Question

Calculate the concentration of a solution prepared by adding 15.00 mL of 2.00 × 10 − 3 M K M n O 4 from a buret into a 50.00 mL volumetric flask, which is then filled to the 50.00 mL graduation mark with distilled water.

Answer 1

Answer:

The concentration of the solution is 6 $10^{-4}$ mol/dm3.

Explanation:

We have the relationship between concentration and volume to be:

$c_{1} v_{1} = c_{2} v_{2}$   where c1v1 and c2v2 are initial and final concentrations and volumes respectively.

NOTE: (volume should be in litres if concentration is in Molar, M. But seeing as you have 2 × 10-3, I assume you have converted from mL to L already.)

15mL × 0.002mol/dm3 = 50mL × $x$ mol/dm3

∴ $x$ = $\frac{0.03}{50}$

= 0.0006 ≅ 6 ×$10^{-4}$mol/dm3

Answer 2

Based on the data provided, the final concentration of the solution is  6 * 10⁻⁴ mol/dm3

What is concentration of a solution?

Concentration of a solution is the amount of solute dissolved in a given volume of solution in litres.

The formula: C1V1 = C2V2 is used to calculate the concentration of solutions after dilution where

• C1 and C2 are initial and final concentrations and
• V1 and V2  are the final and initial volumes respectively.

Using C1V1 = C2V2:

15 × 0.002= 50 × C2

C2 = 6 * 10⁻⁴ mol/dm3

Therefore, the final concentration of the solution is  6 * 10⁻⁴ mol/dm3.

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