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Acids & Bases

This guide explores the fundamentals of acids and bases, including how to calculate pH, understand pOH, and apply the ion-product constant of water (Kw). It covers concepts like the self-ionization of water, and classifications of solutions as acidic, basic, or neutral based on hydrogen and hydroxide ion concentrations. Readers will find examples for practical application of pH calculations and detailed rules for naming binary and ternary acids. This thorough resource is ideal for students and anyone seeking clarity in acid-base chemistry.

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Acids & Bases

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  1. Acids & Bases Calculating pH and Naming

  2. Finding the pH of Solutions Self- ionization of water – the simple dissociation of water H2O H+ + OH- Concentration of ea. ion in pure water: [H+] = 1.0 x 10-7M + [OH-] = 1.0 x 10-7M Ion-product constant for water (Kw),Where Kw = 1.0 x 10-14 Kw = [H+] [OH-] Acid [H+] > [OH-] Base [H+] < [OH-] Neutral [H+] = [OH-]

  3. pH Scale pH = -log[H+] pOH = -log[OH-] pH + pOH = 14

  4. Example 1. If the [H+]in a solution is 1.0 x 10-5M, is the solution acidic, basic or neutral? 1.0 x 10-5 M What is the concentration of the [OH-]? Use the ion-product constant for water (Kw): Kw = [H+] [OH-] 1.0 x 10-14 = [1.0 x 10-5] [OH-] 1.0 x 10-14 = [OH-] 1.0 x 10-5 1.0 x 10-(14-5) pH 5 = acidic 1.0 x 10-9 OH-

  5. Examples 2. If the pH is 9, what is the concentration of the hydroxide ion? Kw = [H+] [OH-] 1.0 x 10-14 = [1.0 x 10-9] [OH-] 1.0 x 10-5 = [OH-] 14 = pH + pOH 14 = 9 + pOH 5 = pOH 3. If the pOH is 4, what is the concentration of the hydrogen ion? Kw = [H+] [OH-] 1.0 x 10-14 = [H+] [1.0 x 10-4] 1.0 x 10-10 = [H+] 14 = pH + pOH 14 = pH + 4 10 = pH

  6. Example 4. A solution has a pH of 4. Calculate the pOH, [H+] and [OH-]. Is it acidic, basic, or neutral? • pOH = 14.00- 4 = 9 • acidic

  7. Fill in the chart. 1.0 X 10 -8 1.0 X 10 -6 6 2 12 1.0 X 10 -2

  8. Naming Acids • Binary acids • Contains 2 different elements: H and another • Always has “hydro-” prefix • Root of other element’s name • Ending “-ic” • Examples: HI, H2S, HBr

  9. Naming Acids • Ternary Acids - Oxyacids • Contains 3 different elements: H, O, and another • No prefix • Name of polyatomic ion • Ending “–ic” for “-ate” and “–ous” for “-ite” • Examples: HClO4, H3PO4, HNO2

  10. H2SO3 Sulfurous acid HF Hydrofluoric acid H2Se Hydroselenic acid Perchloric acid HClO4 Carbonic acid H2CO3 Hydrobromic acid HBr Practice

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