposed to react with 0.425 (?)OH to produce H2O and (?)Cl. Then I tried to find the moles of all the possible alkali metal hydroxides by adding the molar mass of hydrogen and oxygen, then adding them to the different alkali metals. Then I took my given mass of 4.36 g and divided it by each of those molar masses. If the result was not 0.0425, then I eliminated it as a solution. This is my final result: 4.36/102.47514 = 0.0425 mol RbOH, where 102.47514 = 1.00794 + 15.9994 + 85.4678. I then concluded that the alkali metal was rubidium, seeing how the numbers matched up. However, I am completely sure this is not the correct way to do this problem. Could someone tell me how they would do this titration problem?