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I can't find the answer of A 0.1052 g sample of copper metal is dissolved in 55 mL of concentrated HNO3 to form Cu2+ ions and then water is added to make a total volume of 208.5 mL. (Calculate the molarity of Cu2+.)

I calculated 0.1052*63.546/6.022e23/0.2085 but webassign told me its wrong

2 answers

You have
0.1052/63.546 = .0016555 moles Cu

.0016555mole/.2085L = .00794 M

Don't know why you tossed in Avogadro's number - who cares how many ions there are? Molarity is moles/liter. And, it makes no difference how the ions were produced. You are only interested in moles of Cu2+/liters of solution

I think
Steve thinks right. The 6.02E23 is extraneous to the problem.