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5 litre of a solution contains 25 mg of ...

5 litre of a solution contains 25 mg of `CaCO_(3)`. What is its concentration in ppm? (mol.wt of `CaCO_(3)` is 100)

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5 litres of a solution contains 25mg of CaCO_(3) . What is its concentration in ppm ?

Calculate molarity of CaCO_(3) (aq.) solution which has concentration of CaCO_(3)=200 ppm.

Knowledge Check

  • 10 g of CaCO_(3) contains :

    A
    10 moles of `CaCO_(3)`
    B
    0.1 g atom of Ca
    C
    `6 xx 10^(23)` atoms of Ca
    D
    0.1 equivalent of Ca

  • 10 g of CaCO_(3) contains

    A
    10 moles of `CaCO_(3)`
    B
    `0.1 g` atom of `Ca`
    C
    `6 xx 10^(23)` atoms of `Ca`
    D
    0.1 of equivalent of `Ca`

  • 250 ml of a calcium carbonate solution contains 2.5 grams of CaCO_(3) . If 10 ml of this solution is diluted to one litre, what is the concentration of the resultant solution ?

    A
    0.1 M
    B
    0.001 M
    C
    0.01 M
    D
    `10^(-4)M`

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    For the reaction CaCO_(3) (s) hArr CaO (s) + CO_(2) (g), K_(p) = 1*16 " atm . If "20* 0" g of " CaCO_(3) " is heated to " 800^(@)C" in a 10 litre container, what % of "CaCO_(3) " would remain unreached at equilibrium ? ( Mol. wt. of " CaCO_(3) = 100, R = 0*0821 " L atm mol"^(-1) K^(-1) )

    A solution with mass of 1.00 kg contains 3 mg of solute. Express this concentration in ppm and ppb.

    One kilogram sample of hard water contains 4.44 mg of CaCl_(2) and 1.9 mg of NaCl. The total hardness in tems of ppm of CaCO_(3) is :

    The solubility of CaCO_(3) is 7 mg/litre . CaCO_(3) is 7 mg/litre . Calculate the solubility product of BaCO_(3) from this information and from the fact that when Na_(2)CO_(3) is added slowly to a solution containing equimator concentration of Ca^(+2) and Ba^(+2) , no precipitate of CaCO_(3) is formed until 90 \% of Ba^(+2) has been precipitated as BaCO_(3)

    One litre of a sample of hard water contains 5.55 mg of CaCl_(1) and 4.75 mg of MgCl_(2) . The total harness of ppm of CaCO_(3) is

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