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March 27, 2017

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A 3.50 g sample of KCl is dissolved in 10.0 mL of water. The resulting solution is then added to 60.0 mL of a 0.500 M CaCl2(aq) solution. Assuming that the volumes are additive, calculate the concentrations of each ion present in the final solution.


*confused*

  • AP Chem - ,

    Change grams to mols for KCl.
    Change 60.0 mL of 0.500 M solution CaCl2 to mols.
    Write the ionization equation to show how the molecules break apart.
    Note the mol ratios.
    Calculate molarity which = #mols/L soln for each ion.
    I don't think I've omitted a step but post your work if you get stuck.

  • AP Chem - ,

    There is not much to it.
    how many moles of KCl? That give you the mole Cl, moles of K from that.

    How many moles of CaCl2? That gives you themoles of Ca, and 2Cl ions.

    Now add the Cl ions from the calcium chloride, and the KCl.
    Concentration Cl=moles Cl/total volume and so on.

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