The empirical formula for the Brilliant Blue dye is: C37H34N2O9S3Na2 and the formula weight are 792.86g/mol. How would you prepare a 5.25 x 10-6 M solution of Brilliant Blue dye. How many grams of the dye you need to add to a 1.00 L of water to make this solution.
Even though I have no idea what I am doing, I attempted to do the problem:
(5.25 x10^-6/1L)(1L/1000mL)(792.86 g/1 mol)= 4.2 x10^-6 g
Am I correct?
That is the answer for preparing 1mL.
did you intend on that?
(5.25 x10^-6 moles)(792.86 g/1 mol)=????? <= 3 significant figures.
M=moles/L
They question tells you that you need 1 L. So, in this case M=moles. The other conversion isn’t required to answer this problem.
My mistake, I did not intend for the other conversion. Thank you guys very much!
Well, it looks like you made a small mistake in your calculation. Let me help you out with the correct answer.
To prepare a 5.25 x 10-6 M solution of Brilliant Blue dye, you first need to calculate the number of moles required. The formula weight of the dye is given as 792.86 g/mol.
So, the number of moles required is:
(5.25 x 10-6 mol/L) x (1 L/1000 mL) = 5.25 x 10-9 mol
Now, to find the mass required, you can multiply the number of moles by the molar mass of the dye:
5.25 x 10-9 mol x 792.86 g/mol = 4.15 x 10-6 g
So, to prepare a 5.25 x 10-6 M solution, you would need to add approximately 4.15 x 10-6 grams of Brilliant Blue dye to 1.00 liter of water.
Please note that these calculations assume you have access to pure Brilliant Blue dye, and there are no other factors to consider in the solubility or stability of the dye.
You're close, but there is a small error in your calculation. Let's go through the steps to find the correct answer.
First, let's calculate the number of moles of Brilliant Blue dye required to make a 5.25 x 10^-6 M solution:
Molarity (M) = moles of solute / liters of solution
Given:
Molarity (M) = 5.25 x 10^-6 M
Liters of solution = 1.00 L
Therefore, moles of solute = Molarity (M) x Liters of solution
moles of solute = (5.25 x 10^-6 M) x (1.00 L) = 5.25 x 10^-6 moles
Now, let's use the moles of solute to calculate the grams of Brilliant Blue dye required:
Formula weight = grams / moles
Given:
Formula weight = 792.86 g/mol
moles of solute = 5.25 x 10^-6 moles
Therefore, grams of solute = Formula weight x moles of solute
grams of solute = (792.86 g/mol) x (5.25 x 10^-6 moles) = 4.16 x 10^-3 g
So, you need to add 4.16 x 10^-3 grams of Brilliant Blue dye to 1.00 L of water to prepare a 5.25 x 10^-6 M solution.
Note: When performing calculations like this, it is always good practice to use the correct number of significant figures. In this case, since the molarity was given with 3 significant figures, it is appropriate to report the grams of dye with 3 significant figures as well, giving the answer as 4.16 x 10^-3 g.