Question

how many liters of a 3.01 m k2so4 solution are needed to provide 57.8 g of k2so4 (molar mass 174.01 g/mol )? recall that m is equivalent to mol/l .

Answer 1

To obtain 57.8 g of K2SO4 from a 3.01 M solution, 0.110 liters of the solution is required.

Step-by-step explanation:

To calculate how many liters of a 3.01 M K2SO4 solution are needed to provide 57.8 g of K2SO4, we first need to find the number of moles of K2SO4. The molar mass of K2SO4 is 174.01 g/mol, so we use the given mass to calculate the moles of K2SO4:

Moles of K2SO4 = Mass (g) / Molar Mass (g/mol) = 57.8 g / 174.01 g/mol ≈ 0.332 moles

Since molarity (M) is defined as moles of solute per liter of solution, we can rearrange the formula to solve for the volume (V) in liters:

Volume (L) = Moles of solute / Molarity (M) = 0.332 moles / 3.01 M ≈ 0.110 liters

Therefore, approximately 0.110 liters of the 3.01 M K2SO4 solution is needed to obtain 57.8 g of K2SO4.