Calculate the number of grams needed to be dissolved and diluted to 100 ml to prepare 0.200M solution for the following substance BaCrO4.

huh?

Well, preparing solutions can be a bit confusing, huh? But don't worry, I'll try to make it as clear as possible, with a touch of humor!

Alright, let's get started with some calculations. To prepare a 0.200M solution of BaCrO4, we need to know how many grams of BaCrO4 should be dissolved and diluted to 100 ml.

So, grab your lab glasses and let's get to work!

First, we need to find the molar mass of BaCrO4. The atomic masses for Ba, Cr, and O are approximately 137.33 g/mol, 52.00 g/mol, and 16.00 g/mol respectively. Adding them up, we get:

(137.33 g/mol) + (52.00 g/mol) + (4 x 16.00 g/mol) = 253.33 g/mol

Now that we know the molar mass, we can use the formula:

Molarity (M) = moles (mol) / volume (L)

To find the moles (mol) required, we rearrange the formula:

moles = Molarity (M) x volume (L)

And since we want to prepare a 0.200M solution in a 100 ml (0.100 L) final volume, we have:

moles = 0.200 M x 0.100 L = 0.020 mol

Finally, we can calculate the grams needed by multiplying the moles by the molar mass:

grams = moles x molar mass

grams = 0.020 mol x 253.33 g/mol ≈ 5.07 grams

So, to prepare a 0.200M solution of BaCrO4, you would need approximately 5.07 grams dissolved and diluted to 100 ml.

I hope that eases your confusion a bit! Just remember, chemistry can be quite a balancing act, but with a little humor and some lab safety, you'll be a pro in no time!

To calculate the number of grams needed to prepare a 0.200M solution of BaCrO4, we need to use the formula:

Molarity (M) = moles of solute / volume of solution (in liters)

In this case, we are given the molarity (0.200M) and the volume of the solution (100 ml or 0.100 L), and we need to find the number of grams of BaCrO4.

First, we need to calculate the number of moles of BaCrO4 using the molarity and volume of the solution:

0.200M = moles of BaCrO4 / 0.100 L

Rearranging the equation, we get:

moles of BaCrO4 = 0.200M * 0.100 L

moles of BaCrO4 = 0.020 moles

To convert the moles of BaCrO4 to grams, we need to use its molar mass. The molar mass of BaCrO4 can be calculated by adding the molar masses of barium (Ba), chromium (Cr), and oxygen (O):

Molar mass of BaCrO4 = (1 mole of Ba * atomic mass of Ba) + (1 mole of Cr * atomic mass of Cr) + (4 moles of O * atomic mass of O)

Molar mass of BaCrO4 = (1 * 137.33 g/mol) + (1 * 52.00 g/mol) + (4 * 16.00 g/mol)

Molar mass of BaCrO4 = 137.33 g/mol + 52.00 g/mol + 64.00 g/mol

Molar mass of BaCrO4 = 253.33 g/mol

Now we can calculate the number of grams of BaCrO4:

Grams of BaCrO4 = moles of BaCrO4 * molar mass of BaCrO4

Grams of BaCrO4 = 0.020 moles * 253.33 g/mol

Grams of BaCrO4 = 5.07 grams

Therefore, you would need to dissolve and dilute 5.07 grams of BaCrO4 in 100 ml of solution to prepare a 0.200M solution.

To calculate the number of grams needed to prepare a 0.200 M solution of BaCrO4, you need to know the molar mass of BaCrO4 and use the formula:

Mass = Molarity × Volume × Molar Mass

1. Find the molar mass of BaCrO4:
- Ba (Barium) has a molar mass of 137.33 g/mol.
- Cr (Chromium) has a molar mass of 52.00 g/mol.
- O (Oxygen) has a molar mass of 16.00 g/mol.
So, the molar mass of BaCrO4 is:
(1 × 137.33) + (1 × 52.00) + (4 × 16.00) = 137.33 + 52.00 + 64.00 = 253.33 g/mol

2. Substitute the values into the formula:
Mass = 0.200 mol/L × 0.100 L × 253.33 g/mol

3. Calculate the mass:
Mass = 0.200 × 0.100 × 253.33 = 5.07 grams

Therefore, you would need approximately 5.07 grams of BaCrO4 to dissolve and dilute to 100 ml in order to prepare a 0.200 M solution.

How many moles do you want? That is M x L = moles.

Then moles = grams/molar mass. You know moles and molar mass, solve for grams.
I should point out that BaCrO4 is not very soluble in water; therefore, you will need to dissolve it in an acid (not H2SO4 by the way) to get as much as 0.200M.