A 0.20-molar solution of a weak monoprotic acid HA has a pH of 3.00. The equilibrium constant is: a. 2.0x10^-3 b. 5.0x10^-3 c. 2.0x10^-7 d. 5.0x10^-6 e. 5.0x10^-7
Added by George P.
Step 1
We know the pH of the solution, which is 3.00. We can use this to find the concentration of H+ ions in the solution: $pH = -\log[H^+]$ $3.00 = -\log[H^+]$ $H^+ = 10^{-3}$ Show more…
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