Suppose of nickel (II) iodide is dissolved in of a aqueous solution of potassium

Question

Suppose of nickel (II) iodide is dissolved in of a 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) iodide is dissolved in it.Be sure your answer has the correct number of significant digits Suppose 0.176 g of nickel (II) iodide is dissolved in 250 mL of a 17.0 mM 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) iodide is dissolved in it.Be sure your answer has the correct number of significant digits

Explanation / Answer

no of moles of Ni I2 =0.176/312.5

=0.00056

gram eq=0.00056/2=0.00028

no of moles of KI

=250*17*10^-3-3

=4.250*10^-3

gram eq=4.25*10^-3

so all ni will be reacted and no Ni cation will be left as NiCO3 won't dissolve in water to give Ni Cation

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