Part 1. Warm-up - A few fundamental concepts 1A) Which of these combinations represent conjugate acid-base pairs? Select all that apply. O Multiple answers: Multiple answers are accepted for this question Select one or more answers and submit. For keyboard navigation. SHOW MORE V co, & CO2 a b NH, & NH," H* & H2 HSO, & so, d HCOOH & HCO0 B) Consider these four weak bases with the following base ionization constants. Which base will have the weakest conjugate acid? Base lonization Constant (Kb value) 1.0 x 10-3 3.0 x 10-5 2.6 x 10-7 B1 B2 B3 B4 4.0 x 10-9 Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a b B2 B4 1c) Solutions of strong acids have a lower pH than solutions of weak acids. Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a True False

Part 1. Warm-up - A few fundamental concepts 1A) Which of these combinations represent conjugate acid-base pairs? Select all that apply. O Multiple answers: Multiple answers are accepted for this question Select one or more answers and submit. For keyboard navigation. SHOW MORE V co, & CO2 a b NH, & NH," H* & H2 HSO, & so, d HCOOH & HCO0 B) Consider these four weak bases with the following base ionization constants. Which base will have the weakest conjugate acid? Base lonization Constant (Kb value) 1.0 x 10-3 3.0 x 10-5 2.6 x 10-7 B1 B2 B3 B4 4.0 x 10-9 Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a b B2 B4 1c) Solutions of strong acids have a lower pH than solutions of weak acids. Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a True False

Chemistry

10th Edition

ISBN:9781305957404

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

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

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 10RQ: For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen...

See similar textbooks

Similar questions

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.
How do the components of a conjugate acid—base pair differ from one another4? Give an example of a conjugate acid—base pair to illustrate your answer.
Which of the following compounds or ions has the weakest conjugate base? Briefly explain your choice. a) HCN b) HClO c) NH4+
1. Which of the following can act as a Lewis acid? (Hint : In each case, draw the Lewis electron dot structure of the molecule or ion. Are there lone pairs of electrons on the central atom? If so, it can be a Lewis base. Does the central atom lack an electron pair? If so, it can behave as a Lewis acid.) PH3 BCl3 H2S HS−
2. The molecule whose structure is illustrated here is amphetamine, a stimulant Which description best fits this molecule? (Note: There may be more than one answer.) Brønsted acid Lewis acid Brønsted base Lewis base
Each box represents an acid solution at equilibrium. Squares represent H+ ions, and circles represent the anion. Water molecules are not shown. Which figure represents a strong acid? Which figure is a weak acid?
Gastric juice, the digestive ?uid produced in the stomach, contains hydrochloric acid, HCl, Milk of Magnesia, a suspension of solid Mg(OH)2 in an aqueous medium, is sometimes used to neutralize-excess stomach acid. Write a complete balanced equation for the neutralization reaction, and identify the conjugate acid—base pairs.
Write equations that show NH3 as both a conjugate acid and a conjugate base.
Mark each of the following statements True or False: a. The conjugate base of a strong acid is always a weak base. b. The conjugate acid of a strong base is always a weak acid. c. The stronger the acid, the weaker its conjugate base, and vice versa.
The following reactions illustrate Brnsted acid-base behavior. Complete each equation. a.HI(aq)+?H3O+(aq)+I(aq) b.NH3(l)+?NH4++NH2 c.H2C2O4(aq)+H2O(l)?+HC2O4(aq) d.H2N2O2(aq)+H2O(l)H3O+(aq)+? e.?+H2O(l)H3O+(aq)+CO32(aq)
Trimethylamine, (CH3)3N, reacts readily with diborane, B2H6. The diborane dissociates to two BH3 fragments, each of which can react with trimethylamine to form a complex, (CH3)3N:BH3. Write an equation for this reaction and interpret it in terms of Lewis acid-base theory.
Consider the following four biological solutions: (1) bile, pH 8.0, (2) blood, pH 7.4, (3) urine, pH 6.0, and (4) gastric juice, pH 1.6. a. Which solution has the lowest [H3O+]? b. Which solution has the lowest [OH]? c. List the solutions in order of decreasing acidity. d. List the solutions in order of increasing basicity.