Question

What is the molarity of 0.25 dm^3 of a solution containing 10.35 g of k2CO3? ​

Answer 1

Answer:

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Answer 2

Given:-

→Volume of the solution = 0.25dm³

→Mass of K₂CO₃ (solute) = 10.35g

To find:-

→Molarity of the solution

Solution:

•Atomic mass of Potassium(K) = 39u

•Atomic mass of Carbon(C) = 12u

•Atomic mass of Oxygen(O) = 16u

Thus, the molecular mass of K₂CO₃:-

= 39×2+12+16×3

= 78+12+48

= 138u

We know that molar mass is the molecular/atomic mass in grams. Thus, molar mass of K₂CO₃ is 138g.

Number of moles in 10.35g of K₂CO₃:-

= Given Mass/Molar mass

= 10.35/138

= 0.075 mole

Hence, 0.075 mole are there in 10.35g of K₂CO₃.

Now, let's convert the volume of the solution from dm³ to L.

=> 1dm³ = 1L

=> 0.25dm³ = 0.25×1

=> 0.25L

Molarity of a solution:-

= Moles of solute/Liters of solution

= 0.075/0.25

= 0.3 M

Thus, molarity of the solution is 0.3 M .