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+.)
See the post above.
To calculate the molarity of Cu2+ ions, we first need to determine the number of moles of Cu2+ ions formed. We can use the given mass of the copper metal to achieve this.
1. Calculate the number of moles of copper metal:
- Given mass of copper metal = 0.1052 g
- Copper has a molar mass of 63.55 g/mol.
- Number of moles of copper = mass / molar mass = 0.1052 g / 63.55 g/mol
2. Next, we need to find the number of moles of Cu2+ ions formed. Since copper metal is oxidized to Cu2+ ions, the moles of copper are equal to the moles of Cu2+ ions.
3. Now we can calculate the molarity of Cu2+ ions:
- Molarity (M) is defined as moles of solute divided by volume of solution in liters.
- Volume of solution in liters = 208.5 mL / 1000 (since 1 L = 1000 mL)
- Molarity of Cu2+ = moles of Cu2+ / volume of solution (in liters)
By following the steps above and plugging in the values, you should be able to calculate the molarity of Cu2+ ions.