Question

An aqueous solution containing 0.5 mole of glucose in 2 L of solution, is diluted by adding 18 L of water. Final mole of solute in the solution is​

Answer 1

Answer:

6.0×10¹⁸ is it the correct answer

Answer 2

Given: Number of moles of glucose = 0.5

          The volume of glucose = 2L

          Water added = 18L

To find: Final mole of solute in the solution

Solution:

If we dilute the solution by adding water of some volume, then the mole of solute in the solution will be equal to

C₂ =( V₁ × C₁ )/V₂

Where C₁ is the mole of solute before diluting, V₁ is the volume of solution before diluting, V₂ is the total volume of solution, C₂ is the mole of the solute after diluting.

V₂ will be equal to 2 + 18 = 20L

Putting the value into the equation we get,

C₂ = ( 0.5 × 2 ) / 20

    = 1/20 = 0.05

Therefore, the mole of solute in solution after diluting will be equal to 0.05