Slide 1Slide 2Slide 3Write the dissociation equations for each of the acids shown on the previous slide. Identify the acid and its conjugate base.Remember that diprotic and triprotic acids will have 2 and 3 conjugate acid-base pairs, respectively. H2SO4 H+ + HSO4-Sulfuric acid (H2SO4):diprotic acid HAAcidA-conjugatebase HAAcidA-conjugatebaseH+ + SO4=Same for carbonic acid (H2CO3).H3PO4 has 3 conjugate acid-base pairs.Acetic acid is monoprotic: CH3COOH H+ + CH3COO- Homework CommentWrite the equations for the complete dissociation of each of these acidsHCl H+ + Cl-HNO3 H+ + NO3-H2SO4 H+ + HSO4- H+ + SO4-2HF H+ + F-CH3COOH H+ + CH3COO-H2CO3 H+ + HCO3- H+ + CO3-2H3PO4 H+ + H2PO4- H+ + HPO4-2 H+ + PO4-3**diprotic (2 protons to donate;2 A-B pairs, 2 Kas)‡ - triprotic (3 protons to donate; 3 A-B pairs; 3 Kas)‡*Homework AnswersRemember that in any aqueous solution: [H+] [OH-] = 1 x 10-14 What is [H+] (in moles/L or M) when [OH-] = 1 x 10-6 M 1 x 10-8 M 1 x 10-2 M 1 x 10-12 0.00005 M 2 x 10-10 0.1 M 1 x 10-13 5.68 x 10-5 M 1.76 x 10-10 2.65 x 10-12 M 3.77 x 10-3 What is [OH-] (in moles/L or M) when [H+] = 1 x 10-8 M 1 x 10-6 M 1 x 10-10 M 1 x 10-4 0.008 M 1.25 x 10-12 0.0000000001 M 1 x 10-4 5.68 x 10-9 M 1.76 x 10-6 2.65 x 10-7 M 3.77 x 10-8Homework
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