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A 0.1090 g sample of copper metal is dissolved in 60. ml of concentrated hno3 to form cu2+ ions and then water is added to make a total volume of 203.1 ml. (calculate the molarity of cu2+.)

Answer :

Chlidonias

Mass of Copper metal dissolved = 0.1090 g

Moles of Copper dissolved = [tex] 0.1090 g * \frac{1 mol}{63.55 g} = 0.00172 mol Cu [/tex]

Total volume of the solution = 203.1 mL [tex] * \frac{1 L}{1000 mL} = 0.2031 L [/tex]

Calculating the molarity of copper ions in the solution:

Molarity of a solution = [tex] \frac{Moles of solute}{Volume of solution (L)} [/tex]

= [tex] \frac{0.00172 mol Cu^{2+}}{0.2031 L} [/tex]

=0.00845 mol/L

Therefore the molarity of copper ions is 0.00845 mol/L

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