A 0.1052 g sample of copper metal is dissolved in 55 mL of concentrated HNO3 to form Cu2+ ions...
Question:
A 0.1052 g sample of copper metal is dissolved in 55 mL of concentrated {eq}HNO_3 {/eq} to form {eq}Cu_2 {/eq}+ ions and then water is added to make a total volume of 208.5 mL.
Calculate the molarity of {eq}Cu_2 {/eq}+.
Molarity
Molarity is another name for the concentration and is the number of moles of Solute per litre of solution.
Molarity is important when we are considering pH as well as neutralisation reactions
Answer and Explanation:
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View this answerFirst, to solve this question we must find the number of moles of Copper metal dissolved:
{eq}n(Cu) = \frac{m(Cu)}{A(Cu)} = \frac{0.1052}{63.546} =...
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