<p>Exam 2 Material</p><p>1. Write the conjugate acids for the following:</p><p>- 2- H2O OH CO3 NH3</p><p>2. Write the conjugate bases for the following:</p><p>- - H2O OH H2SO4 NH2</p><p>3. Calculate the pH of a 0.015 M acetic acid solution. -5 The Ka value is 1.8x10 + - CH3COOH  H + CH3COO</p><p>4. Calculate [H+] for a solution with a pOH of 4.75</p><p>5. List the 7 strong acids:</p><p>6. Rank in order of increasing base strength: ClO- BrO- IO-</p><p>7. Calculate the pH of the following solutions a. 1.20 M HCl b. .003 M HNO3 c. .020 M NaOH d. .001 M Ba(OH)2</p><p>8. Calculate the pH of a 0.15 M formic acid (HCOOH) solution that also contains -4 0.05 M sodium formate (HCOONa). Ka= 1.8x10 for formic acid.</p><p>9. What is the pH of a solution containing 25 grams HCl dissolved in 1.5 L water?</p><p>10. Predict whether aqueous solutions of the following compounds are acidic basic or neutral. </p><p> a. NH4Br b. FeCl3</p><p> c. Na2CO3</p><p> d. KClO4</p><p> e. NaHC2O4</p><p>11. Rank these acids from strongest to weakest HF HCl HBr HI</p><p>12. Which is a stronger acid? Explain your reasoning.</p><p> a. HNO3 HNO2</p><p> b. H2S H2O</p><p>- c. H2SO4 HSO4</p><p> d. H2SO4 H2SeO4</p><p> e. CCl3COOH CH3COOH</p><p>13. Identify the Lewis acid and Lewis base among the reactants in each reaction 3+ - a. Fe(ClO4)3 (s) + 6H2O (l) Fe(H2O)6 (aq) + 3ClO4 (aq)</p><p>- - b. CN (aq) + H2O (l) HCN (aq) + OH (aq)</p><p> c. (CH3)3N (g) + BF3 (g) (CH3)3NBF (s)</p><p>- - d. HIO + NH2 NH3 + IO</p><p>14. What is the pH of a 0.10 M solution CH3CO2H if 0.05 M NaCH3CO2 is added? -5 Ka= 1.8x10</p><p>15. Classify the following solutions as acids, basic, or neutral a. KCl b. NH4NO3</p><p> c. Na2CO3 d. RbF 16. 34.6 g of NH4Cl is added to 3.98 L of 0.0145 M solution of NH3. Kb (NH3)= 1.8*10-5 a. What is the pH of the original solution before the addition of NH4Cl?</p><p> b. Calculate the pH of the solution after the NH4Cl is added. Assume volume remains constant. </p><p>17. A buffer contains .1 mol of acetic acid and .13 mol of sodium acetate in 1 L. a. What is the pH of the buffer? b. What is the pH of the buffer after .02 mol of KOH is added? c. What is the pH of the buffer after the addition of .02 mol HNO3?</p><p>18. Find the pH at the following points in the titration of 30 mL of 0.05 M HClO4 with 0.1 M KOH. a. Before adding any KOH b. When 5 mL of .1 M KOH is added c. When 15 mL of .1 M KOH is added</p><p>19. For the titration of a weak acid with a strong base, the equivalence point it at/above/below a pH of 7. (circle one)</p><p>20. For the titration of a strong acid with a strong base, the equivalence point it at/above/below a pH of 7. (circle one)</p><p>21. Calculate the pH in the titration of 50.00 mL of .2 M ammonia by .2 M -5 hydrochloric acid. Kb for ammonia is 1.8x10 : a. At the start of the titration b. After 20 mL of HCl has been added c. At the equivalence point</p>