Unit+11-+Acids+&+Bases



Acids I. ex. vinegar, asprin, lemon juice II. Tends to burn things III. pH A. Acids 0-7 1. 0 is a strong acid 2. 7 is a weak acid B. Bases 7-14 1. 14 is a strong base 2. 7 is a weak base C. 7 is neutral, neither base nor acid 1. Kw a. When you have strong acids (1) Concentration of H3O+ b. When you have strong bases (1) X is the concentration of OH- or (1 x 10^ -14 D. Calculate pH of Acids 1. pH= -log (H+) E. Calculate pOH of Bases 1. pOH= -log (OH-) IV. Definitions A. Arrhenius 1. Produce H+ ion or H3O+ ion B. Brosted-Lowry 1. proton donor C. Lewis 1. Substance that accepts an electron pair V. Calculating Equilibria A. Use ICE Tables 1. I is the initial molarity of the substance 2. C is the change, which is - x in an acid and + x in a base. The change also has molarity 3. E is the Equilibria, which is molarity minus x in an acid, and molarity plus x in a base 4. Put into an equation to find what x equals, may require the quadratic formula 5. Find what the pH is, and also pOH 6. Ka is the equation of the acid and Kb is the equation of the base VI. Titrations A. How to Find Titrations 1. Write out the equations 2. Find the volume or concentration 3. May have to use stoichiometry Bases I. ex. Laundry Detergent, Drain Ckeaner II. Hurts skin and eyes III. Definitions A. Arrhenius 1. Produce OH- ions B. Bronsted- Lowry 1. proton acceptor C. Lewis 1. Subtance that donates an electron pair IV. Calculating Equilibria V. Titrations

1) What is the pH of a 0.20 M HCl solution? A. < 0 B. 0.70 C. 1.61 D. 12.39 E. 13.30 2) What is the [OH-] for a solution at 25°C that has [H3O+] = 2.35 × 10-3 M? A. 4.26 × 10-5 M B. 2.35 × 10-11 M C. 4.26 × 10-12 M D. 2.35 × 10-17 M E. none of these choices is correct 3) What is the [OH-] for a solution at 25°C that has pH = 4.29? A. 1.4 × 10-2 M B. 5.l × 10-5 M C. 1.9 × 10-10 M D. 7.3 × 10-13 M E. 9.71 M 4) What is the [H3O+] for a solution at 25°C that has pOH = 5.640? A. 2.34 × 10-4 M B. 2.29 × 10-6 M C. 4.37 × 10-9 M D. 4.27 × 10-11 M E. 8.360 M 5) Select the pair of substances in which an acid is listed followed by its conjugate base. A. H+, HCl B. NH3, NH4+ C. HPO42-, H2PO4- D. HCO3-, CO32- E. CH3COOH, CH3COOH2+ 6) Select the pair of substances which is not a conjugate acid-base pair. A. H3O+, H2O B. HNO2, NO2- C. H2SO4, HSO4- D. H2S, S2- E. NH3, NH2- 7) According to Brønsted and Lowry, which one of the following is not a conjugate acid-base pair? A. H3O+/OH- B. CH3OH2+/CH3OH C. HI/I- D. HSO4-/SO42- E. H2/H- 8) A 0.050 M solution of the weak acid HA has [H3O+] = 3.77 × 10-4 M. What is the Ka for the acid? A. 7.5 × 10-3 M B. 2.8 × 10-6 M C. 7.0 × 10-7 M D. 7.0 × 10-8 M E. 2.6 × 10-11 M

1)B 2)C 3C 4)C 5)D 6)D 7)A 8)B