A 0.1098 g sample of copper metal is dissolved in 34 mL of concentrated HNO3 to form Cu2+ ions and then water is added to make a total volume of 209.5 mL. (Calculate the molarity of Cu2+.)
moles Cu^2+ = grams/atomic mass.
The M = moles/L soln or moles/0.2095 = ?
Well, we could write a whole equation to solve this, but let's not get too chemical about it. Copper, like most metals, likes to dissolve in HNO3 when it's in a party mood. So, our first step is to calculate the moles of copper in that 0.1098 g sample. We can start by finding the molar mass of copper, which is about 63.55 g/mol. Then it's just a matter of dividing the mass by the molar mass to get the moles of copper.
0.1098 g / 63.55 g/mol ≈ 0.00173 mol
Now that we've got that out of the way, let's focus on the volume. Remember, we start with 34 mL of concentrated HNO3, and after adding water, we end up with a total volume of 209.5 mL. That means the final volume of copper solution is:
209.5 mL - 34 mL = 175.5 mL
And since we're in a molar mood, we need to convert mL to liters:
175.5 mL ÷ 1000 mL/L = 0.1755 L
Finally, we can calculate the molarity of Cu2+. This time, we divide the moles of copper by the volume in liters:
0.00173 mol / 0.1755 L ≈ 0.00988 M
So, the molarity of Cu2+ is approximately 0.00988 M. Just remember, when it comes to copper and HNO3, they're a real dynamic duo – like Batman and Robin, except with more chemistry and less capes. Keep mixing it up, my friend!
To calculate the molarity of Cu2+ ions, we need to determine the number of moles of Cu2+ ions and then divide it by the volume of the solution in liters.
Step 1: Convert the mass of copper to moles.
Given: Mass of copper = 0.1098 g
Molar mass of copper (Cu) = 63.55 g/mol
Using the formula: Moles = Mass / Molar Mass
Moles of copper = 0.1098 g / 63.55 g/mol
Step 2: Calculate the moles of Cu2+ ions produced.
In this reaction, each copper atom (Cu) is converted into one copper ion (Cu2+).
Moles of Cu2+ ions = Moles of copper
Step 3: Convert the volume of the solution to liters.
Given: Volume of the solution = 209.5 mL
1 L = 1000 mL
Volume of the solution in liters = 209.5 mL / 1000 mL/L
Step 4: Calculate the molarity of Cu2+ ions.
Molarity (M) = Moles of Cu2+ ions / Volume of the solution in liters
Substituting the values, we have:
Molarity = Moles of Cu2+ ions / Volume of the solution in liters
Now, let's perform the calculations.
Moles of copper = 0.1098 g / 63.55 g/mol = 0.001727 mol
Moles of Cu2+ ions = 0.001727 mol
Volume of the solution in liters = 209.5 mL / 1000 mL/L = 0.2095 L
Molarity = 0.001727 mol / 0.2095 L = 0.008248 M
Therefore, the molarity of Cu2+ ions is 0.008248 M.
To calculate the molarity of Cu2+, we need to know the moles of Cu2+ ions present in the solution.
First, let's determine the moles of copper (Cu) in the sample. The molar mass of copper is 63.55 g/mol.
Moles of Cu = Mass of Cu / Molar mass of Cu
Moles of Cu = 0.1098 g / 63.55 g/mol
Next, we need to calculate the moles of Cu2+ ions. Since copper is oxidized from an oxidation state of 0 to +2, each mole of Cu forms one mole of Cu2+.
Moles of Cu2+ = Moles of Cu
Now, we can find the molarity of Cu2+ using the equation:
Molarity (M) = Moles of solute / Volume of solution in liters
Since the volume of the solution is given in milliliters, we need to convert it to liters.
Volume of solution = 209.5 mL = 0.2095 L
Molarity of Cu2+ = Moles of Cu2+ / Volume of solution
Now, we can substitute the values into the equation and calculate the molarity of Cu2+.
Molarity of Cu2+ = Moles of Cu2+ / Volume of solution
Molarity of Cu2+ = Moles of Cu / Volume of solution
Molarity of Cu2+ = (0.1098 g / 63.55 g/mol) / 0.2095 L
By evaluating the expression, you will get the molarity of Cu2+.