Organic Chemistry
8th Edition
ISBN: 9781305580350
Author: William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. Foote
Publisher: Cengage Learning
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Question
Chapter 4, Problem 4.25P
(a)
Interpretation Introduction
Interpretation:
The possibility of evolution of carbon dioxide when sodium bicarbonate reacts with sulfuric acid has to be explained.
(b)
Interpretation Introduction
Interpretation:
The possibility of evolution of carbon dioxide when sodium bicarbonate reacts with ethanol has to be explained.
(c)
Interpretation Introduction
Interpretation:
The possibility of evolution of carbon dioxide when sodium bicarbonate reacts with ammonium chloride has to be explained.
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(a) Wr ite an equat ion for the react ion in whichH2C6H7O5-(aq) acts as a base in H2O(l). (b) Write an equationfor the reaction in which H2C6H7O5-(aq) acts as an acidin H2O(l). (c) What is the conjugate acid of H2C6H7O5-(aq)?What is its conjugate base?
Number 16.20
(a) Write a balanced equation representing the reaction of the acid, H2PO4- with the base, water.
(b) Write the expression for Ka of H2PO4- in terms of concentrations of relevant species.
Chapter 4 Solutions
Organic Chemistry
Ch. 4.2 - For each conjugate acid-base pair, identify the...Ch. 4.2 - Write these reactions as proton-transfer...Ch. 4.2 - Following is a structural formula for guanidine,...Ch. 4.2 - Write an equation to show the proton transfer...Ch. 4.3 - For each value of Ka, calculate the corresponding...Ch. 4.4 - Predict the position of equilibrium and calculate...Ch. 4.5 - Calculate Keq for a reaction with G0 = 17.1 kJ/mol...Ch. 4.6 - Acid-Base Equilibria Many factors contribute to...Ch. 4.6 - What is the relative trend in acidity and pKa of...Ch. 4.7 - Write an equation for the reaction between each...
Ch. 4 - For each conjugate acid-base pair, identify the...Ch. 4 - Complete a net ionic equation for each...Ch. 4 - Arrange the compounds in each set in order of...Ch. 4 - Prob. 4.12PCh. 4 - In acetic acid, CH3COOH, the OH hydrogen is more...Ch. 4 - Which has the larger numerical value? (a) The pKa...Ch. 4 - In each pair, select the stronger acid. (a)...Ch. 4 - Arrange the compounds in each set in order of...Ch. 4 - Arrange the compounds in each set in order of...Ch. 4 - If the G for a reaction is 4.5 kcal/mol at 298 K,...Ch. 4 - Calculate the Keq for the following reactions from...Ch. 4 - Prob. 4.20PCh. 4 - Answer true or false to the following statements...Ch. 4 - In each of the following three reaction coordinate...Ch. 4 - The acid-base chemistry reaction of barium...Ch. 4 - Unless under pressure, carbonic acid (H2CO3) in...Ch. 4 - Prob. 4.25PCh. 4 - Acetic acid, CH3COOH, is a weak organic acid, pKa...Ch. 4 - Benzoic acid, C6H5COOH (pKa 4.19), is only...Ch. 4 - Prob. 4.28PCh. 4 - One way to determine the predominant species at...Ch. 4 - Will acetylene react with sodium hydride according...Ch. 4 - Prob. 4.31PCh. 4 - For each equation, label the Lewis acid and the...Ch. 4 - Complete the equation for the reaction between...Ch. 4 - Each of these reactions can be written as a Lewis...Ch. 4 - The sec-butyl cation can react as both a...Ch. 4 - Prob. 4.36APCh. 4 - Prob. 4.37APCh. 4 - Prob. 4.38APCh. 4 - Explain why the hydronium ion, H3O+, is the...Ch. 4 - What is the strongest base that can exist in...Ch. 4 - Prob. 4.42APCh. 4 - Prob. 4.43APCh. 4 - Methyl isocyanate, CH3N=C=O, is used in the...Ch. 4 - Offer an explanation for the following...Ch. 4 - Prob. 4.46APCh. 4 - Alcohols (Chapter 10) are weak organic acids, pKa...Ch. 4 - As we shall see in Chapter 19, hydrogens on a...Ch. 4 - 2,4-Pentanedione is a considerably stronger acid...Ch. 4 - Write an equation for the acid-base reaction...Ch. 4 - Prob. 4.51APCh. 4 - Prob. 4.52APCh. 4 - Prob. 4.53APCh. 4 - Following is a structural formula for imidazole, a...
