Question

Suppose 0.509 g of nickel(II) chloride is dissolved in 100. mL of a 23.0 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) chloride is dissolved in it. Be sure your answer has the correct number of significant digits. (M)

Answer 1

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Weight of Nickel (II) chloride = 0.5099 Molar mass Nicla = 129.6 g/mol. .. moles of Niche - men .. weight = 0.509 mol Molar mass 129.6 " = 3.93x10-3 mol Nice → N, 2+ + 241 is moles of Np2+ ion = moles of Nicla = 393x10-3 mol Volume of solution - 100 ml. ó. Molarity [N2+] = moles of N; 2+ Volume of solution link) 3.93 x 10-3 -X1000 100 - 3.93 x 10-2 M Scanned with CamScanner