Weak Acids, Weak Bases, and Their Salts Report Name Section B. Effecet of Concen
ID: 942668 • Letter: W
Question
Weak Acids, Weak Bases, and Their Salts Report Name Section B. Effecet of Concentration on Degree of lonization Record the pH, [H,0% and [OH-] of each solution that you investigated. 1.0 M 0.10 M 0.010 M HCI pH .2 OH-1 HC,H,0, pH 342423.23 12 ATx 0 x Ib-12 OH-] NH3(aq) pH Amm OH 5020524x10 20401 Using your data, calculate the value of Ka or Kp and the degree of ionization, c, for each of the solutions you investigated 1.0 M 0.10 M 0.010 M e 2 132 525 7 92 004 024 4 132 .525 .477 022 xo CHA) 00503 60524 00 Sample CalculationsExplanation / Answer
Table 1
For HCl 1.0 M 0.1 M 0.01 M
pH 0 1 2
[H3O+] 1.0 M 0.1 M 0.01 M
[OH-] 1x10^-14 1x10^-13 1x10^-12
For HC2H3O2
pH 2.4 2.9 3.4
[H3O+] 4.2x10^-3 1.3x10^-3 4.2x10^-4
[OH-] 2.3x10^-12 7.4x10^-12 2.3x10^-11
NH3(aq)
pH 11.6 11.13 10.6
[H3O+] 2.3x10^-12 7.4x10^-12 2.3x10^-11
[OH-] 4.2x10^-3 1.3x10^-3 4.2x10^-4
Table 2
For HCl
Ka 1x10^-14 1x10^-14 1x10^-14
alpha 100 100 100
For HC2H3O2
Ka 9.6x10^-15
alpha 0.42
For NH3
Kb 9.66x10^-15
alpha 0.42
So doing the calculation in the same manner for the rest, we can say that Ka value increases as the concentration goes down. Similarly alpha which is dissociation increases as the concentration decreases for both acid or base in solution.
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