Question

100ml of 0.1 M urea solution is diluted upto 200ml then the molarity is...

Answer 1

Answer:

molarity =

Explanation:

m1v1=m2v2

100x0.1=200m2

10/200=m2

1/20=m2

0.5 is the answer of this question

Answer 2

The required molarity of the diluted solution is 0.05M.

Given:

100ml of 0.1M urea solution is diluted up to 200ml of solution.

To Find:

the molarity of the new diluted solution of 200ml.

Solution:

We can solve the problem in the following way.

(A solution is called the stock solution when it is concentrated form. The same solution when diluted to obtain a lower concentration is called a diluted solution.)

(The diluted solution that is obtained from the stock solution is generally sought for actual use.)

We know that if M1 = the molarity of the stock solution, V1= the volume of the stock solution, M2 = the molarity of the diluted solution, and V2 = the volume of the diluted solution; the equation for dilution is $M1V1=M2V2$.

We are aware of the fact that the amount of moles in any solution does not change irrespective of changing the concentration of the solution or the volume of the solution, and remains constant.

We can write the following equation from the given data.

$M1V1=M2V2\\100\times 0.1 =M2\times 200\\M2=\frac{10}{200} \\M2=0.05M$

Therefore, the required molarity of the diluted solution is 0.05M which is the final result.

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