If 0.4575 g of CaCO3 were dissolved and diluted in a 300.00 mL volumetric flask (assume...
If 0.4575 g of CaCO3 were dissolved and diluted in a 300.00 mL volumetric flask (assume the density of the solution is 1.00 g/mL), what would the calcium (Ca2+) concentration be in a) molarity and b)ppm?
Homework Answers
Mass = volume * density
= 300 *1
= 300 grams
Ppb = (mass of solute / mass of Solution ) *10^6
= (0.4575 / 300 ) *10^6
= 1525
CaCO3 = Ca2+(aq) + CO3 2- (aq)
Moles of CaCO3 = moles of Ca2+
= Mass / molar mass of CaCO3
= 0.4575 / 100
= 4.575*10^-3
Molarity = moles / volume (in litre)
= (4.575*10^-3 / 0.300)
= 0.01525
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