Questions in solutions

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	The expression relating mole fraction of solute $({{x}_{2}})$and molarity (M) of the solution is (Where $\rho$ is the density of solution and ${{M}_{1}}$and ${{M}_{2}}$are the molar masses of solvent and solute, respectively)
	A molal solution of sodium chloride has a density of $1.21\,g\,m{{l}^{-1}}.$The molarity of this solution is
	The molality of a sulphuric acid solution in which the mole fraction of water is 0.85 is
	150 ml of ${{C}_{2}}{{H}_{5}}OH$(density =0.78 g/ml) is diluted to one litre by adding water; molality of the solution is
	An aqueous solution of non-electrolyte ‘A’ with molecular mass 60 contains 6 g in 500 mL and has a density equal to $1.05\,g\,{{L}^{-1}}$. The molality of solution is
	An aqueous solution of urea containing 18 g urea in $1500\,c{{m}^{3}}$of the solution has density equal to 1.052. If the molecular weight of urea is 60, then the molality of the solution is
	How many grams of $NaOH$ will be required to neutralize 12.2 grams of benzoic acid
	The volume of 95% ${{H}_{2}}S{{O}_{4}}$$\text{(density}=1.85\,c{{m}^{-3}}\text{)}$ needed to prepare $100\,c{{m}^{3}}$of 15% solution of ${{H}_{2}}S{{O}_{4}}$$\text{(density}=1.10\,c{{m}^{-3}}\text{)}$ will be
	How many moles of $F{{e}^{2+}}$ion are formed when excess iron is treated with 50 ml of 4.0 N $HCl$ under inert atmosphere? Assume no change in volume
	A 0.01M ammonia solution is 5% ionised. The concentration of $O{{H}^{-}}$ions is