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torquemada
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Homework Statement
(c) A 0.1036 g sample of copper metal is dissolved in 48 mL of concentrated HNO3 to form Cu2+ ions and then water is added to make a total volume of 208.1 mL. (Calculate the molarity of Cu2+.)
Homework Equations
Molarity = Moles/Liter
The Attempt at a Solution
.1036g/63.55g/mol = .0016302124 moles
.0016302124/.2081 (moles of Copper Ions over final Volume in liters) = .0078337935 M - webassign says this is wrong. I'm thinking perhaps the reaction between copper metal and HNO3 to yield Cu2+ ions isn't 1:1 in stoichiometry and maybe i have to balance the equation and use oxidation states to get it right but i have no idea how to approach balancing this reaction because I'm not even clear what the products are and then I'm not sure if water does anything additional to the solution besides add volume, maybe some other reaction happens? thx
The molarity they want is the molarity of Cu2+