13. What is the difference between a strong acid and a weak acid? A) a strong acid contains strong covalent bonds whereas a week acid does not B) a strong acid has more hydrogen atoms in its molecule than a weak acid C) a weak acid is nonpolar, whereas a strong acid is polar D) strong acids react with both strong and weak bases, whereas weak acids do not E) none of the above A B CDE OOOOO

13. What is the difference between a strong acid and a weak acid? A) a strong acid contains strong covalent bonds whereas a week acid does not B) a strong acid has more hydrogen atoms in its molecule than a weak acid C) a weak acid is nonpolar, whereas a strong acid is polar D) strong acids react with both strong and weak bases, whereas weak acids do not E) none of the above A B CDE OOOOO

World of Chemistry, 3rd edition

3rd Edition

ISBN:9781133109655

Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Chapter16: Acids And Bases

Section: Chapter Questions

Problem 2STP

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Similar questions

A 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 . . . cations
For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen atom? b. the electronegativity of the element bonded to the oxygen atom that bears the acidic hydrogen? c. the number of oxygen atoms? How does the strength of a conjugate base depend on these factors? What type of solution forms when a nonmetal oxide dissolves in water? Give an example of such an oxide. What type of solution forms when a metal oxide dissolves in water? Give an example of such an oxide.
Differentiate between the terms strength and concentration as they apply to acids and bases. When is HCl strong? Weak? Concentrated? Dilute? Answer the same questions for ammonia. Is the conjugate base of a weak acid a strong base?
Explain the difference between a strong acid and a weak acid.
Classify the solutions represented in Exercises 9.28 and 9.30 as acidic, basic, or neutral.
Consider two beakers of pure water at different temperatures. How do their pH values compare? Which is more acidic? More basic? Explain.
According to the Arrhenius theory of acids and bases, how do you recognize an acid and a base?
Arsenic acid (H3AsO4) is a moderately weak triprotic acid. Write equations showing its stepwise dissociation. Which of the three anions formed in these reactions will be the strongest Brnsted base? Which will be the weakest Brnsted base? Explain your answers.
What is a salt? List some anions that behave as weak bases in water. List some anions that have no basic properties in water. List some cations that behave as weak acids in water. List some cations that have no acidic properties in water. Using these lists, give some formulas for salts that have only weak base properties in water. What strategy would you use to solve for the pH of these basic salt solutions? Identify some salts that have only weak acid properties in water. What strategy would you use to solve for the pH of these acidic salt solutions? Identify some salts that have no acidic or basic properties in water (produce neutral solutions). When a salt contains both a weak acid ion and a weak base ion, how do you predict whether the solution pH is acidic, basic, or neutral?