<, =, Neutral, Basic.
Since the molarity of either acid is the same, the moles of each acid are equal. That means the difference between their pH is determined solely on which acid dissociates more. Since the strong acid dissociates more (releases more
#H^+#ions), it will have a lower pH.
Since both acids are monoprotic (they only release one hydrogen) they will both take the same amount of
#OH^-#to be neutralized.
The conjugate acid/base of strong acids and bases aren't strong enough to ionize water, so the pH will be exactly 7.
The conjugate base of the weak acid is strong enough to react with water to form
#OH^-#, causing the pH to be basic.
Strong Acid + Strong Base Titration at eqv pt => pH = 7
Weak Acid + Strong Base Titration at eqv pt => pH >7
Mixing of equal volumes of equimolar acid and base solutions will react completely. The pH at the equivalence points will be a function of salt ion hydrolysis.
Since neither of the salt ions reacts with water, the pH of a strong acid + strong base titration at the equivalence point is exclusively dependent upon the autoionization of water.
We set up an ICE table as usual.