<p>Chemistry Acids and Bases 1</p><p>1. For each tell whether it is a property of acids, bases, or both. A. feels slippery B. tastes sour C. tastes bitter D. electrolyte E. turns litmus red F. turns litmus blue, G. turns phenolphthalein clear H. turns phenolphthalein pink I. conducts electricity when dissolved in water J. pH increaser K. pH reducer</p><p>2. Classify each as acid or base. A. proton donor B. proton acceptor C. produces OH- D. produces H+ E. electron pair donor F. electron pair acceptor</p><p>3. Classify each as a strong or weak acid or base. A. HCl B. HNO2 C. NaOH D. Mg(OH)2</p><p>4. Write chemical equations to show how each acid or base dissociates in water solution. A. HCl B. H2SO4 C. H3PO4 D. HBr E. NaOH F. Ca(OH)2 G. NH4OH H. NH3 I. H2O J. HClO3 K. HF L. H2SO3 M. CH3COOH</p><p>- + 5. For each tell whether the solution is acidic or basic and find: [OH ], [H+], [H3O ], pH and pOH. A. pH 7 B. pH 2 C. pH 13 D. pOH 12 E. pOH 4</p><p>6. A solution has a hydrogen ion concentration of 1 x 10-6M. What is its pH?</p><p>7. What is the pH of solution if the [H+] = 7.2 x 10-9M?</p><p>8. What is the pOH of a solution if the [OH-] = 3.5 x 10-2M?</p><p>9. What is the pOH of a solution that has a pH of 3.4?</p><p>10. Classify each solution as acidic, basic, or neutral. a. [H+] = 2.5 x 10-9M d. [H+] = 1 x 10-7M b. pOH = 12.0 e. pH = 0.8 c. [OH-] = 9.8 x 10-11M</p><p>11. Calculate the pH of each solution and determine if it’s acidic or basic. a. [H+] = 1 x 10-5M c. [OH-] = 2.2 x 10-7M</p><p> b. [H+] = 4.4 x 10-11M d. pOH = 1.4</p><p>12. Why is there a minus sign in the definition of pH?</p><p>13. A solution has a pOH of 12.4. What is the pH of this solution?</p><p>14. What is the pH of a solution with [H+] = 2 x 10-3M?</p>