If Kb for NX3 is 7.0×10−6, what is the pOH of  a 0.175 M aqueous solution of  NX3? 2: If Kb for NX3 is 7.0×10−6, what is the percent ionization of a  0.325 M aqueous solution of NX3? 3: If Kb for NX3 is 7.0×10−6 , what is the the pKa for the following reaction? HNX3+(aq)+H2O(l)⇌NX3(aq)+H3O+(aq)

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1: If Kb for NX3 is 7.0×10−6, what is the pOH of  a 0.175 M aqueous solution of  NX3?
2: If Kb for NX3 is 7.0×10−6, what is the percent ionization of a  0.325 M aqueous solution of NX3?
3: If Kb for NX3 is 7.0×10−6 , what is the the pKa for the following reaction?
HNX3+(aq)+H2O(l)⇌NX3(aq)+H3O+(aq)
 
Many common weak bases are derivatives of NH3,
where one or more of the hydrogen atoms have been
replaced by another substituent. Such reactions can
be generically symbolized as
=
NX3(aq) + H₂O(1) ⇒ HNX3+ (aq) + OH(aq)
where NX3 is the base and HNX3+ is the
conjugate acid. The equilibrium-constant expression
for this reaction is
Kb =
where K₁, is the base ionization constant. The extent
of ionization, and thus the strength of the base,
increases as the value of K₁, increases.
K₂ and Ki are related through the equation
Kax Kb = Kw
As the strength of an acid increases, its Ką value
increase and the strength of the conjugate base
decreases (smaller K₁ value).
[HNX3+][OH-]
[NX3]
Transcribed Image Text:Many common weak bases are derivatives of NH3, where one or more of the hydrogen atoms have been replaced by another substituent. Such reactions can be generically symbolized as = NX3(aq) + H₂O(1) ⇒ HNX3+ (aq) + OH(aq) where NX3 is the base and HNX3+ is the conjugate acid. The equilibrium-constant expression for this reaction is Kb = where K₁, is the base ionization constant. The extent of ionization, and thus the strength of the base, increases as the value of K₁, increases. K₂ and Ki are related through the equation Kax Kb = Kw As the strength of an acid increases, its Ką value increase and the strength of the conjugate base decreases (smaller K₁ value). [HNX3+][OH-] [NX3]
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