A solution of H2SO4(aq) with a molal concentration of 6.25 m has a density of 1.300 g/mL. What is the molar concentration of this solution?

Didn't I work this for you a couple days ago? 6.25m means 6.25 mols/kg solvent.

6.25 mol H2SO4 = 6.25 x molar mass = ? grams H2SO4.
Then solvent = 1000, H2SO4 = ? grams = total mass solution. Use density to convert to mL, convert to L and M = mols/L soln. Post your work if you get stuck.

15,3

To find the molar concentration of the solution, we need to convert the molal concentration to molar concentration using the density of the solution.

Given:
Molal concentration (m) = 6.25 m
Density = 1.300 g/mL

Step 1: Convert density to kg/L
Since density is given in g/mL, we need to convert it to kg/L:
1 g/mL = 0.001 kg/mL
Multiply the given density by 0.001 to convert it to kg/L:
Density = 1.300 g/mL x 0.001 kg/g = 0.0013 kg/mL

Step 2: Convert molal concentration to moles of solute
Molal concentration (m) is defined as moles of solute per kg of solvent.
To find the moles of solute, we need to multiply the molal concentration by the mass of the solvent.
In this case, the solvent is water (H2O) since we are working with an aqueous solution.

For every 1000 g (1 kg) of water, the molal concentration corresponds to the molar concentration (M).

So, to find the moles of solute per liter (1000 mL) of solution (M), we can multiply the molal concentration by the density of the solution:

Molar concentration (M) = molal concentration (m) x density

Molar concentration (M) = 6.25 m x 0.0013 kg/mL

Step 3: Convert the density from kg/mL to kg/L
To convert the density from kg/mL to kg/L, we need to multiply it by 1000 mL/L.
So, 0.0013 kg/mL x 1000 mL/L = 1.3 kg/L

Substituting the values into the equation from Step 2:

Molar concentration (M) = 6.25 m x 1.3 kg/L

Molar concentration (M) = 8.125 M

Therefore, the molar concentration of the solution is 8.125 M.

To find the molar concentration (or molarity) of the solution, we need to convert the given molal concentration into molar concentration.

Molal concentration (m) is defined as the number of moles of solute per kilogram of solvent. In this case, the given molal concentration is 6.25 m, which means there are 6.25 moles of solute per kilogram of solvent (water in this case).

First, we need to convert the density of the solution (1.300 g/mL) to the mass of the solution.

Given:
Density of the solution = 1.300 g/mL

To convert the density to mass, we can use the formula:
mass = density x volume

Since the density is given in grams per milliliter (g/mL), we need to convert the volume of the solution to milliliters (mL).

Assuming the solution has a volume of 1 liter (1000 mL), the mass of the solution can be calculated as:
mass = 1.300 g/mL x 1000 mL = 1300 g

Next, we need to find the mass of the solvent (water) in the solution. We can assume that the density of water is 1 g/mL.

Using the formula:
mass = density x volume

The mass of the water can be calculated as:
mass = 1 g/mL x 1000 mL = 1000 g

Now, we have the mass of the solute (H2SO4) and the solvent (water), and we can calculate the molar concentration (molarity).

To convert molal concentration to molar concentration, we need to consider the molecular weight (molar mass) of the solute. The molecular weight of H2SO4 is 98.09 g/mol.

The equation for converting molal concentration to molar concentration is:
Molarity (M) = (molal concentration x molecular weight) / solvent mass

Molarity (M) = (6.25 m x 98.09 g/mol) / 1000 g

Calculating the result:
Molarity (M) = 0.613 M

Therefore, the molar concentration of the solution is 0.613 M.