Question

How many grams of K2CO3 are needed to prepare a 400.0 mL of a 4.25M solution?

Answer 1

Answer:

235 g

Explanation:

From the question;

• Volume is 400.0 mL
• Molarity of a solution is 4.25 M

We need to determine the mass of the solute K₂CO₃,

we know that;

Molarity = Number of moles ÷ Volume

Therefore;

First we determine the number of moles of the solute;

Moles = Molarity × volume

Moles of  K₂CO₃ = 4.25 M × 0.4 L

                           = 1.7 moles

Secondly, we determine the mass of  K₂CO₃,

We know that;

Mass = Moles × Molar mass

Molar mass of  K₂CO₃, is 138.205 g/mol

Therefore;

Mass = 1.7 moles × 138.205 g/mol

         = 234.9485 g  

         = 235 g

Thus, the mass of  K₂CO₃ needed is 235 g