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o Calculate the pH of 500 ml of buffer solution containing .2M of ammonium sulphate and 0.3M ammonium hydroxide which 5 2.1% ionized in dilute solution. (kb of ammonium hydroxide is 1.8×10^-5)
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Respuesta :

Answer is 9

pKb=−logK

b=−log10^-5=5

  • A mixture of ammonium hydroxide and ammonium chloride forms a basic buffer solution.

  • Henderson's equation for the basic buffer solution is as given below-

pOH=pKb+log[acid]*[salt]

Substitute values in the above expression.

pOH=5+log0.1*0.1=5

Hence, the pH of the solution is pH=14−pOH=14−5=9

What do you mean by pH ?

  • potential of hydrogen
  • a measure of the acidity or alkalinity of a solution
  • equal to the common logarithm of the reciprocal of the concentration of hydrogen ions in moles per cubic decimetre of solution.
  • Pure water has a pH of 7,
  • acid solutions have a pH of less than 7,
  • and alkaline solution with a pH greater than 7.

Learn more about pH here

https://brainly.com/question/13557815

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