Calculate the mass ( g ) of the solute acetonitrile and the volume ( L ) of the solvent C6H6 that should be mixed to produce 4.72 kg of a solution that is 1.34 m acetonitrile.
molality = moles/kg solvent
moles = grams/molar mass.
The above two equations are needed.
equation 1.
You are given molality = 1.34 and kg solvent is 4.74 kg. Solve for moles.
Then use equation 2.
Plug in moles and molar mass, solve for grams.
Isn't 4.72Kg the mixed solution and the solvent?
To calculate the mass of the solute acetonitrile, we need to use the equation:
Mass = molarity * volume * molar mass
Given:
- The mass of the solution = 4.72 kg
- The molarity of acetonitrile = 1.34 M
First, let's convert the mass of the solution from kg to grams:
4.72 kg = 4720 g
Next, we need to find the molar mass of acetonitrile (CH3CN). The molar mass of carbon (C) is 12.01 g/mol, hydrogen (H) is 1.01 g/mol, and nitrogen (N) is 14.01 g/mol. We add them up to get:
12.01 g/mol + 3 * 1.01 g/mol + 14.01 g/mol = 41.05 g/mol
Now, we can rearrange the equation to solve for the volume of the solvent:
Volume = mass / (molarity * molar mass)
Volume = 4720 g / (1.34 mol/L * 41.05 g/mol)
Now let's solve for the volume of the solvent:
Volume = 84.367 L
Therefore, to produce 4.72 kg of a solution that is 1.34 M acetonitrile, you would need to mix 84.367 L of the solvent C6H6 (benzene) and the mass of the solute acetonitrile would be equal to the mass of the solution, which is 4720 g.