The pH of the equivalence points is 8.54
Concept of pH
A solution's acidity or alkalinity can be determined based on the concentration of hydrogen ions in the solution, or pH. Acidic aqueous solutions at 25 °C have a pH under 7, while basic or alkaline aqueous solutions have a pH above 7. Since the concentration of H3O+ is equal to the concentration of OH in pure water, a pH level of 7.0 at 25°C is referred to as "neutral". Strong bases may have a pH above 14, while very strong acids may have a pH below 14.
0.0520 M CH3COOH in 42.2 mL of moles is as follows:
2.194x103 mol CH3COOH = 0.0422L (0.0520mol / L)
that react with NaOH, resulting in:
NaOH + CH3COOH = CH3COO + Na+ + H2O
Thus, 1 mole of acetic acid and 1 mole of NaOH react.
As a result, 2.194x103 mol of NaOH are required to reach the equivalence point in volume:
To attain the equivalency point, 2.194x103 mol (1L / 0.0372mol) = 0.05899L 58.99mL of 0.0372 M NaOH
You will only have CH3COO at the equivalency point because it is in equilibrium with water, so:
H2O(l) + CH3COO(aq) CH3COOH(aq) + OH (aq)
A definition of equilibrium is:
Kb = 5.6x1010 = [OH] / [CH3COO] / [CH3COOH]
2.194x103mol of CH3COO has a molarity of (0.05899L + 0.0422L) = 0.02168M.
Therefore, equilibrium concentrations are:
[CH3COO]=0.02168M-X [CH3COOH]=X [OH]=X
5.6x1010 = [X] [X] / [0.02168M - X] converts to Kb.
1.214x1011 - 5.6x1010X = X2 X2 + 5.6x1010X - 1.214x1011 = 0 Finding the value of X:
False response; there are no negative concentrations. X: -3.48x106
As [OH] = X, [OH] = 3.484x106M, X is 3.484x106.
As 14 = pOH + pH pH = 8.54, pOH = -log [OH], or 5.46.
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