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Understanding Conjugate Acid and Base Pairs in Acid-Base Equilibria

Learn the concept of conjugate acid-base pairs in acid-base reactions, including polyprotic acids. Identify conjugate acids and bases and understand the ionization of monoprotic, diprotic, and triprotic acids. Explore examples and reactions.

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Understanding Conjugate Acid and Base Pairs in Acid-Base Equilibria

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  1. Acids & Bases Lesson #2 Conjugate Acid and Bases Polyprotic Acids

  2. Acids and Bases • Equilibria • Most acid base reactions can go forward and reverse • HF + SO32- HSO3- + F- Acid Base (donates proton) (accepts proton) • HF + SO32- HSO3- + F- Acid base Acid Base (donates proton) (accepts proton) Start wit h an acid and base on the reactant side and end up with an acid and base on the product side

  3. Conjugate Acid-Base Pairs • Looking at this reaction:HIO3 + NO2- HNO2 + IO3- acid base acid base HIO3 loses one proton (H+) to become IO3- on the • HIO3 is acting as an acid while IO3- is acting as a base

  4. Conjugate Acid-Base Pairs • HIO3 and IO3- form what is called a conjugate acid-base pair. • The only difference between these two is the IO3- has one less “H” and one more (-) charge than the HIO3. • All conjugate acid-base pairs are like this • The form with one more H (eg. HIO3) is called the conjugate acid. The form with one less H (eg. IO3-) is called the conjugate base.

  5. Conjugate Acid-Base Pairs • Out of every acid-base reaction, you always get 2 conjugate pairs. For example, in this reaction: • HIO3 + NO2- HNO2 + IO3- Acid base acid base • The two conjugate pairs are: Conjugate pair 1 Conjugate pair 2 HIO3 & IO3- NO2- & HNO2 Acid base base acid

  6. Conjugate Acids • Given an ion, find the conjugate base and conjugate acid • Find the conjugate Acid • Find the conjugate Acid of HSO4-

  7. Conjugate Bases • Find the conjugate base • Find the conjugate base of H2PO4-

  8. Polyprotic Acids •  So far, we’ve been looking at acids that only have one proton (H+) to release. • These are acids with one hydrogen in their formulas (eg. HCl, HNO3, HClO etc.) • Acids that release only one proton are called monoprotic acids. •  Example • acetic acid (CH3COOH) is monoprotic. • This is because only the “H” on the end of this acid (The “H” on the “COOH”) comes off in solution. • The other three “H”s are bonded directly and strongly to the Carbon atom in the “CH3” and are not released. • “H”s bonded directly to Carbon atoms (like in “CH3”, “CH3CH2” etc. ) are NOT released in solution and are not considered as “acidic protons”.

  9. Polyprotic Acids • The ionization of a monoprotic acid is quite simple, as we’ve seen before: • Example • HNO3(aq) + H2O(l)  H3O+(aq) + NO3-

  10. Polyprotic Acids • Acids that release two protons are called diprotic acids. • Some examples of diprotic acids are: H2SO4,, H2CO3, H2SO3 etc. • Acids that release three protons are called triprotic acids. • Some examples of triprotic acids are: H3PO4,, H3AsO4, H3BO3 etc. • Acids that release more than one proton are called polyprotic acids. • “polyprotic acids” would include“diprotic” and “triprotic” acids • Don’t look at any acids that release more than 3 protons

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