Question

Calculate the volume in liters of a ×1.0310−6mM silver(II) oxide solution that contains 900.mg of silver(II) oxide AgO.

Answer 1

Answer : The volume of solution will be, $7.047\times 10^6L$

Explanation : Given,

Mass of AgO = 900 mg  = 900000 g

conversion used : (1 mg = 1000 g)

Molar mass of AgO = 124 g/mole

Molarity of AgO = $1.03\times 10^{-6}mM=0.00103M$

Molarity : It is defined as the number of moles of solute present in one liter of solution.

Formula used :

$\text{Molarity}=\frac{\text{Mass of solute}}{\text{Molar mass of solute}\times \text{volume of solution in liter}}$

Now put all the given values in this formula, we get the active mass of urea.

$0.00103M=\frac{900000g}{124g/mole\times \text{volume of solution in liter}}$

$\text{volume of solution in liter}=7046664.579L=7.047\times 10^6L$

Therefore, the volume of solution will be, $7.047\times 10^6L$