A 1.345 gram sample of a compound containing barium and oxygen was dissolved in hydrochloric acid to give a solution of barium ions (Ba+2), which was then completely precipitated out with excess potassium chromate to give 2.012 grams of barium chromate, BaCrO4.   (a) How many moles of barium ions(Ba+2) were in the original sample? (b) How many grams of barium ions (Ba+2) were in the original sample? (c) How many grams of oxygen ions(O-2) were in the original sample? (d) What is the percentage by mass of O ions (O-2) in the original(1.345g) sample?

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A: Given data concentration of Ca3(PO4)2=0.829M Moles of Ca+2= 0.0186 Volume of Ca3(PO4)2=?

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Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.