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Answer 1 · 2016-01-03T18:57:50

The conjugate bases are #"F"^-# and #"ClO"^-#.

According to the Brønsted-Lowry theory, an acid #"HA"# donates a proton to a base #"B"#.

Its conjugate base #"A"^-# is the product remaining after the loss of the proton.

#bb"HF"#

The equation for #"HF"# reacting with a base #"B"# is

#underbrace("HF")_color(red)("acid") + "B" ⇌ underbrace("F"^-)_color(red)("conjugate base") + "BH"^+#

The conjugate base is #"F"^-#.

#bb"HClO"#

The equation for #"HClO"# is

#underbrace("HClO")_color(red)("acid") + "B" ⇌ underbrace("ClO"^-)_color(red)("conjugate base") + "BH"^+#

The conjugate base is #"ClO"^-#.