Question

what is the molarity of the solution obtained by diluting 13.9 ml of 18 m h₂so₄ to 100 ml?

Answer 1

Answer:

M1V1 = M2V2

18 x 13.9 = M2 x 100

250.2/100 = M2

M2 = 2.502

Answer 2

Given,

18M solution of $H_{2} SO_{4}$

To find,

Molarity of the solution obtained by diluting 13.9ml of given solution to 100ml.

Solution,

Molarity of the solution is given as,

$M = \frac{moles}{volume(l)}$

Where, $moles = \frac{mass}{molar mass}$ and $volume$ is taken in liters.

Calculating moles of $H_{2} SO_{4}$ that are present in 13.9ml of the given solution,

             $18 = \frac{moles}{13.9*10^{-3} }\\moles = 18*13.9*10^{-3}$

New volume = 13.9ml from previous solution + 100ml of added water for                                dilution.

New volume = $13.9 + 100ml = 113.9ml = 113.9*10^{-3}l$

The molarity of the solution formed will be equal to the ratio of moles present in 13.9 ml of a given solution and the net volume obtained after dilution.

                                                    = $\frac{18*13.9*10^{-3} }{113.9*10^{-3} }M$

                                                    $= \frac{250.2}{113.9}M\\= 2.196M$

Therefore, the molarity of the new solution is $2.196M.$