Concept explainers
Interpretation:
The correct
Concept introduction:
pKa: It is introduced as an index to express the acidity of weak acids, where
In aqueous solution an acid undergoes ionization. The ionization of an acid is can be expressed in terms of equilibrium constant. The quantitative measurement tells about the strength of the acid. Higher the value of
The dissociation constant for the acid is
For simplifications
The lower value of
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Chemistry & Chemical Reactivity
- (a) Given that Ka for acetic acid is 1.8 x 10-5 and that forhypochlorous acid is 3.0 x 10-8, which is the stronger acid?(b) Which is the stronger base, the acetate ion or the hypochloriteion? (c) Calculate Kb values for CH3COO- and ClO-.arrow_forward(b) Calculate the pH of 0.0005 mol dm-3 ethanois acid when its pKa = 4.75 CH;COOH() -> CH;COO (a H(a + Ka = pH =arrow_forwardWhat is the pOH of:(a) a 0.0100 F solution of phtalic acid?(b) a 0.0100 F solution of monopotassium phtalate? (c) a 0.0100 F solution of dipotassium phtalate?if pKa1 = 2.950 and pKa2 = 5.408 for phtalic acidarrow_forward
- The base B has pKb 5.00. (a) What is the value of pKa for the acid BH? (b) At what pH is [BH] [B]? (c) Which is the principal species, B or BH, at pH 7.00? (d) What is the quotient [B]/[BH] at pH 12.00?arrow_forwardIf the pH value of an aqueous solution of trimethylamine [(CH3)3N] is 10.75, what should the molarity of this solution be? (CH3)3N + H2O ↔ (CH3)3NH+ + OH-, Kb = 6,3 × 10-5arrow_forwardFor an acid with a pKa of 5.00, what is the pKb of its conjugate base?arrow_forward
- Ammonia (NH3) is a weak base that under acidic conditions becomes protonated to the ammonium ion in thefollowing reaction:NH3 + H+ → NH4 +NH3 freely permeates biological membranes, including thoseof lysosomes. The lysosome is a subcellular organelle witha pH of about 4.5–5.0; the pH of cytoplasm is about 7.0.What is the effect on the pH of the fluid content of lysosomes when cells are exposed to ammonia? Note: Ammonium (NH4 +) does not diffuse freely across membranes.arrow_forwardThe acid HA has pKa 7.00. (a) Which is the principal species, HA or A, at pH 6.00? (b) Which is the principal species at pH 8.00? (c) What is the quotient [A]/[HA] at (i) pH 7.00; (ii) at pH 6.00?arrow_forwardA weak acid has a pKa of 7.6. What is the proportion of A- to HA if pH is 9.08? Round to one decimal place. Thank You!arrow_forward
- Choose the stronger acid in each of the following pairs:(a) H₂Se or H₃As (b) B(OH)₃ or Al(OH)₃(c) HBrO₂ or HBrOarrow_forward3. Which is the stronger acid: (a) Benzoic acid with a Ka of 6.5 x10-5 or hydrocyanic acid with a Ka of 4.9 x 10-10? (b) Boric acid with a pKa of 9.14 or carbonic acid with a pKa of 6.37arrow_forward5) Identify which of the following reactions are unfavorable and explain why: A) :o: B) C) + cig CHzö. D)arrow_forward
- Organic ChemistryChemistryISBN:9781305580350Author:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. FootePublisher:Cengage Learning