Concept explainers
(a)
Interpretation:
The product of reaction between hydrochloric acid and ammonia has to be identified. Also, the proton transfer in acid-base reaction of hydrochloric acid and ammonia has to be determined.
Concept Introduction:
In Bronsted–Lowry theory, acid is defined as a substance that donates a proton. In a solution, it dissociates to give
Base is defined as a substance that accepts a proton. In a solution, it dissociates to give
Brønsted–Lowry acid transfer a proton and form base as the other compound can accept a proton. This is called conjugate acid-base pair. In pair of conjugate acid and base, the acid form is protonated and the base form lost the proton.
Every base has a conjugate acid. They are related by loss or gain of proton. The expression for base and conjugate acid is as follows:
Every acid has a conjugate base. They are related by loss or gain of proton. The expression for conjugate base and acid is as follows:
The reaction mechanism in which proton is donated by a compound and accepted by the other compound is called a proton transfer reaction. It involves transfer of protons between two species in
(b)
Interpretation:
The product of reaction between hydrogen carbonate ion and nitric acid has to be identified. Also, the proton transfer in acid-base reaction of hydrogen carbonate ion and nitric acid has to be determined.
Concept Introduction:
Refer to part (a)
(c)
Interpretation:
The product of reaction between cyanide ion and formic acid has to be identified. Also, the proton transfer in acid-base reaction of cyanide ion and formic acid has to be determined.
Concept Introduction:
Refer to part (a)
(d)
Interpretation:
The product of reaction between acetate ion and water has to be identified. Also, the proton transfer in acid-base reaction of acetate ion and water has to be determined.
Concept Introduction:
Refer to part (a).
Want to see the full answer?
Check out a sample textbook solutionChapter 15 Solutions
Chemistry: Principles and Practice
- Write two BrnstedLowry acid-base reactions and show how they represent proton-transfer reactions.arrow_forwardFollow the directions of Question 19 for the following acids: (a) hypochlorous acid (b) formic acid, HCHO2 (c) acetic acid, HC2H3O2 (d) hydrobromic acid (e) sulfurous acidarrow_forwardA base is a substance that dissociates in water into one or more ______ ions and one or more ________. a.hydrogen . . . anions b.hydrogen . . . cations c.hydroxide . . . anions d.hydroxide . . . cationsarrow_forward
- In Arrhenius acidbase theory, what ion is responsible for the properties of a. acidic solutions b. basic solutionsarrow_forward. What does it mean to say that an acid is strong in aqueous solution? What does this reveal about the ability of the acids anion to attract protons?arrow_forwardClassify each of the following as a strong or weak acid or base. a NH3 b HCNO c Mg(OH)2 d HClO3arrow_forward
- Acidity of a solution is determined by the concentration H of hydrogen ions in the solution (measured in moles per liter of solution). Chemists use the negative of the logarithm of the concentration of hydrogen ions to define the pH scale, as shown in the following formula. pH = -log (H) Lower pH values indicate a more acidic solution. (a) Normal rain has a pH value of 5.6. Rain in the eastern United States often has a pH level of 3.8. How much more acidic is this than normal rain? (Round your answer to two decimal places.) 63.10 times as acidic as normal rain (b) If the pH of water in a lake falls below a value of 5, fish often fail to reproduce. How much more acidic is this than normal water with a pH of 5.6? (Round your answer to two decimal places.) * times as acidic as normal waterarrow_forwardAs K2O dissolves in water, the oxide ion reacts with water moleculesto form hydroxide ions. (a) Write the molecular and netionic equations for this reaction. (b) Based on the definitions ofacid and base, what ion is the base in this reaction? (c) What is theacid in the reaction? (d) What is the spectator ion in the reaction?arrow_forwardCalculate the pH of each of the following strong acid solutions. (a) 0.00813 M HBrO4 pH = (b) 0.443 g of HBr in 39.0 L of solution pH = (c) 25.0 mL of 6.80 M HBrO4 diluted to 2.00 L pH = (d) a mixture formed by adding 65.0 mL of 0.00719 M HBrO4 to 67.0 mL of 0.00254 M HBr pH =arrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub Co
- Chemistry for Today: General, Organic, and Bioche...ChemistryISBN:9781305960060Author:Spencer L. Seager, Michael R. Slabaugh, Maren S. HansenPublisher:Cengage LearningPrinciples of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage Learning