A piece of nickel is placed in a beaker with 350 mL of copper (II) sulfate. Calculate the concentration of the copper (II) sulfate solution.
Initial mass of nickel - 15.5 g
Final mass of nickel - 11.4 g
What do i do with the final and initial masses of nickel?
CuSO4(aq) + Ni ==> NiSO4(aq) + Cu
mass Ni used = 15.5 - 11.4 = ??g Ni.
Convert mass Ni to mols Ni. mols = grams/molar mass.
Mols Ni = mols Cu (from the equation which tells you 1 mol CuSO4 = 1 mol Ni).
mols Cu = mols CuSO4 (since 1 mol Cu is in 1 mol CuSO4).
molarity CuSO4 = mols/L.
To calculate the concentration of the copper (II) sulfate solution, we need to use the mass change of the nickel. Here's what you can do with the final and initial masses of nickel:
1. Calculate the mass of nickel lost:
Mass lost = Initial mass of nickel - Final mass of nickel
= 15.5 g - 11.4 g
= 4.1 g
2. Convert the mass of nickel lost to moles. Since the molar mass of nickel is 58.69 g/mol:
Moles of nickel = Mass lost / Molar mass of nickel
= 4.1 g / 58.69 g/mol
3. Use the balanced chemical equation between nickel and copper (II) sulfate to determine the moles of copper (II) sulfate reacted. The equation is:
Ni + CuSO4 → NiSO4 + Cu
The stoichiometric ratio is 1:1, meaning 1 mole of nickel reacts with 1 mole of copper (II) sulfate.
4. Assume that all the copper (II) sulfate has reacted, the moles of copper (II) sulfate reacted is equal to the moles of nickel:
Moles of copper (II) sulfate = Moles of nickel
5. Finally, calculate the concentration of the copper (II) sulfate solution in moles per liter (Molarity):
Concentration (M) = Moles of copper (II) sulfate / Volume of solution (L)
= Moles of copper (II) sulfate / 0.350 L (since the volume of the solution is stated as 350 mL)
I hope this helps! Let me know if you have any further questions.
To calculate the concentration of the copper (II) sulfate solution, we need to use the concept of stoichiometry. Since we have the masses of nickel before and after the reaction, we can determine the amount of nickel that reacted with the copper (II) sulfate.
1. Calculate the change in mass of nickel: Initial mass - Final mass
Change in mass = 15.5 g - 11.4 g = 4.1 g
2. Determine the moles of nickel that reacted with copper (II) sulfate using the molar mass of nickel.
Molar mass of nickel = 58.69 g/mol
Moles of nickel reacted = Change in mass / Molar mass
Moles of nickel reacted = 4.1 g / 58.69 g/mol
3. Write and balance the chemical equation for the reaction between nickel and copper (II) sulfate:
Ni + CuSO4 -> NiSO4 + Cu
4. Since the reaction is a 1:1 ratio between nickel and copper (II) sulfate, the moles of nickel reacted would be the same as the moles of copper (II) sulfate.
5. Calculate the volume of copper (II) sulfate solution in liters.
Volume of copper (II) sulfate = 350 mL = 350/1000 L
6. Calculate the concentration of copper (II) sulfate using the formula:
Concentration (molarity) = Moles of copper (II) sulfate / Volume of copper (II) sulfate
Now, substitute the values into the formula to calculate the concentration:
Concentration = Moles of nickel reacted / Volume of copper (II) sulfate
= (4.1 g / 58.69 g/mol) / (350/1000 L) = (0.070 mol) / (0.350 L)
= 0.20 M
Therefore, the concentration of the copper (II) sulfate solution is 0.20 M.