QUESTION 6 A titration of 45.0 ml of 0.17M HNO3 with a 0.25M LIOH solution. What is the pH of the solution after 27.0 mL of LIOH are added? Write answer in decimal form to two decimal places. K = 1.0x1034 pH = pKa+ log[A]/[HA] pH = -log[H,O"] 14 = pH + pOH

Question 6 of 6 Points possible: 1.00 Not yet answered Consider the generic weak acid HA, for which Ka = 1.2 x 10. Which of the following mixtures would result in a buffer solution when 30.0 mL of each of the two solutions are mixed? Select one: 0.10 M NaOH and 0.10 M HA 0.20 M NaOH and 0.10 M HA 0.10 M NaOH and 0.20 M HA 0.01 M NaOH and 0.20 M HA None of the above are correct

When 30 .00 mL of 0.1011 M HCl in 50 mL of deionized water is titrated against 0.09889 M NaOH, the pH increases. What is the volume (in mL) of NaOH required to reach the equivalence point and a pH of 7.00? Find the pH when the volume of NaOH added is 0.02 mL less than the volume required to reach the equivalence point. Find the pH when the volume of NaOH added is 0.01 mL less than the volume required to reach the equivalence point. Find the pH when the volume of NaOH added is 0.02 mL more than the volume required to reach the equivalence point. Comment on the significance of the changes in pH values in relation to the increments of sodium hydroxide added when going “through” the end point. Define equivalence point. For a weak base/strong acid titration, is the pH at the equivalence point <, >, or equal to 7?

QUESTION 11 Which of the following acid/base conjugate pairs could you use to make a buffer solution with a pH of 12.55? The K, for the acids are given in parentheses. O Chlorous acid/ chlorite (K, = 1.1 x 10-2) O Ammonium / ammonia (K, = 5.8 x 10-10) O Benzoic acid / benzoate (K, = 6.3 x 10-5) O Hydrofluoric acid / fluoride (Kg = 6.6 x 10-4) O Hydrogen phosphate /phosphate (K, = 4.2 x 10-13)