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Problem: Suppose 2.57g of nickel(II) chloride is dissolved in 350.mL of a 38.0mM aqueous solution of potassium carbonate.Calculate the final molarity of nickel(II) cation in the solution. You can assume the volume of the solution doesn't change when the nickel(II) chloride is dissolved in it.Be sure your answer has the correct number of significant digits.

FREE Expert Solution

We’re being asked to calculate the molarity (M) of nickel(II) cation in 2.57g of nickel(II) chloride is dissolved in 350.mL . Recall that:


Molarity (M)=moles of soluteLiters of solution


• Dissociation of NiCl2: NiCl2(s)  Ni2+(aq) + 2 Cl(aq)


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Problem Details

Suppose 2.57g of nickel(II) chloride is dissolved in 350.mL of a 38.0mM aqueous solution of potassium carbonate.

Calculate the final molarity of nickel(II) cation in the solution. You can assume the volume of the solution doesn't change when the nickel(II) chloride is dissolved in it.

Be sure your answer has the correct number of significant digits.



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