Answer :
Final answer:
The molarity of the solution prepared by diluting 20.2 ml of 2.10 M AgNO₃ to the final volume of 98.5 ml is 0.43 M.
Explanation:
The concept in focus here is molarity and dilution in chemistry. Molarity (M) is defined as the number of moles of solute per liter of solution. The question gives the initial volume and molarity of a AgNO₃ solution, and asks for the final molarity after dilution.
The principal equation used in dilution calculations is M₁V₁ = M₂V₂ where M₁ is the initial molarity, V₁ is the initial volume, M₂ is the final molarity, and V₂ is the final volume. In your question, M₁ = 2.10 M, V₁ = 20.2 ml, and V₂ = 98.5 ml. The final molarity, M₂, can be found by rearranging the equation to M₂ = M₁V₁/V₂.
Substituting the given values gives M₂ = (2.10 M * 20.2 ml) / 98.5 ml = 0.428 M (rounded to two decimal places). So the molarity of the diluted solution is 0.43 M.
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