The molal boiling point elevation constant Kb = 1.97 C .Kg. Mol-1 for a certain substance X. When 31.98 g of urea are dissolved in 650.G of X. The solution boils at 137.0 C. Calculate the boiling point of pure X

Boiling point of pure liquid is 135.4°C

Explanation:

The boiling point elevation (Colligative property of solutions) follows the formula:

ΔT = Kb×m×i

ΔT is equal to increase in boiling point (Boililng point solution - boiling point pure liquid), Kb is boiling point elevation constant of the liquid, m is molality of solution and i is Van't Hoff factor.

Molality of solution (Moles urea / Kg X):

Moles urea: 31.98g * (1mol / 60.06g) = 0.53247 moles

-60.06g/mol = Molar mass urea-

In 650g = 0.650kg:

0.53247 moles urea / 0.650kg = 0.8192m

Van't Hoff factor of urea is 1

Replacing in the equation:

ΔT = Kb×m×i

ΔT = 1.97°CKgMol⁻¹×0.8192m×1

ΔT = 1.6

As the solution boils at 137°C:

ΔT = Boililng point solution - boiling point pure liquid

ΔT = 1.6°C = 137.0°C - boiling point pure liquid

Boiling point of pure liquid is 135.4°C

answer: e.   sour taste

explanation: acids are those substances which dissociates in water to give ions. as they dissociate to give ions, they act as electrolytes and thus are electrically conductive. acids are sour in taste. example: hcl

bases are those substances which dissociates in water to give ions or accepts ions. as they dissociate to give ions, they act as electrolytes and thus are electrically conductive. bases are bitter in taste. bases are slippery in nature.