Calculate the pH of each of the following solutions.
a. 0.98 M KIO4
b. 0.24 M Ca(CH3CO2)2
c. 0.55 M HF
d. Mixture of 0.25 M HF in 0.25 M HBr
with work !
a) a. 0.98 M KIO4
KIO4 is the salt of strong acid and strong base. so pH should be 7
pH = 7
b) 0.24 M Ca(CH3CO2)2
Ca(CH3CO2)2 is the salt of weak acid and strong base . so the pH should be more than 7
pH = 7 + 1/2 [pKa + log C]
pH =7 + 1/2 [4.74 + log 0.24]
pH = 9.06
c) c. 0.55 M HF
pH = 1/2 [pKa - log C]
pH = 1/2 [3.20 -log 0.55]
pH = 1.73
d. Mixture of 0.25 M HF in 0.25 M HBr
HBr is strong acid HF is weak acid .so HBr acidity is dominent
[H+] = 0.25 M
pH = -log [H+]
pH = 0.602
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