If a buffer solution is 0.190 M in a weak acid (Ka = 5.8 x 10^-5) and 0.550 M in its conjugate base, what is the pH?
What if it said "if a buffer solution is ___ M in a weak base (Kb = ____) and ___ M in its conjugate acid, what is the pH? Would the steps from the first problem still be identical to this problem?
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The steps would be the same. Use the Henderson-Hasselbalch equation for both.
Thank you! we havn't covered this in lecture yet so I wasn't sure what the formula was called
1 answer