If A Buffer Solution Is 0 × e@ning.cor × ing.com/ibiscms/mod/ibis/view.php?id 41
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If A Buffer Solution Is 0 × e@ning.cor × ing.com/ibiscms/mod/ibis/view.php?id 4167082 ng Jump to... Print Cak lator-Perodie Tabe uestion 1 of 28 Sapling Learning At a concentration of 1M,the weak acid HNO2 is 2% ionized and the pH of the solutin is 1.7. What happens when KNOs) is dissolved into the solution? The concentration of H increases According to Le Châtelier's principle, addition of NO2 will shift the acid-ionization reaction to the left what happens to when the equilibrium shifts leftward? The pH IncreasesExplanation / Answer
HNO2(aq) <-----> H+(aq) + NO2-(aq)
if you add KNO2 to the above solution then KNO2 is completely ionized,
KNO2 (aq) -----> K+(aq) + NO2-(aq)
BY the above reaction the concentration of NO2- increases.
Due to the common ion effect the NO2- react with H+ ion and reverse the reaction to form HNO2.SO the concentration of HNO2 increases.
Hence the dissocition of HNO2 decreases.and also the H+ ion concentration decreases.
pH = -log[H+]
If [H+] ion concentration decreases then pH of the solution increases from 1.7 to higher from the above formula