10% (m/m) aqueous potassium iodide has a density of 1.202 g mL-1 . The true statements about this solution are

10% solution of Kl contains, 10 g of KI in 90 g (or 0.09 kg) of water. Molar mass of KI = (39 +127) g mol-1 = 166 g mol-1∴molality of solution=Number of moles of KIMass of water (in kg)                                   =10g/166gmol−10.09kg            =0.67molkg−1 Further,Molarity (M)= Moles of KI  Volume of solution(inL)                                  =10g/166gmol−1×1000100g/1.202gmL−1=10/166×100083.19[∵ Volume = Mass / density =100/1.202=83.19mL]                                                      =0.72molL−1=0.72M Number of moles of KI=10g166gmol−1=0.06mol Number of moles of water =90g18gmol−1=5mol Mole fraction of KI=nKInKI+nH2O                                =0.065+0.06=0.065.06=0.01186