List of top Chemistry Questions on Solutions asked in AP EAMCET

At \( T(K) \), two liquids A and B form an ideal solution. The vapour pressures of pure liquids A and B at that temperature are 400 and 600 mm Hg respectively. If the mole fraction of liquid B is 0.3 in the mixture, the mole fractions of A and B in vapour phase respectively are:
0.1 mole of H\(_3\)PO\(_3\) is present in 500 mL of solution. The normality of it is:
At 300 K, the vapour pressures of A and B liquids are 500 and 400 mm Hg respectively. Equal moles of A and B are mixed to form an ideal solution. The mole fraction of A and B in vapor state is respectively.
Two statements are given below:
Statement - I: Liquids A and B form a non-ideal solution with positive deviation. The interactions between A and B are weaker than A-A and B-B interactions.
Statement - II: For an ideal solution, \( \Delta H_{\text{mix}} = 0 \), \( \Delta V_{\text{mix}} = 0 \).
The correct answer is
A solution containing 18.25g of HCL and 500g of water. Find molality.
 
Dissolving $120\, g$ of a compound (mol. wt $= 60$) in $1000\, g$ of water gave a solution of density $1.12\, g \, mL^{-1}$. The molarity of solution is
Benzene and toluene form an ideal solution over the entire range of composition. Hie vapour pressure of pure benzene and toluene at $T (K)$ are $50\, mm \,Hg$ and $40\, mm \,Hg$ respectively. What is the mole fraction of toluene in vapour phase when $117\, g$ of benzene is mixed with $46\, g$ of toluene ? (molar mass of benzene and toluene are $78$ and $92\, g\, mol^{-1}$ respectively)