Question

Can anyone please help with how to calculate degree of ionization for the first 3 solutions as well as how to calculate the expected pH for solution 4? thank you!

Experiment 8: Equilibria of Weak Acids and Bases Lab Report Sheet 1 Composition 20.0 mL of 0.1 M HC2H302 - (A weak acid) pH 12.76 2.42 2.59 10.0 mL of 0.10 M HC2H3O2 + 10.0 mL H20 - (effect of dilution on the degree of ionization of weak acid) 10.0 mL of 0.10 M HC2H,02 + 90.0 mL of H2O -- (effect of dilution on the degree of ionization of weak acid) 10.0 mL of 0.10 M HC2H2O2 + 10.0 mL of 0.10HCI -- (common ion effect on the pH and ionization of weak acid) 50.0 mL of 0.10 M HC2H2O2 +50.0 mL of 0.10 M NaC2H2O2 - (An acid buffer) 11.74 57 16.03 7 10 10.0 mL of solution 5 + 6 mL of H2O-- (effect of adding water on the pH of the buffer) 10.0 mL of solution 5 + 1 mL of 0.10 M NaOH (effect of adding small amount of base on the pH of the buffer) 10.0 mL of solution 5 + 6 mL of 0.10 M NaOH -- (effect of adding large amount of base on the pH on the buffer-Buffer capacity) 20mL of 0.10 NH3 (A weak base) 8 [11.65 113.26 11.12 97 10 20.0 mL of 0.10 M NH.NO, (A salt of weak base and strong acid) 5.60 11 50.0 mL of 0.10 M NH3 + 50.0 mL of 0.10 M NH.NO3 solution (A Base buffer) lau2 12 9.36 10 mL of solution 11 + 6 mL H20- (Effect of adding water on the pH of the base buffer) 13 10 mL of solution 11 + 1 mL of 0.10 M HCI- (effect of adding small amount of acid on the pH of the base buffer - Buffer capacity) 14. 10 mL of solution 11 + 6 mL of 0.10 M HCI- (effect of adding large amounts of acid on the pH of the buffer - Buffer capacity) 2.35

Answer 1

0.01 01042 (V.) 10.0ml of o.10M HOC hq + 10.0ml of 0.1 M HCL > This is a mixture of weak Acid and strong Acid so ph will be only decided by Strong Acid. 1407= 10x0.1 = 0.05 ph = -log[nt ] -2 -1 og 5 = 1.3 REDMI NOTE 5 PRO MI DUAL CAMERA