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
- Calculate the Ka's for the following acids: (a) Citric acid, pKa = 3.14 (b) Tartaric acid, pKa = 2.98arrow_forwardDicarboxylic acids have two dissociation constants, one for the initial dissociation into a monoanion and one for the second dissociation into a dianion. For oxalic acid, HO2C—CO2H, the first ionization constant is pKal = 1.2 and the second ionization constant is pKa2 = 4.2. Why is the second carboxyl group far less acidic than the first?arrow_forwardWhich of the following acid/conjugate base pairs has a pKa value of 9.44? A. Ammonium/ammonia B. carboxylic acid/carboxylate C. imidazolium/imidazolearrow_forward
- Do the equilibria of the following acid–base reactions lie to the right or the left? (The pKa of H2O2 is 11.6.)arrow_forward(b) What is Ka of the 2-hydroxyethylammonium ion, HOCH2CH2NH3+ (pKb of HOCH2CH2CH2NH2 = 4.49)?arrow_forward6)Rank the following compounds in order of increasing pKa values, and explain your choices in detail.arrow_forward
- Aniline (conjugate acid pKa 4.63) is a considerably stronger base than diphenylamine (pKa 0.79). Account for these marked differences.arrow_forwardWhat is the K a of an acid whose pK a is 8.60?arrow_forwardGiven the normal blood pH is 7.35, what is the expected pKa of H2CO3 ([H2CO3] = 0.50M and [HCO3-] = 0.100M) ?arrow_forward
- At what pH will 25% of a compound with a pKa of 5.3 be in its basic form?arrow_forwardThe Kb for dimethylamine, CH3NH2, at 25oC is 4.0×10-4. What’s the Ka of its conjugate acid?arrow_forwardCalculate the ratio of ethyl amine (CH3CH2NH2) to the ethyl ammonium ion (CH3CH2NH3+) in a solution with a pH of 11.0. pKa for CH3CH2NH3+ = 10.636.arrow_forward
- Organic ChemistryChemistryISBN:9781305580350Author:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. FootePublisher:Cengage Learning