Calculate the molality of 6.00 M H2SO4 solution. The density of the solution is 1.34 g/mL.

7.98?

6.00 M is 6.00 moles/L of soln.

That is 6 moles x (98 g/mol) = 588 grams H2SO4 in the liter of soln..
Take 1 L of the solution. That will have a mass of volume x density = 1000 mL x 1.34 g/mL = 1340 grams. How much is H2SO4 and how much water. There are 588 grams H2SO4; therefore, 1340 g-588 = 752 g H2O.
molality = mols/kg solvent. You know moles H2SO4. You know kg solvent. You finish.

Yes, but check all my math leading up to that last step.

Well, it seems we have a real "acidic" situation here! To find the molality of the solution, we need to know the moles of solute (H2SO4) and the mass of the solvent (water). But wait, where is the mass of the water in this question? Don't worry, I've got a trick up my sleeve.

Since the density of the solution is given to be 1.34 g/mL, we can assume that the mass of the solution is equivalent to its volume (in mL). So, we can say that the mass of the solution is 1.34 g/mL multiplied by the volume of the solution in milliliters.

Now, to transform the volume from milliliters to liters, we divide by 1000. So, the mass of the solution is 1.34 g/mL multiplied by the volume in liters, which is 6.00 L.

Next, we need to find the moles of H2SO4 in the solution. The molarity of the solution is given as 6.00 M, which means there are 6.00 moles of H2SO4 per liter of solution.

So, we can multiply the molarity by the volume in liters (6.00 L) to find the moles of H2SO4.

Now that we have the moles of solute (H2SO4) and the mass of the solvent (water), we can calculate the molality of the solution using the formula:

Molality = Moles of Solute / Mass of Solvent (in kg)

So, let's put on our calculations hat and solve this equation!

To calculate the molality of a solution, you need to know the moles of solute dissolved in a certain mass of solvent. In this case, the solute is H2SO4 and the solvent is water.

To find the molality, follow these steps:

Step 1: Convert the given concentration from Molarity (M) to moles per liter (mol/L).
The concentration of the H2SO4 solution is given as 6.00 M, which means there are 6.00 moles of H2SO4 in 1 liter of solution.

Step 2: Convert the density of the solution from grams per milliliter (g/mL) to grams per liter (g/L).
The density of the solution is given as 1.34 g/mL. Since there are 1000 mL in 1 L, the density can be converted to 1.34 g/mL times 1000 mL/L, giving us 1340 g/L.

Step 3: Calculate the moles of H2SO4 in the solution.
Since the solution is 6.00 M, there are 6.00 moles of H2SO4 in 1 liter of solution. Therefore, in 1340 g/L of solution, there will be (6.00 moles/L) multiplied by (1340 g/L) moles of H2SO4. Calculate this value to find the number of moles of H2SO4 in the given mass of solution.

Step 4: Convert the mass of solvent to kilograms (kg).
Since molality is defined as moles of solute per kilogram of solvent, we need to convert the mass of solvent from grams to kilograms. Divide the given density (1340 g/L) by 1000 to get the mass of solution in kilograms.

Step 5: Calculate the molality.
Divide the calculated moles of H2SO4 in Step 3 by the mass of solvent in kilograms calculated in Step 4. This will give you the molality of the solution.

So, to calculate the molality of the 6.00 M H2SO4 solution with a density of 1.34 g/mL, follow these steps and perform the necessary calculations.