Question

If enough of a monoprotic acid is dissolved in water to produce a 0.0100 M solution with a pH of 6.75, what is the equilibrium constant, Kg, for the acid?

Answer 1

first identify the H+ from pH and then construct the ICE table and substitute the values in the Ka equation and calculate the value as follows

Monopotic And HA HA - Het + Á I 0.0100 0 0 ¢ x tx txe (0.01-2 Quj - Ka= [44] [A] Ull well ... LHAS But pH=6.15 pHs Hog (ht? 5) [ht] = 1,778 x167 M P.e [ht] =[4] = 1.778 X107 ka = (1.778 8107) 2 (0.01–1.778x167) ka = 3,162 XOR Acquees : 3.162 xrohr 3.162 X