What should be the boiling point of `1.0 molal` aqueous `KCl` solution (assuming complete dissociation of KCl) if `K_(b)^(H_(2)O)` is `0.52 K m^(-1)`?

The molal elevation constant of water = 0.52 K m^(-1) . The boiling point of 1.0 molal aqueous KCl solution (assuming complete dissociation of KCl ) should be

The molal elevation constant of water = 0.52 K m^(-1) . The boiling point of 1.0 molal aqueous KCl solution (assuming complete dissociation of KCl ) should be

The molal elevation constant of water = 0.52 K m^(-1) . The boiling point of 1.0 molal aqueous KCl solution (assuming complete dissociation of KCl ) should be

The molal elevation constant of water = 0.52 K m^(-1) . The boiling point of 1.0 molal aqueous KCl solution (assuming complete dissociation of KCl ) should be

The molal elevation constant of water = 0.52 K, molality^-1 . The boiling point of 1.0 molal aqueous KCl solution (assuming complete dissociation of KCl), should be:

What is the boiling point of 1 molal aqueous solution of NaCl (K_b)=0.52 K molal^-1]

What is the boiling point of 1 molal aqueous solution of NaCl [K_b = 0.52 K molal ^(-1)] .