how many grams of NH4Cl are required to prepare 250 mL of .122 M NH4Cl solution?

I set this up using the molarity equation and the part that I was missing is moles. So I divided the 0.122 by .25 L and got .031 mol.

Then I took that and multiplied it by the molar mass of NH4Cl and got it wrong.
How do I do this problem?

Well, well, well, looks like you're in a bit of a pickle! But fear not, my friend, for Clown Bot is here to save the day with a side of laughter. Let's break it down.

To find the grams of NH4Cl needed, you have correctly calculated the moles of NH4Cl you need in your solution. However, multiplying it by the molar mass of NH4Cl is giving you some trouble. But worry not, I'll shed some light on it.

The molar mass of NH4Cl is 53.49 g/mol (approximately). So now, all you need to do is multiply the moles by the molar mass to get the grams of NH4Cl.

So, 0.031 mol × 53.49 g/mol = approximately 1.657 grams of NH4Cl. Ta-da!

And there you have it! The amount of NH4Cl you need to prepare your .122 M solution is approximately 1.657 grams, or roughly the size of a very enthusiastic clown nose. I hope this answer has brought a smile to your face!

To calculate the number of grams of NH4Cl required to prepare a 250 mL solution with a concentration of 0.122 M, you need to follow these steps:

Step 1: Calculate the number of moles of NH4Cl needed.
Molarity (M) = moles of solute / volume of solution in liters

Given:
Molarity (M) = 0.122 M
Volume of solution = 250 mL = 0.25 L

0.122 M = moles of NH4Cl / 0.25 L

Moles of NH4Cl = 0.122 M x 0.25 L
Moles of NH4Cl = 0.0305 mol

Step 2: Convert moles to grams using the molar mass of NH4Cl.
The molar mass of NH4Cl is:
N (14.01 g/mol) + H (1.007 g/mol) × 4 + Cl (35.45 g/mol)
Molar mass of NH4Cl = 14.01 + 1.007 × 4 + 35.45
Molar mass of NH4Cl = 53.49 g/mol

Grams of NH4Cl = Moles of NH4Cl x Molar mass of NH4Cl
Grams of NH4Cl = 0.0305 mol x 53.49 g/mol
Grams of NH4Cl ≈ 1.63 g

Therefore, you will need approximately 1.63 grams of NH4Cl to prepare a 250 mL solution with a concentration of 0.122 M NH4Cl.

To determine the number of grams of NH4Cl required to prepare a certain volume of a given molarity solution, you need to follow a few steps:

Step 1: Convert the given volume from milliliters (mL) to liters (L).
In this case, you have 250 mL, so divide it by 1000 to convert it to 0.250 L.

Step 2: Use the given molarity (M) and volume (in moles) to calculate the number of moles of NH4Cl.
The molarity (M) is given as 0.122 M, which means there are 0.122 moles of NH4Cl in every liter of solution. Multiply the molarity by the volume in liters:
0.122 M x 0.250 L = 0.0305 moles.

Step 3: Use the molar mass of NH4Cl to convert moles to grams.
The molar mass of NH4Cl can be calculated by adding up the atomic masses of its components:
N: 1 x 14.01 g/mol = 14.01 g/mol
H: 4 x 1.01 g/mol = 4.04 g/mol
Cl: 1 x 35.45 g/mol = 35.45 g/mol

Add the individual masses together: 14.01 g/mol + 4.04 g/mol + 35.45 g/mol = 53.50 g/mol.

Finally, multiply the number of moles by the molar mass to get the mass in grams:
0.0305 moles x 53.50 g/mol = 1.64 grams.

Therefore, you would need approximately 1.64 grams of NH4Cl to prepare a 250 mL solution with a molarity of 0.122 M.

What you did looks ok to me. 1.72 g?It could be that you rounded the 0.0305 to 0.031 too soon. You are allowed three significant figures so I would use 0.0305 for the moles required.