157k views
2 votes
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.

User BMBM
by
8.6k points

2 Answers

2 votes

Final answer:

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.

User Themefield
by
8.1k points
1 vote

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

User Frilox
by
8.0k points
Welcome to QAmmunity.org, where you can ask questions and receive answers from other members of our community.