A 0.25 M CuSO4 solution is required. A student is given 60 grams of copper sulphate. Calculate the volume of water needed to dissolve copper sulphate crystals and make this solution.
3 answers
Your answer
M is one mole of solute per liter of solution
using the molar mass, calculate the moles of CuSO4
then calculate the liters of solution for 0.25 M
using the molar mass, calculate the moles of CuSO4
then calculate the liters of solution for 0.25 M
For making a solution with predefined volume and concentration from a solid stock reagent (assuming 100% pure chemical), the formula ...
grams reagent needed = Molarity needed x Volume needed (Liters) x Formula Wt of reagent
So, for your problem ...
given 60 grams CuSO4 = 0.25 Molar solution x Volume needed (Liters) x 160 grams/mole CuSO4
Solve for Volume needed = 60g/[(0.25mole/L)(160g/mole)] = 0.150 L total volume solution = 150 ml total volume of solution...
Mixing should be as follows...
Transfer 60 grams CuSO4 into mixing container and follow with enough water to dilute to 150 ml... Now understand, that this method does Not say add 150 ml of water... It prompts one to add solvent (water) up to but not to exceed 150 ml total volume. The reagent will occupy some of the volume when dissolved.
grams reagent needed = Molarity needed x Volume needed (Liters) x Formula Wt of reagent
So, for your problem ...
given 60 grams CuSO4 = 0.25 Molar solution x Volume needed (Liters) x 160 grams/mole CuSO4
Solve for Volume needed = 60g/[(0.25mole/L)(160g/mole)] = 0.150 L total volume solution = 150 ml total volume of solution...
Mixing should be as follows...
Transfer 60 grams CuSO4 into mixing container and follow with enough water to dilute to 150 ml... Now understand, that this method does Not say add 150 ml of water... It prompts one to add solvent (water) up to but not to exceed 150 ml total volume. The reagent will occupy some of the volume when dissolved.
1 answer