A solution is made by dissolving 6.4 g of bromine (Br2) in enough CCl4 to make 80 mL of solution. What is the molarity of the solution formed?
I got 5.006 but I'm not too sure if it is correct. Thanks to anyone who checks this
Molarity= molessolute/literssolution= (6.4/160)/.080)=.5
Well, let's dive into the question, shall we?
First of all, I have to say, bromine seems like a pretty clingy element. It doesn't like to let go easily, does it?
Now, let's focus on the numbers here. You dissolved 6.4 grams of bromine in enough CCl4 to make 80 mL of solution. That's quite an intimate bromine-CCl4 relationship you have there.
To find the molarity of the solution, we need to calculate the number of moles of bromine. Don't worry, the molar team is always ready for action!
The molar mass of bromine (Br2) is approximately 159.8 g/mol. So, to calculate the number of moles, we divide the mass (6.4 g) by the molar mass (159.8 g/mol).
6.4 g / 159.8 g/mol = 0.04006 mol
Now that we know the number of moles, we can determine the molarity by dividing the moles by the volume (in liters). I see you have 80 mL of solution, but we need it in liters, right?
So, we divide the volume (80 mL) by 1000 to convert it to liters.
80 mL / 1000 = 0.08 L
Now, finally, we can calculate the molarity by dividing the moles (0.04006 mol) by the volume in liters (0.08 L).
Molarity = 0.04006 mol / 0.08 L = 0.50075 M
So, it seems like the molarity of the solution is approximately 0.50075 M.
And remember, wherever there's a bromine, there's often some trouble brewing!
To find the molarity of the solution, we need to first calculate the moles of bromine (Br2) present in the solution, and then divide it by the volume of the solution in liters.
1. Calculate the moles of Br2:
Molar mass of Br2 = 79.904 g/mol
Mass of Br2 = 6.4 g
Moles of Br2 = Mass of Br2 / Molar mass of Br2
= 6.4 g / 79.904 g/mol
2. Convert the volume of the solution to liters:
Volume of solution = 80 mL = 80 / 1000 L
= 0.08 L
3. Calculate the molarity (M) of the solution:
Molarity (M) = Moles of solute / Volume of solution
= Moles of Br2 / Volume of solution
= (6.4 g / 79.904 g/mol) / 0.08 L
Molarity (M) ≈ 5.02 M
Therefore, the molarity of the solution formed is approximately 5.02 M, not 5.006 M.
To find the molarity of the solution, you need to determine the number of moles of bromine (Br₂) dissolved in the solution and then divide it by the volume of the solution in liters.
First, let's calculate the number of moles of bromine:
1. Determine the molar mass of bromine (Br₂), which is 79.9 g/mol (2 * 79.9 = 159.8 g/mol).
2. Divide the mass of bromine (6.4 g) by its molar mass (159.8 g/mol) to find the number of moles:
Number of moles = mass / molar mass
Number of moles = 6.4 g / 159.8 g/mol
After dividing, you should get approximately 0.04 moles (rounded to two decimal places).
Now, let's calculate the molarity of the solution:
3. Convert the volume given from milliliters (mL) to liters (L). Since there are 1000 mL in a liter, divide the volume by 1000:
Volume in liters = 80 mL / 1000
After dividing, you should obtain 0.08 L.
4. Divide the number of moles of bromine by the volume in liters to find the molarity:
Molarity = moles / volume in liters
Molarity = 0.04 moles / 0.08 L
After dividing, you should get 0.5 M (rounded to one decimal place).
So, the molarity of the solution formed is 0.5 M. Your answer of 5.006 M is incorrect.