The empirical formula for Brilliant Blie dye is C37 H34 N2 O9 S3 Na2, and the formula weight is 792.86 g/mol. How would you prepare a 4.73 X 10^-6 M solution of Brilliant Blue dye? How many grams of the dye do you need to add to a 1.00 L of water to make this solution?
I have no idea what this question is asking. Do you need to calculate a number or just explain what to do to create the dye? Thank you for your help because I am lost!!!
grams= Molarity*volumeinliters*molmass
= 4.73E-6*1*792.86 grams
I think the problem is asking for a detailed explanation of how to prepare 1 L of the soln including calculations.
You want a 4.73E-4M soln which means you want 4.73E-4 moles/L soln.
So you weigh the number of grams to obtain 4.73E-4 moles (moles = grams/molar mass), place that in a 1L volumetric flask, add enough water to dissolve all of the dye, then add additional water to the mark of the volumetric flask. Note that I did NOT (repeat NOT) say to add the grams of dye to 1 L water.
To prepare a 4.73 x 10^-6 M solution of Brilliant Blue dye, you will need to calculate the amount of dye needed to make this concentration in a 1.00 L solution.
The concentration of a solution is given by the formula:
Concentration (M) = (moles of solute) / (volume of solution in liters)
To calculate moles of solute needed, we can use the formula:
moles of solute = concentration (M) x volume of solution (L)
Given that the concentration is 4.73 x 10^-6 M and the volume of solution is 1.00 L, we can substitute these values into the formula:
moles of solute = (4.73 x 10^-6 M) x (1.00 L)
moles of solute = 4.73 x 10^-6 moles
Now we can calculate the mass of the dye needed using the molar mass (formula weight) of the dye, which is given as 792.86 g/mol:
mass of dye = moles of solute x molar mass
mass of dye = (4.73 x 10^-6 moles) x (792.86 g/mol)
mass of dye = 3.75 x 10^-3 grams
Therefore, you will need to add 3.75 x 10^-3 grams of Brilliant Blue dye to a 1.00 L solution of water to make a 4.73 x 10^-6 M solution of the dye.
To prepare a 4.73 x 10^-6 M solution of Brilliant Blue dye, you need to know the molar mass of the dye and the desired final volume of the solution.
First, let's calculate the number of moles needed to prepare the solution. The molar concentration (M) is defined as moles of solute per liter of solution. Rearranging this equation, we have:
M = moles of solute / volume of solution
Rearranging further, we get:
moles of solute = M x volume of solution
Given that the molar concentration (M) is 4.73 x 10^-6 M and the desired final volume of the solution is 1.00 L, we can substitute these values into the equation:
moles of solute = (4.73 x 10^-6 M) x (1.00 L)
Now, to calculate the grams of dye needed, we'll use the empirical formula and the formula weight. The empirical formula tells us the relative ratios of each element present in the compound, while the formula weight gives us the total mass of one mole of the compound.
The empirical formula for Brilliant Blue dye is C37 H34 N2 O9 S3 Na2. From this formula, we can calculate its formula weight as 792.86 g/mol.
To determine the number of moles needed, we first need to calculate the number of moles of each element in the empirical formula.
Number of moles of carbon (C) = 37 moles
Number of moles of hydrogen (H) = 34 moles
Number of moles of nitrogen (N) = 2 moles
Number of moles of oxygen (O) = 9 moles
Number of moles of sulfur (S) = 3 moles
Number of moles of sodium (Na) = 2 moles
To find the total moles of the compound, we add up the moles of each element:
Total moles of the compound = (37 + 34 + 2 + 9 + 3 + 2) moles
Now, we can calculate the grams of dye needed using the formula:
grams of dye = moles of dye x formula weight
Substituting the values we obtained:
grams of dye = [(37 + 34 + 2 + 9 + 3 + 2) moles] x (792.86 g/mol)
This calculation will give you the mass in grams of Brilliant Blue dye that needs to be added to prepare the 4.73 x 10^-6 M solution in 1.00 L of water.
Note: It's important to handle dyes and chemicals safely and responsibly. If you are not familiar with proper lab procedures, it is recommended to seek guidance from a qualified professional.