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What is the molarity of a solution when 20.0 mL of 1.55 M NaCl solution is diluted to a volume of 200.0 mL?

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Answer :

Final answer:

The molarity of the NaCl solution after it has been diluted to 200.0 mL from 20.0 mL is 0.155 M.

Explanation:

Your question is asking about the molarity of a solution after it has been diluted. Molarity is a measurement of the concentration of a solution, expressed in moles of solute per liter of solution.

In order to solve this, we'll use the formula M1V1 = M2V2. This formula states that the initial concentration (M1) times the initial volume (V1) is equal to the final concentration (M2) times the final volume (V2).

Given that the initial concentration (M1) is 1.55 M and the initial volume (V1) is 20.0 ml (or 0.02 L, when converted to liters), and that the final volume (V2) is 200.0 ml (or 0.2 L, when converted to liters), we substitute these values into our formula and solve for the final molarity (M2).

The result is: (1.55M) * (0.02L) = M2 * (0.2L)

By performing the necessary calculations, we find that M2, the molarity after dilution, is 0.155 M.

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