Concept explainers
(a)
Interpretation:
The dissociation constant of an acid that has
Concept introduction:
Dissociation constant
The formula used to calculate the value of
(b)
Interpretation:
The dissociation constant of an acid that has
Concept introduction:
Dissociation constant
The formula used to calculate the value of
(c)
Interpretation:
The dissociation constant of an acid that has
Concept introduction:
Dissociation constant
The formula used to calculate the value of
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Organic Chemistry
- Acid-Base Equilibria Many factors contribute to the acidity of organic compounds. Electronegativity, resonance, induction, hybridization, aromaticity, and atomic size, all play a role. In the following comparisons, you are asked to identify the factor(s) that would be most important to analyze when predicting relative acidity, and then to predict the trend in acidity and pKa values. For each of the following pairs of compounds answer the following two multiple-choice questions. 1. What factor(s) are the most important to consider when predicting the relative acidity of the two compounds? a. Electronegativity of the atom possessing the hydrogen. b. Resonance stabilization of the anionic conjugate base. c. Inductive stabilization of the anionic conjugate base. d. Hybridization of the atom possessing the hydrogen. e. The atomic size of the atom possessing the hydrogen.arrow_forwardIf the G for a reaction is 4.5 kcal/mol at 298 K, what is the Keq for this reaction? What is the change in entropy of this reaction if H = 3.2 kcal/mol?arrow_forwardConsider these acids (a) Arrange the acids in order of increasing acid strength from weakest to strongest. (b) Which acid has the smallest pKa value?arrow_forward
- Will acetylene react with sodium hydride according to the following equation to form a salt and hydrogen, H2? Using pKa values given in Table 4.1, calculate Keq for this equilibrium.arrow_forwardDefine or illustrate the meaning of the following terms: a. Ka reaction b. Ka equilibrium constant c. Kb reaction d. Kb equilibrium constant e. conjugate acidbase pairarrow_forwardIdentify the acid and conjugate base in each reaction. Calculate the pKA for each acid. List them in order from the strongest to weakest acid. The acid-ionization constants, KA, at 25°C are provided for each. C6H5OH + H2O Û H3O+ + C6H5O-, KA = 1.2589254 x 10-10 CH3CO2H + H2O Û H3O+ CH3CO2-, KA = 1.5848 x 10-5 CF6CO2H+H2O Û H3O+ + CF6CO2-, KA = 0.6309arrow_forward
- Write the acid dissociation constant expression (Ka ) for the dissociation of HCN.arrow_forwardWhich of the following is true about acids and bases? A. When bases ionize, they donate protons. B. Strong acids and bases are completely ionized in dilute aqueous solutions. C. The dissociation constant of a strong acid is lower than that for a weak acid. D. The pKa of a strong acid will be higher than that for a weak acid.arrow_forwardExplain why-(i) Anhydrous calcium chloride is used in desiccators(ii) If bottle full of concentrated H 2SO4 is left open in the atmosphere by accident, the acid starts flowing out the bottle of its own.arrow_forward
- The acids are: isopropanol, ethyne, and phenol. Which acid will NOT be deprotanated by NaOH and which acid will deprotonate in the presence of NaHCO3. After an acid base reaction, which compound above has the weakest conjugate base?arrow_forwardthe dissociation constant of 0.25 M propanoic acid C2H5COOH is 1.3 × 10-⁵. a) What is the dissociation rate of C2H5COOH in this solution?arrow_forwardPart 1. Choose the stronger acid in each pair of compounds. Part 2. Arrange the following compounds in order of increasing basicity. Part 3. Determine if the oxide is acidic or basearrow_forward
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