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- (A) Which of the following is the strongest base? NH (B) (C) (D)arrow_forwardC6H5NH2 + H2O <-> C6H5NH3+ + OH-. Aniline, a weak base, reacts with water according to the reaction. (a) a sample of aniline is dissolved in water to produce 25.0 mL of 0.10 m solution. The pH of the solution 8.82. Calculate the equilibrium constant, Kb, for this reaction (b) What is the percent disassociation for the solution in part (a) (c) 25.0 mL of 0.10 HCI was then added in a titration experiment. What is the pH at the equivalence point?arrow_forwardProvide a reason of using ammonnum hydroxide and ammonium chloride in precipitation of Group IV cations. SWERarrow_forward
- Consider two acids: HCO,H (formic acid, pKa = 3.8) and pivalic acid [(CH3)3CCO2H, pKa = 5.0]. (a) Which acid has the larger K,? (b) Which acid is the stronger acid? (c) Which acid forms the stronger conjugate base? (d) When each acid is dissolved in water, for which acid does the equilibrium lie further to the right?arrow_forwarda net ionic equation to show that morphine, C17H19O3N, behaves as a Bronsted-Lowry base in water.arrow_forward(ii) Ph. - COOHarrow_forward
- In each of the following cases, is the concentration of acid before and after dissociation nearly the same or very different?Explain your reasoning: (a) a concentrated solution of a strong acid; (b) a concentrated solution of a weak acid; (c) a dilute solu-tion of a weak acid; (d) a dilute solution of a strong acid.arrow_forwardHydrochloric acid in the stomach is a very strong acid compared to ethanoic acid that is found in citrus fruits. Explain (with reference to formation of hydronium ions) why hydrochloric acid has a much lower pH compared to ethanoic acid. You should support this answer with accompanying ionic equations.arrow_forward2.3 7 (a) Describe what happens when each of the following molecules is separately dissolved in water and illustrate with an equation in each case: (i) ethanoic acid (CH3COOH) (ii) ammonia (NH3) (b) Identify the conjugate acids and bases in the substances mentioned in question 7(a) above. (c) Explain the difference between: (i) a strong acid and weak acid and (ii) a strong base and a weak basearrow_forward
- Phosphorous acid (H3PO3) has the Lewis structure shown at right.(a) Explain why H3PO3 is diprotic and not triprotic. (b) A 25.0-mL sample of an H3PO3 solution titrated with 0.102 M NaOH requires 23.3 mL of NaOH to neutralize both acidic protons. What is the molarityof the H3PO3 solution? (c) The original solution from part (b) has a pH of 1.59. Calculate the percentionization and Ka1 for H3PO3, assuming that Ka1 >> Ka2. (d) How does the osmotic pressure of a 0.050 M solution of HCl compare qualitatively with that of a 0.050 M solution of H3PO3? Explain.arrow_forwardWhich, if any, of the following statements are true? (a) The stronger the base, the smaller the pKb. (b) The stronger the base, the larger the pKb. (c) The stronger the base, the smaller the Kb. (d) The stronger the base, the larger the Kb. (e) The stronger the base, the smaller the pKa of its conjugate acid. (f) The stronger the base, the larger the pKa of its conjugate acid.arrow_forward1. The pH of a 0.1 M solution of a monobasic acid P is 1.0 while the pH of a 0.2 M solution of another monobasic acid Q is 3.4. (a) Which, P or Q. is a more concentrated solution? (b) Which, P or Q. is a stronger acid? (c) Which, P or Q, will react faster when a piece of magnesium is dropped to them? (d) Which, P or Q, contains more H'(aq) ions in 50 cm' solution? (e) Which, P or Q or both, can be neutralized by an alkali? (f) Name an instrument to measure the pH of the above solutions. (g) Is Pa strong acid? Explain your answer.arrow_forward
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