Please help me with these questions  1. How is the molar concentration of OH- measures in a saturated Ca(OH)2 solution for this experiment? 2. How many times should a burette and / or piper be rinsed before it is used to deliver a solution for an analysis 3. Explain how to add less-than-a-drop of titrant from a buret?

1) Why are the titrations in this lab carried out in acidic solution? 2) If a student weighs out 0.565 g of oxalate unknown and it takes 26.8 mL of permanganate solution to titrate it, how much oxalate unknown should the student weigh out in order to use 35.0 mL of permanganate solution?

At each stage of the titration: A. Determine the amount (mol) of weak acid, weak base, and strong acid present. B. Determine the total volume of the combined solutions. C. Determine [H;O*] or [OH], whichever predominates, using the total volume and the nature of the solution: weak base, buffer, weak acid, or strong acid. D. Calculate pH. Determine the pH during the titration of 37.3 mL of 0.336 M methylamine (CH3NH2, K, = 4.2x10-4) by 0.336 M HI at the following points. (Assume the titration is done at 25 °C.) Note that state symbols are not shown for species in this problem. (a) Before the addition of any HI 12.067 (b) After the addition of 16.2 mL of HI 10.74 (c) At the titration midpoint 10.62 (d) At the equivalence point (e) After adding 56.0 mL of HI

Knowing that the unknown acid is monoprotic and the stoic honesty of this reaction is 1:1, we can determine the moles of acid by titration  A. true  B. false