Analytical chemistry

Calculate to four decimal places the mass of pure dry CaCO3 required to make 1 L of a 1000
ppm Ca stock solution.

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  1. 1000 ppm, means 1000g
    1000 ppm means .001g of Ca+2 ion, or .001/ 40.078 moles Ca, so you want then the same number of moles of C and O3

    element, moles, mass
    Ca, .001/40.078, .001g
    C, ibid times 12.0107, 0.000299683118
    3O, ibid times 3*15.9994, 0.00119761964

    Now adding up the masses,
    0.00119761964+.001+.000299683118
    I get 0.00249730276 grams of CaCO3. Now, is the mass of a liter of solution to four decimal places really 1000g? No, depends on temperature, it varies some. So you have to have temperature given. http://water.usgs.gov/edu/density.html

    check my work

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