Alcl3 very acidic the higher the charge on the metal

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-AlCl3= very acidic (the higher the charge on the metal ion= the stronger the acidity of the hydrated ion QUALITATIVE PREDICTION OF pH FOR SOLUTIONS OF SALTS Ka > Kb pH<7 (acidic) Ka < Kb pH> 7 (basic) Ka= Kb pH= 7 (neutral) ACID SOLUTIONS IN WHICH WATER CONTRIBUTES TO H+ CONCENTRATION -If [H+] is greater than or equal to 10^-6 don’t count water [H+]= (Ka[HA]o + Kw)^1/2 Kw= [H+] [OH-] Charge balance: Positive & negative charges carried by ions must balance Material balance equation: HA originally dissolved must be present at equilibrium, as either A- or HA STRONG ACID SOLUTIONS IN WHICH WATER CONTRIBUTES TO THE H+ CONCENTRATION -If very dilute solution Ex. 1.0 x 10^-1 M HNO3= very dilute Use charge balance: [Positive charge]= [Negative charge] [H+]= [NO3-] + [OH-] Kw= [H+] [OH-] [H+]= [NO3-] + [Kw/ H+] -For dilute acids in water: [ H+]^2 – Ca[H+] – Kw= 0 *NEED TO KNOW STRONG ACIDS
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HCl, HClO4, HI, HBr, H2SO4, HNO3 *NEED TO KNOW STRONG BASES KOH, NaOH, LiOH, Sr(OH)2, Ba(OH)2, Ca(OH)2 *NEED TO KNOW WEAK BASES NH3, CO3^2-
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  • Fall '07
  • Holcombe
  • Equilibrium, Acids, Diprotic Acid

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