the recomended daily allowance of calcium is 1000 mg of Ca*2+ ions. calcium carbonate is used to supply the calcium in vitamin tablets. HOw many moles of calcium ions does 1000 mg represent? how many moles of calcium carbonate are needed to supply the required amount of calcium ions? what mass of calcium carbonate must each tablet contain?
2006-10-23 10:45:34 · 2 answers · asked by babycakez 3 in Science & Mathematics ➔ Chemistry
Well, 1000mg (Ca)2+ = 1g. 1 mole of Ca = 40g, so that 1000mg represents 0.025 moles (Ca)2+. Calcium Carbonate is just CaCO3, with a molar mass of 100g (Ca = 40g, C = 12g, 3O = 48g). Each molecule contains one atom of Ca... therefore 1 (Ca)2+ ion. You know you need 0.025 moles of (Ca)2+, so multiply that by the molar mass of CaCO3: 100g/mol * 0.025mol = 2.5g CaCO3 (or 2500mg CaCO3). Hope this helps!
2006-10-23 10:48:17 · answer #1 · answered by Anonymous · 0⤊ 0⤋
ok, first you need to find out the molar mass of calcium, which is about 40g, i believe
so, number of mole = (amt of ca u have)/(ca molar mass) = (1.0g)/(40g)
To calculate how much calcium carbonate u need, you need to find out what is the molar mass of calcium carbonate, which is about 84g. so, number mol (the answer for the first part)= (amt. ca. carbonate needed)/(80g)
2006-10-23 10:52:03 · answer #2 · answered by Travis 4 · 0⤊ 0⤋