All of the halides salts of Ag following equilibrium: except AgF) have a very lo

Question

All of the halides salts of Ag following equilibrium: except AgF) have a very low solubility in water. The compound AaB, exists in soutic as the AgBr (s)Ag+ (aq) Br (aq) Using the data in the table given: AgF (s) AgCl (s) AgBr (s) AgI (s) Ag+ (aq) F (aq) Cl-(aq) Br-(aq) I-(aq) AH,o (in kJ/mol) 204.6 -127.1 -100.4 -61.8 105.6 -332.6 -167.2 -121.5 -55.2 So (in J/mol K) 84.0 96.2 107.1 115.572.7-13.8 56.5 82.4 111 a) Calculate the Ho (in k /mol) for dissolving AgBr in aqueous solution. kl/mol b) Calculate the ASo (in J/molK) for dissolving AgBr in aqueous solution. J/molk c) Calculate the Go (in kJ/mol) for dissolving AgBr in aqueous solution at 25°C. d) What is the value for Ksp at this temperature?

Explanation / Answer

DH0rxn = (DH0f,Ag+ + DH0f,Br-)-(DH0f,AgBr(s))

       = (105.6+-121.5)-(-100.4)
     
        = 84.5 kj/mol

DS0rxn = (S0f,Ag+ + S0f,Br-)-(S0f,AgBr(s))

      = (72.7+82.4)-(107.1)

      = 48 j/mol.k

dG0 = DH0-TDS0

    = (84.5)-(298*48*10^-3)

     = 70.2 kj

DG0 = -RTlnKsp

70.2*10^3 = -8.314*298lnKsp

Ksp = 4.95*10^-13

Related Questions

Navigate

• Browse (All)
• Browse A
• Subjects

---