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+.)
mols Cu = grams/atomic mass.
M = mols/0.2085L
To calculate the molarity of Cu2+ ions, we need to first determine the number of moles of Cu2+ ions present in the solution.
Step 1: Calculate the number of moles of Cu2+ ions produced.
Molar mass of Cu2+ = atomic mass of Cu = 63.55 g/mol
Number of moles of Cu2+ = mass of Cu2+ ions / molar mass of Cu2+
Since we have 0.1052 g of Cu, the number of moles of Cu2+ ions is:
moles of Cu2+ = 0.1052 g / 63.55 g/mol
Step 2: Calculate the volume of the solution in liters.
Since we are given the volume in milliliters, we need to convert it to liters.
Volume of solution = 208.5 mL = 208.5/1000 L
Step 3: Calculate the molarity of Cu2+ ions.
Molarity is defined as the number of moles of solute divided by the volume of the solution in liters.
Molarity of Cu2+ = moles of Cu2+ ions / volume of solution
Now, let's substitute the values we calculated to find the molarity of Cu2+ ions.
Molarity of Cu2+ = (0.1052 g / 63.55 g/mol) / (208.5/1000 L)
Simplifying the expression, we get:
Molarity of Cu2+ = (0.1052 / 63.55) / (208.5/1000)
Molarity of Cu2+ = 0.00166 M
Therefore, the molarity of Cu2+ ions in the solution is 0.00166 M.