This was a question for a Food Chemistry class, and I am throughly confused. Any help would be greatly appreciated.
If .35g of antacid contains .125g of Ca(OH)2, and you add 25ml of .1M HCl, how much base will you need to reach the end point?
2007-04-01 12:26:08 · 1 answers · asked by megan6288 1 in Science & Mathematics ➔ Chemistry
First you will have to convert the grams of Ca(OH)2 to moles. You need to divide the mass by the molecular mass.
The tricky part is that 1 mole of Ca(OH)2 will give 2 moles of (OH)- when ionized. So you need half as many moles of Ca(OH)2 as you would need of HCl for the titration.
Calculate how many moles of HCl you have. 1 molar is 1 mole dissolved in 1 liter. You have .025 liters of 0.1 molar.
Divide the moles of H+ by 2 nad you have the moles of Ca(OH)2 that you need.
2007-04-01 12:32:47 · answer #1 · answered by reb1240 7 · 0⤊ 0⤋