# Chemistry

posted by .

Calculate the volume ( L ) of the solute water and the volume ( L ) of the solvent tetrahydrofuran that should be added to generate 4.73 kg of a solution that is 1.36 m water.

• Chemistry -

m = moles/Kg solvent.
1.36 = moles water/4.73
moles H2O = 1.36 x 4.73 = 6.43
moles water amd 6.43 x 18 g/mol = 115.7 g
You can look up the density of water and the density of tetrahydrofuran and convert from grams to L. I must point out that this will NOT, howver, have a mass of 4.73 kg for the SOLUTION. The solution will have a mass of 4.73 kg + 0.116 kg = 4.85 kg.

You can go through another iteration by subtracting the water from the THF and redoing the calculation like this.
1.36 = moles H2O/(4.73-0.116)
1.36 x 4.61 = 6.28 moles water.
6.28 x 18 = 113 grams or 0.133 kg H2O.
That will be a total mass of solution of 0.113 + 4.62 kg solvent = 4.73 for the solution and that would satisfy the criteria. I don't know if you intended to write SOLUTION or solvent.
You can check this number to see if it produces 1.36 m in H2O.
113 g H2O = 6.28 moles.
That in 4.62 kg THF = 6.28/4.62 = 1.36 m

## Similar Questions

1. ### Chemistry

What volume (mL) of the solvent benzene should be added to 142 mL of the solute CH3CN to generate a solution that is 2.68% by mass CH3CN?

What volume ( L ) of the solute methanol should be added with 4450 mL of the solvent water to make a solution that is 0.443 m methanol. i do not know how to approach this question
3. ### chemistry

Calculate the volume ( L ) of the solute C3H8O3 and the mass ( g ) of the solvent H2O that should be added to produce 6050 g of a solution that is 1.17 m C3H8O3.
4. ### Chemistry

Calculate the volume (L) of the solute C4H8O and the volume (mL) of the solvent C2H5OH that should be combined to prepare 5.54 kg of a solution that is 0.608 m. Molar Mass (g/mol) C4H8O 72.12 C2H5OH 46.07 Density (kg/L): C4H8O 0.8892 …
5. ### FlunkyJunkie

Calculate the volume (mL) of the solute (CH3)2CO and the volume (L) of the solvent H2O that should be added to prepare 1.36 kg of a solution that is 25.7 g (CH3)2CO per 100. g solution. Molar Mass (g/mol) (CH3)2CO 58.05 H2O 18.015 …
6. ### chemistry

Calculate the volume (mL) of the solute (CH3)2CO and the volume (L) of the solvent H2O that should be added to prepare 1.36 kg of a solution that is 25.7 g (CH3)2CO per 100. g solution. Molar Mass (g/mol) (CH3)2CO 58.05 H2O 18.015 …
7. ### Chem

Calculate the volume ( mL ) of the solute acetic acid and the volume ( L ) of the solvent H2O that should be added to generate 5.01 kg of a solution that is 0.694 m acetic acid. volume ( mL ) of the CH3CO2H volume ( L ) of the H2O …
8. ### chemistry

a. Find the amount of solute based on this information Volume = 500 ml Concentration of solution= 15% (w/w) Solute (molar mass) = H2SO4 is 98.0g/mol b. Find the molar mass Amount of solute= 117.0g Volume of solution= 2.00L concentration …
9. ### chemistry

a. Find the amount of solute based on this information Volume = 500 ml Concentration of solution= 15% (w/w) Solute (molar mass) = H2SO4 is 98.0g/mol b. Find the molar mass Amount of solute= 117.0g Volume of solution= 2.00L concentration …
10. ### chem

Water is the solvent and you can assume the density of water is 1.0g/cc. a.) What will be the amount of solute in grams if the volume is 500 mL and the concentration of solution is 15% w/w?

More Similar Questions