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Question Intro: When an amide (NH2-) is dissolved in water,


Intro: When an amide (NH2-) is dissolved in water, it acts as a strong base according to the reaction NH2-(aq) + HSO(l) —–> NH3(aq)+OH-(aq) In contrast, ammonia dissolved in water results in the equilibrium: NH3(aq)+H2O(l)<—->NH4+(aq)+OH-(aq) The equilibrium constant expression for this reaction is Kb= [NH4+][-OH]/[NH3] NOTE: that we add a subscript “b” to the equlibrium constant to designate it as a weak base equilibrium. Ka Kb=Kw for all conjugate acid-base pairs pKa+pKb=pKw=14 Equations for pH calculations: pH+pOH=14 Ka=10^-pKa (same for Kw and Kb) pKa=-log10(Ka) Kw[H3O+][OH-]=1X10^-14 AT 25C pKw=14
part 1) The equilibrium constants for bases are given the label, Kb. Write the equilibrium constant expression for NH3(aq) in water ( the reaction is given above)
Part 2) Deteremine whether each species below can act as an acid or a base. Write the reaction that would occur in water for each given species. Identify the conjugate acid (or conjugate base) for each reaction. Write the equilibrium constant expression (Ka or Kb) for each reaction below
a) HCN b) HOCl C) CH3COO- d)HClO4 e) HNO3
Part 3)
a) Calculate the pH for a solution containing 2.53×10^-2 M H3O+(hydronium ion). Is this an acidic or basic solution
b) Calculate the pOH for the same solution.

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