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pH from molarity and Ka

Chemistry
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A buffer solution is 0.441 M in HNO2 and 0.245 M in KNO2. If Ka for HNO2 is 4.5E-4, what is the pH of this buffer solution?

Apr 24th, 2015

. From the Henderson-Hasselbalch equationfor buffer of weak acid and salt of weak acid-strong base (Acidic buffer)

pH = pKa + log[KNO2] / [HNO2]

where pKa = - log[4.5 x 10^(-4)] = 3.347

pH = 3.347 + log [0.245] /[0.441]

=3.347 + log (0.555)

=3.347 -0.255 

=3.092 (answer)


Apr 24th, 2015

please  check soilution..any doubts do let me know..regards..Sumit sans

Apr 24th, 2015

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