What are deltaTb and deltaTf for an aqueous solution that is 1.5g nacl in 0.250kg h2o? Given Kb=0.51 C/m and kr=1.86 C/m

Question

asked Jun 6, 2020 214k views

1 Answer

Lebolo · Answer 1 · 2020-06-10T18:58:02+0000

Answer:

for given question is 2.79 and
is 0.52

$\Delta T_b = I * K_b * m$ {i- vant hoff’s constant ; Kb- constant ; m molarity }

M = no. of moles of the solute present in one kg of solution

Let the weight of amount of solute be “w” and its molecular mass be “M”

Let the mass of the solvent in the given question be “x”

$\Delta T_b = I * K_b * (w/M)/ x$

$\Delta T_b = I * K_b * w/Mx$

$\Delta T_b = 1 * 0.51 *1.5/(0.250 * 58.44) = 0.052$

$\Delta T_f = M * K_f = 1.86 * 1.5 = 2.79$