To prepare a 400 mL solution of .7500 M NaC2H3O2, how many grams of NaC2H3O2 would be needed?

I am wondering if I set this up, I got an answer of .0435 g NaC2H3O2. But i'm not sure if that is right? Is that the correct answer?

That isn't the answer I obtained.

How many moles will you need? That will be M x L = 0.7500M x 0.400L = 0.300 moles. How many grams is that?
grams = moles x molar mass NaC2H3O2 = ??

To determine the number of grams of NaC2H3O2 needed to prepare a 400 mL solution with a concentration of 0.7500 M NaC2H3O2, you can use the formula:

Amount (in moles) = Concentration (in M) x Volume (in L)

First, convert the volume of the solution from milliliters to liters:

400 mL = 400/1000 L = 0.4 L

Now, substitute the given values into the formula:

Amount (in moles) = 0.7500 M x 0.4 L = 0.3 moles

To convert moles to grams, you need to know the molar mass of NaC2H3O2. The molar mass is calculated by adding up the atomic masses of all the atoms in a molecule.

The atomic masses are as follows:
Na: 22.99 g/mol
C: 12.01 g/mol
H: 1.01 g/mol
O: 16.00 g/mol

Now, calculate the molar mass of NaC2H3O2:
Molar mass (NaC2H3O2) = (22.99 g/mol) + 2 * (12.01 g/mol) + 3 * (1.01 g/mol) + 2 * (16.00 g/mol) = 82.03 g/mol

Finally, use the equation:

Mass (in grams) = Amount (in moles) x Molar mass (in g/mol)

Mass (in grams) = 0.3 moles x 82.03 g/mol ≈ 24.61 grams

Therefore, the correct answer is approximately 24.61 grams of NaC2H3O2. So, your initial answer of 0.0435 grams is not correct.