SOLUTION:
The problem can be solved by Henderson-Hasselbalch equation as:
CH3COOH <--------> CH3COO- + H+
pH = pKa + log [CH3COO-] / [CH3COOH]
pKa = -logKa = - log 1.76 X 10-5 = 4.75; pH = 3.570
3.57 = 4.75 + log[CH3COO-] / [CH3COOH]
log[CH3COO-] / [CH3COOH] = 3.57 - 4.75 = - 1.18
[CH3COO-] / [CH3COOH] = antilog(-1.18) = 0.066
Hence the ratio of acetate to acetic acid is 0.066
What is the ratio of acetate ion to acetic add (K_ a = 1.76 times 10^-5)...
What is the ratio of acetate ion to acetic acid (K_a = 1.76 times 10^-5) in a buffer containing these compounds at pH 3.920?
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What is the ratio of acetate ion to acetic acid (Ka = 1.76 x 10-5) in a buffer containing these compounds at pH 4.07
What is the ratio of acetate ion to acetic acid (Ka = 1.76×10–5) in a solution containing these compounds at pH 3.17? Write your answer as a decimal and not as a fraction.
What is the ratio of acetate ion to acetic acid (Ka = 1.76×10–5) in a solution containing these compounds at pH 4.25 ? Write your answer as a decimal and not as a fraction.
What is the ratio of the concentrations of acetate ion and undissociated acetic acid at pH 4.10? (The pKa of acetic acid is 4.76.)
A) A buffer containing acetic acid and sodium acetate has a pH of 5.45. The Ka value for CH3CO2H is 1.80 × 10-5. What is the ratio of the concentration of CH3CO2H to CH3CO2-? [CH3CO2H]/[ CH3CO2-] = _________ B) What is the pH change when 29.6 mL of 0.117 M NaOH is added to 95.4 mL of a buffer solution consisting of 0.123 M NH3 and 0.179 M NH4Cl (Ka for ammonium ion is 5.6x10^-10.) pH change =_______
Bonus) What concentration of acetate ion in 0.500 M acetic acid produces a buffer solution with pH = 5.00? K, for acetic acid = 1.80x10-5
Acetic acid has a Ka of 1.8*10^-5. Three acetic acid/ acetate buffer solutions, A,B, and C, wer made using varying concentrations: 1. [acetic acid] ten times greater than [acetate] 2. [acetate] ten times greater than [acetic acid] 3. [acetate] = [acetic acid] Match each buffer to the expected pH pH = 3.74 pH= 4.74 pH = 5.74
Part A Acetic acid has a Ka of 1.8×10−5. Three acetic acid/acetate buffer solutions, A, B, and C, were made using varying concentrations: [acetic acid] ten times greater than [acetate], [acetate] ten times greater than [acetic acid], and [acetate]=[acetic acid]. Match each buffer to the expected pH. Drag each item to the appropriate bin. Part B How many grams of dry NH4Cl need to be added to 2.40 L of a 0.100 M solution of ammonia, NH3, to prepare a...