Question

How many liters of a 3.67 M K2SO4 solution are needed to provide 57.3 g of K2SO4(molar mass 174.01 g/mol)? Recall that M is equivalent to mol/L.

Answer 1

To find the number of liters of a 3.67 M K2SO4 solution needed to provide 57.3 g of K2SO4, use the formula for molarity. First, find the number of moles of K2SO4. Then, rearrange the molarity formula to solve for volume.

Step-by-step explanation:

To find the number of liters of a 3.67 M K2SO4 solution needed to provide 57.3 g of K2SO4, we can use the formula for molarity:

Molarity (M) = Number of moles / Volume (in liters)

First, we need to find the number of moles of K2SO4. Using the molar mass of K2SO4 (174.01 g/mol), we can calculate:

Number of moles = mass / molar mass = 57.3 g / 174.01 g/mol.

Now, we can rearrange the molarity formula to solve for volume:

Volume (in liters) = Number of moles / Molarity = (57.3 g / 174.01 g/mol) / 3.67 M.

Calculating this expression will give us the number of liters of the K2SO4 solution needed.

Answer 2

Answer: Amount of volume needed in Litres is 0.09L

Explanation:

Given that the concentration in Mol/L =3.67M

Mass of K2SO4 = 57.3g

Molar mass of K2SO4 = 174.01g/mol

From stochiometry,

Mole = Mass/Molar mass

Mole = 57.3/174.01= 0.33mol.

Concentration in mol/L=

Mole/volume

3.67=0.33/volume

Volume= 0.33/3.67

Volume = 0.09L

Therefore the volume of K2SO4 needed is 0.09L