CHM 1301 Lecture Notes - Lecture 16: Acetic Acid, Sodium Acetate, Buffer Solution

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13 Dec 2016

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CHM 1301 Full Course Notes

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The function of a buffer can be summarized as follows: A buffer can protect the ph of a solution by reacting with both strong acids and strong bases, preventing large changes in [oh-] and [h3o+ ] Contains both a weak acid and its conjugate base, or a weak base and its conjugate acid, as the major species in solution. They are solutions that are resistant to changes in ph upon addition of strong acid or base: Ch3co2h (aq) + h2o (l) ch3co2- (l) + h3o+(aq) Ch3co- (aq) + h2o (l) ch3co2h (l) + oh- (aq) 2 h2o (l) h3o+ (aq) + oh- (aq) Calculate the concentration of hydronium ions, acetate ions and acetic acid if you at. 0. 125 m solid sodium acetate in a 1. 00 l solution of 0. 250 m acetic acid. 1. 8x10 -5 = (x 2 + 0. 125x) / (0. 250-x) Assume that x <<< 0. 250 m & x <<<< 0. 125 m.

Related Questions

For conjugate acid-base pairs, how are Ka and Kb related?

Consider the reaction of acetic acid in water:

CH₃CO₂H (aq) + H₂O (l) ⇌ CH₃CO₂⁻ (aq) + H₃O⁺ (aq) where Ka = 1.8 × 10⁻⁵

Which two bases are competing for the proton?
Which is the stronger base?
In light of your answer to part b. why do we classify the acetate ion (CH₃CO₂⁻) as a weak base? Use an appropriate reaction to justify your answer.
In general, as base strength increases, conjugate acid strength decreases. Explain why the conjugate acid of the weak base NH₃ is a weak acid.

To summarize, the conjugate base of a weak acid is a weak base and the conjugate acid of a weak base is a weak acid (weak gives you weak). Assuming Ka for a monoprotic strong acid is 1× 10⁶, calculate Kb for the conjugate base of this strong acid.

Why do conjugate bases of strong acids have no basic properties in the water?

List the conjugate bases of the six common strong acids.

To tie it all together, some instructors have students think of Li⁺, K⁺, Rb⁺, Cs⁺, Ca²⁺, Sr²⁺, and Ba²⁺ as the conjugate acids of the strong bases LiOH, KOH, RbOH, CsOH, Ca(OH)₂, Sr(OH)₂, and Ba(OH)₂. Although not technically correct, the conjugate acid strength of these cations is similar to the conjugate base strength of the strong acids. That is, these cations have no acidic properties in water; similarly, the conjugate bases of strong acids have no basic properties (strong gives you worthless). Fill in the blanks with the correct response. The conjugate base of a weak acid is a_____base. The conjugate acid of a weak base is a_____acid. The conjugate base of a strong acid is a_____base. The conjugate acid of a strong base is a_____ acid. ( Hint: Weak gives you weak and strong gives you worthless.)

periwinklegoat463

For conjugate acid-base pairs, how are K_a and K_b related?

Consider the reaction of acetic acid in water

CH₃CO₂H (aq) H₂O (l) CH₃CO₂^- (aq) H₃O⁺ (aq)

where K_a 1.8 10^-5

(a) Which two bases are competing for the proton?

(b) Which is the stronger base?

(c) In light of your answer to part (b) why do we classify the acetate ion (CH₃CO₂^-) as a weak base? Use an appropriate reaction to justify your answer.

greenalligator494

CHM 1301 Lecture Notes - Lecture 16: Acetic Acid, Sodium Acetate, Buffer Solution

CHM 1301 Full Course Notes

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