A solution is prepared by mixing Mt molesof the salt MCl2 (which dissociates com

Question

A solution is prepared by mixing Mt molesof the salt MCl2 (which dissociates completely to M+2 + 2Cl-) and Lt moles of the ligand HL in 1L. The following reactions may occur:

M+2 + L ---> ML+ K=1.0e8

HL (aq) ----> L- + H+ Ka=1.0e-5

a- Write a mass balance for the metal species

b- Write a mass balance for the ligand species

c- Write a charge balance

d- Suppose that Mt=Lt=0.1M (exactly) and the pH is somehow fixed at 5.00. (This means that the charge balance no longer applies.) Use the equilibria and the two mass balances to find the concentrations of ML+, M+2, L-, HL.

Explanation / Answer

n NaCl = 0.1 . 0.12 = 0,012 (moles)
n MgCl2 = 0.23 . 0.18 = 0,0414 (moles)

=> n Cl- = 0.012 + 0.0414. 2 = 0,0948 (moles)

Ag(+) + Cl(-) --> AgCl
0,0948<0,0948 (moles)

=> n Ag(+) = n AgNO3 = 0,0948 (moles)
=> V AgNO3 = n / CM = 0,0948 / 0,2 = 0,474 (litters)

moles glucose = 90.0 / 180 g/mol = 0.5
moles water = 712 / 18 g/mol = 3.96
mole fraction water = 3.95 / 3.96 + 0.5 = 0.888

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