[" A "0.001" molal actulion of a complex (MAn) in water has the treezing point of "-0,0054^(@)C" ."],[" 100" lonization of the complex salt and "K" is "H_(2)O=1.86km^(-1)" ,white the correct represental "],[" complex "],[[" 1) (MA) "," (2) IMAyA "," (3) IMA.) "," (4) IMA."]]

A .001 molal solution of a complex [MA_8] in water has the freezing point of -0.0054^@C . Assuming 100% ionization of the complex salt and K,for H_2O 1.86Km^-1 , write the correct representation for the complex

A 0.001 molal aqueous solution of a complex [MA_8] has the freezing point of -0.0054^(@)C . If the primary valency of the salt undergoes 100% ionization and K_f for water =1.8 K molality^(-1) the correct representation of complex is

A 0.001 molal aqueous solution of a complex [MA_8] has the freezing point of -0.0054^(@)C . If the primary valency of the salt undergoes 100% ionization and K_f for water =1.8 K molality^(-1) the correct representation of complex is

The 0.0001 molal solution of a complex AB_(10) has the freezing point of -0.0015^(@)C in water. Assuming 100% dissociation of the complex, find the proper representation of the complex [K_(f)(H_(2)O=1.86Km^(-1))] (a) [AB_(8)] (b) [AB_(3)]B_(7) (c ) [AB_(7)]B_(3) (d) [AB_(5)]B_(5) .

The freezing point of a 0.05 molal solution of a non-electrolyte in water is: ( K_(f) = 1.86 "molality"^(-1) )

The freezing point of a 0.05 molal solution of a non-electrolyte in water is: ( K_(f) = 1.86 "molality"^(-1) )

An aqueous solution of urea has freezing point of -0.52^(@)C . If molarity and molality are same and K'_(f) for H_(2)O = 1.86 K "molality"^(-1) the osmotic pressure of solution would be:

A 0.025 m solution of mono basic acid had a freezing point of 0.06^(@)C . Calculate K_(a) for the acid K_(f) for H_(2)O=1.86^(@) "molality"^(-1) .