He mole fraction of potassium nitrate in an aqueous solution is 0.0194. the solution's density is 1.0627 g/ml. calculate the molarity of the solution.

The solution contains potassium nitrate (KNO3) in water (H2O)

The molar mass of KNO3 = 101 g/mol

The molar mass of H2O = 18 g/mol

Mole fraction of KNO3 = 0.0194

Therefore mole fraction of H2O = 1 - 0.0194 = 0.9806

Total mass of the solution = KNO3 + H2O

= 0.0194 moles * 101 g/mol + 0.9806 moles * 18 g/mol

= 1.9594 g + 17.6508 = 19.6102 g

Volume of the solution = Mass of solution/density

= 19.6102 g/ 1.0627 g.ml-1 = 18.453 ml = 0.01845 L

Molarity of KNO3 = moles of KNO3/volume of solution

= 0.0194 mole/0.01845 L = 1.05 M

The mole fraction of potassium nitrate in an aqueous solution is 0.0194. The solution's density is 1.0627 g/mL. What is the molarity of KNO3 in the solution?

Explanation:

m=9

step-by-step explanation:

  the   balanced   equation   for   reaction of   ca metal   with   o2 to   produce   cao   is as below

2 ca+ o2→ 2 cao2

  explanation

the reaction is   balanced     since the   number of atoms   in reactant side is   equal to   number of atoms   in   product side.   for   example   they   are 2   atom of   ca in   reactant   side   and   2   atoms of ca   in   the product side.

  the   process   is a   meet the   requirement   of   redox   reaction because :     calcium   is   oxidized   from   oxidation state 0   to 2+   while   oxygen   is reduced from   oxidation   state   0   to 2-