1) In the year 1618, England was experiencing a drought. Despite the shortage of water, cattle refused to drink from a certain pond in Epson Common. A man named Henry Wicker took some interest in this, and went over and drank a bit of the water himself. It tasted terribly bitter. He took some home and after boiling off the water he was left with Magnesium Sulfate crystals. This salt became known as "Epsom Salts" and soon after they were being used to treat constipation all over Europe. The three naturally occurring isotopes of magnesium are: magnesium-24(23.985 amu), magnesium-25(24.986 amu) and magnesium-26(26.983 amu). Their percent abundances in nature are 78.99%, 10.00% and 11.01% respectively. What is the average atomic mass of magnesium?

Suppose you added 40 mL of water to your vinegar sample instead of 20 mL. Would the titration have required more, less or the same amount of NaOH(aq) for a complete reaction? Explain.

A 25.00 mL sample of 0.125 M sulfuric acid solution is titrated with 0.500 M sodium hydroxide solution. Write the balanced chemical equation for the neutralization reaction.

H2. Titrations are performed by a scientist in the laboratory as follows: a solution of deuterated hydrochloric acid contains 1.08 g DCl in 750 ml of deionised, distilled water. An average amount of 14.95 ml of the DCl(aq) solution is titrated with 25.0 ml of Ca(OH)2 to produce an endpoint (as determined by an appropriate indicator). What is the molarity of the Ca(OH)2 solution? You must include all of your calculations    Please give typed answer