A student prepares a 2M solution of copper sulphate. She adds 17 mL of the solution to a 100 mL volumetric flask and dilutes it up to a final volume of 100 mL with water. What is the final molar concentration of the copper sulphate? How many moles of copper sulphate are in the 100 mL solution.
2M x (17/100) = ??M
To find the final molar concentration of the copper sulphate, we need to determine the concentration of the solution after dilution.
First, let's calculate the amount of copper sulphate that was added to the volumetric flask:
Amount of copper sulphate = concentration × volume
Amount of copper sulphate = 2 mol/L × 0.017 L
Amount of copper sulphate = 0.034 mol
Next, we need to find the final volume of the solution after dilution. This can be obtained by adding the initial volume of the solution (17 mL) to the final volume (100 mL):
Final volume = initial volume + volume after dilution
Final volume = 17 mL + 100 mL
Final volume = 117 mL
Now, we can calculate the final molar concentration of the copper sulphate solution using the formula:
Molar concentration = moles of solute / volume of solution (in liters)
Final molar concentration = 0.034 mol / (117 mL / 1000)
Final molar concentration ≈ 0.291 mol/L
Therefore, the final molar concentration of the copper sulphate solution is approximately 0.291 mol/L.
To determine the number of moles of copper sulphate in the 100 mL solution, we can simply use the given concentration:
Number of moles = concentration × volume
Number of moles = 2 mol/L × 0.100 L
Number of moles = 0.200 mol
Therefore, there are 0.200 moles of copper sulphate in the 100 mL solution.