Calculate the pH of each of the following solutions. (a) 0.17 M KNO2 (b) 0.37 M NaOCl (c) 0.50 M NH4ClO4
a) 0.17 M KNO2
C =0.17 M
Ka of HNO2 = 5.6×10–4
pKa = 3.25
KNO2 is salt of strong base and weak acid . so
pH = 7 + 1/2 (pKa + log C)
= 7 + 1/2 (3.25 + log 0.17)
= 8.24
pH = 8.24
(b) 0.37 M NaOCl
Ka of HClO = 4.0×10–8
pKa = 7.4
NaClO is salt of strong base and weak acid . so
pH = 7 + 1/2 (pKa + log C)
= 7 + 1/2 (7.4 + log 0.37)
= 10.48
pH = 10.48
(c) 0.50 M NH4ClO4
pKb of NH3 = 4.74
NH4ClO4 is salt of stong acid and weak base . so
pH = 7 - 1/2 (pKb + log C)
= 7 - 1/2 (4.74 + log 0.5)
= 4.78
pH = 4.78
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