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pH and pOH calculations for weak acids and weak bases 1. What is the pH of...

pH and pOH calculations for weak acids and weak bases
1. What is the pH of a 0.55 M solution of trimethylamine (pKb= 4.13)
2. What is the pH of a 0.25 M solution of jaspersamine? The pKb value for jaspersamine 4.40.
3. What is the pH of a 0.15 M solution of a weak acid ammonium bromide given that the Kb value for ammonia is 1.8x10^-5.
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Answer #1

Following is the - complete Answer -&- Explanation: for Question - 1 and Question - 2, of the given: Question Set:... in....typed format...

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\RightarrowQuestion - 1:

\RightarrowAnswer:

For tri-methyl-amine:   pH = 11.805

\RightarrowExplanation:

Following is the complete Explanation: for the above: Answer.

  • Given:
  1. Molarity of Tri-methyl amine: Ma = 0.55 M ( mol/L )
  2. For  Tri methyl amine: value of pKb = 4.13
  • ​​​​​​​Step - 1:

​​​​​​​\Rightarrow  pKb = 4.13

\RightarrowKb = 10 -4.13 = 7.413 x 10-5   

  • Step - 2:

​​​​​​​\RightarrowWe know: Kb = [X+ ] x [OH - ] / [ tri-methyl amine ] = 7.413 x 10-5   

\Rightarrow [OH - ] = \sqrt{[Kb * [trimethyl amine]]} = ( \sqrt{[(7.413 * 10-5 ) x ( 0.55 ) ]} ) =  0.00638 M ( mol/L )

  • Step - 3:

​​​​​​​\RightarrowpOH = - log 10 [OH- ] = - log10 [ 0.00638 ] = 2.195

\Rightarrow pH =  ( 14.0 - pOH ) = ( 14.0 - 2.195 ) = 11.805

--------------------------------------------------------------------------------

\RightarrowQuestion - 2:

\RightarrowAnswer:

For jaspersamine:   pH = 11.5

\RightarrowExplanation:

Following is the complete Explanation: for the above: Answer.

  • Given:
  1. ​​​​​​​Molarity of jaspersamine: Ma = 0.25 M ( mol/L )
  2. For  jaspersamine: value of pKb = 4.40
  • ​​​​​​​Step - 1:

​​​​​​​\Rightarrow  pKb = 4.40

\RightarrowKb = 10 -4.40 = 3.98 x 10 -5   

  • Step - 2:

​​​​​​​\RightarrowWe know: Kb = [X+ ] x [OH - ] / [ jaspersamine ] = 3.98 x 10 -5

\Rightarrow [OH - ] = \sqrt{[Kb * [jaspersamine]]} = ( \sqrt{[(3.98 * 10^{-5} ) * ( 0.25 ) ]} ) =  0.00315 M ( mol/L )

  • Step - 3:

​​​​​​​\RightarrowpOH = - log 10 [OH- ] = - log10 [ 0.00315 ] = 2.50

\Rightarrow pH =  ( 14.0 - pOH ) = ( 14.0 - 2.50 ) = 11.5  

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Note: The remaining question: i.e. Question - 3: can be solved, by applying the method followed for solving the above stated solutions...

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