Question

Enough of a monoprotic weak acid is dissolved in water to produce a 0.0157 M solution. The pH of the resulting solution is 2.44 . Calculate the Ka for the acid. 

          Enough of a monoprotic weak acid is dissolved in water to produce a  0.0157
  M solution. The pH of the resulting solution is  2.44
 . Calculate the Ka for the acid.

Added by Yougot G.

Chemistry: Structure and Properties
Chemistry: Structure and Properties
Nivaldo Tro 2nd Edition
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Enough of a monoprotic weak acid is dissolved in water to produce a 0.0157 M solution. The pH of the resulting solution is 2.44 . Calculate the Ka for the acid.
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Transcript

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00:01 Here in this problem is given enough of a monoproteic weak acid is dissolved in water to produce a 0 .0157 molar solution the ph of the resulting solution is 2 .44 we have to calculate the k a for the acid now here ph given 2 .44 what is ph that is negative log concentration of h plus ions and that is equal to 2 .44 so concentration of h plus ion that will be 10 to the power of negative 2 .44 and we get 0 .0036 molar that's the concentration of h plus ion now let the weak acid be h a in aqueous solution it produces h plus ions and a minus ions let's set up the ice table initial concentration 0 .0157 here it is 0 and 0 and change concentration say negative x here it is positive x positive x equilibrium concentration initial minus change concentration here x and x...
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