Calculate the volume in liters required to prepare a 5.00M solution of HCL using 15.4gof HCL.

You have 15.4 g HCl. How many mols is that? That's mols HCl = grams HCl/molar mass HCl.

The M = mols/L solution.
You know M and mols, solve for L.

To calculate the volume of a solution, we need to use the formula:

Volume (in liters) = mass (in grams) / density (in g/mL) = mass (in grams) / (concentration (in mol/L) x molar mass (in g/mol) )

First, let's find the molar mass of HCl (Hydrochloric acid):

H (hydrogen) has a molar mass of 1.01 g/mol, and Cl (chlorine) has a molar mass of 35.45 g/mol. Since HCl contains one hydrogen atom and one chlorine atom, we can add their molar masses together to find the molar mass of HCl:

Molar mass of HCl = 1.01 g/mol + 35.45 g/mol = 36.46 g/mol

Next, we need to convert the mass of HCl given (15.4g) to moles using the molar mass of HCl:

Moles of HCl = mass (in grams) / molar mass (in g/mol) = 15.4g / 36.46 g/mol ≈ 0.423 mol

Now, we can use the molarity (5.00M) and the equation mentioned above to find the volume of the solution:

Volume (in liters) = moles of solute / concentration (in mol/L) = 0.423 mol / 5.00 mol/L ≈ 0.0846 L

To convert the volume from liters to milliliters, multiply by 1000:

Volume (in mL) = 0.0846 L x 1000 mL/L = 84.6 mL

Therefore, to prepare a 5.00M solution of HCl using 15.4g of HCl, you would need approximately 84.6 mL of HCl.