Exercise 2 (Equilibria of Weak Acids and Bases, Solubility Equilibria of Ionic Compounds) 1. Write the ionization equati

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Exercise 2 Equilibria Of Weak Acids And Bases Solubility Equilibria Of Ionic Compounds 1 Write The Ionization Equati 1 (46.5 KiB) Viewed 44 times

Exercise 2 (Equilibria of Weak Acids and Bases, Solubility Equilibria of Ionic Compounds) 1. Write the ionization equation of each acid or base in water and corresponding equilibrium constant, Kaforatid K for base a) HCIO₂ (aq) b) H₂C₂O4 (aq) (Hint: Write the equilibrium reaction in which H₂C₂O4 gives away ONE H".) c) (CH3)2NH (aq) (Hint: This is an organic base.) d) HCO3(aq) acting as a weak base 2. Compare the strengths of weak acids and bases. a) K₂ of HSO, is 6.2 x 108 and K, of HCN is 4.0 x 10-¹0. Which acid is weaker? Which solution is more acidic? Why? b) Kb of ClO is 2.9 x 107 and Ks of NH3 is 1.5x 103. Which base is stronger? Which solution is more basic. Why. 3. Write the balanced dissolving equation and the solubility product expression for each of the following slightly soluble ionic compounds in a saturated aqueous solution: ay Mg.(PO₂)2 (s) b) Cu₂CO3(s) 4. Ksp for FeS is 4 x 10-19 and Ksp for PbS is 7 x 1029 which metal surfiae is less soluble? Why?