Explanation:
Mass of solute = 10.0 g
mass of solvent(water) = m
Volume of solvent( water) = v = 100.0 mL
Density of water= d = 


Mass of solution(M) = Mass of solute + mass of solvent
M = 10.0 g + 100.0 g = 110.0 g
Volume of the solution = V = 113 mL
Density of the solution = D

The density of the solution is 0.9734 g/ml.
Moles of phosphoric acid = 
Moles of water = 
Mole fraction of phosphoric acid =


Mole fraction of water =


![[Molarity]=\frac{\text{Moles of solute}}{\text{Volume of solution(L)}}](https://tex.z-dn.net/?f=%5BMolarity%5D%3D%5Cfrac%7B%5Ctext%7BMoles%20of%20solute%7D%7D%7B%5Ctext%7BVolume%20of%20solution%28L%29%7D%7D)
Moles of phosphoric acid = 0.1020 mol
Volume of the solution = V = 113 mL = 0.113 L ( 1 mL = 0.001 L)
Molarity of the solution :

![[Molality]=\frac{\text{Moles of solute}}{\text{Mass of solvent(kg)}}](https://tex.z-dn.net/?f=%5BMolality%5D%3D%5Cfrac%7B%5Ctext%7BMoles%20of%20solute%7D%7D%7B%5Ctext%7BMass%20of%20solvent%28kg%29%7D%7D)
Moles of phosphoric acid = 0.1020 mol
Mass of solvent(water) = m =100.0 g = 0.100 kg ( 1 g = 0.001 kg)
Molality of the solution :
