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

1.	What is the molarity of 0.25 dm^3 of a solution containing 10.35 g of k2CO3?
Answer» →Volume of the SOLUTION = 0.25dm³→Mass of K₂CO₃ (solute) = 10.35gTo FIND:-→Molarity of the solutionSolution:•Atomic mass of Potassium(K) = 39u•Atomic mass of Carbon(C) = 12u•Atomic mass of Oxygen(O) = 16uThus, the molecular mass of K₂CO₃:-= 39×2+12+16×3= 78+12+48= 138uWe 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 moleHence, 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=> 0.25LMolarity of a solution:-= Moles of solute/Liters of solution= 0.075/0.25= 0.3 MThus, molarity of the solution is 0.3 M .

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