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I usually just look at the products of the equation, and the product with an additional H+ is the conjugate acid because bases accept protons based on the Bronsted- Lowry definition. Similarly, since acids donate protons, the product with an H+ taken away from it will be the conjugate base
The acid on the reactants side of the equation will have a proton that it will lose on the products side. This is how you can identify the Bronsted acid on the reactants side, and the opposite is true for the Bronsted base. Once you have found the Bronsted acid and base, you should remember that the conjugate base is the one on the products side that has lost a proton and the conjugate acid is the one on the products side that has gained a proton.
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