Calculate the pH of a solution containing 0.10 mole of acetic acid, to which is added 0.03 mole of sodium hydroxide (Ka = 1.8 x 10-5).
Moles of sodium acetate formed= 0.03 mol
Excess mole of acetic acid = 0.10-0.03=0.07 mol
It is acidic buffer,
pH = pKa + log(salt/acid)
= 4.74+log(0.03/0.07)
= 4.38
Calculate the pH of a solution containing 0.10 mole of acetic acid, to which is added...
(C))3.75 moo (D) 4.75 (E) 5.75 bios nA oir 9. Ka of acetic acid is 1.8 x 10. What is the pH of a solution 0.1M acetic acid and 0.05M sodium acetate? (A) 4.44 oasd A (B) 4.74 (C) 4.96 (D) 5.04 (E) 5.56 10. A buffer solution containing 0.5M acetic acid and 0.5M sodium acetate hais a pH ot 4.745. 5ml 2M sodium hydroxide is added to 995ml of the buffer solution. What is final pH? (A) 4.569 (C))3.75...
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