In each row check off the boxes that apply to the highlighted reactant. The highlighted reactant acts as a... (check all that apply) reaction Brønsted-Lowry acid Brønsted-Lowry base 2 H2O2() → 2 H201) + O2(9) Lewis acid Lewis base Brønsted-Lowry acid Brønsted-Lowry base HCH,CO,(aq) + NH3(aq) → CH3CO, (aq) + NH (aq) Lewis acid Lewis base Brønsted-Lowry acid 2+ Brønsted-Lowry base Zn "(a9) + 6 CH,CN(aq) → Zn(CH,CN) , (aq) 9. Lewis acid Lewis base O O O O O

In each row check off the boxes that apply to the highlighted reactant. The highlighted reactant acts as a... (check all that apply) reaction Brønsted-Lowry acid Brønsted-Lowry base 2 H2O2() → 2 H201) + O2(9) Lewis acid Lewis base Brønsted-Lowry acid Brønsted-Lowry base HCH,CO,(aq) + NH3(aq) → CH3CO, (aq) + NH (aq) Lewis acid Lewis base Brønsted-Lowry acid 2+ Brønsted-Lowry base Zn "(a9) + 6 CH,CN(aq) → Zn(CH,CN) , (aq) 9. Lewis acid Lewis base O O O O O

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 28Q: The following are representations of acidbase reactions: a. Label each of the species in both...

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The following are representations of acidbase reactions: a. Label each of the species in both equations as an acid or a base and explain your answers. b. For those species that are acids, which labels apply: Arrhenius acid, BrnstedLowry acid, Lewis acid? What about the bases?
In each row check off the boxes that apply to the highlighted reactant. reaction The highlighted reactant acts as a...(check all that apply) Zn2+ (aq) + 6CH3CN (aq) → ZnCH3CN2+6 (aq) Brønsted-Lowry acid Brønsted-Lowry base Lewis acid Lewis base HCl (aq) + H2O (l) → Cl− (aq) + H3O+ (aq) Brønsted-Lowry acid Brønsted-Lowry base Lewis acid Lewis base HCH3CO2 (aq) + NH3 (aq) → CH3CO−2 (aq) + NH+4 (aq) Brønsted-Lowry acid Brønsted-Lowry base Lewis acid Lewis base
Drag the labels from the following list and drop them in the appropriate boxes for the Brønsted -Lowry acid-base reaction: HAsO42-(aq) + HSO4-(aq) ⇆ H2AsO4-(aq) + SO42-(aq).
Which correctly labels the Brønsted-Lowry acid, its conjugate base, the Brønsted-Lowry base, and its conjugate acid for H2O + PH2- → OH- + PH3? (Choose all that apply) Question 36 options: a) Brønsted-Lowry base = PH2- b) Brønsted-Lowry acid = H2O c) conjugate base: OH– d) conjugate acid: OH– e) conjugate acid: PH3 f) Brønsted-Lowry acid = PH2- g) conjugate base: PH3 h) Brønsted-Lowry base = H2O
In the following unbalanced reaction, which reactant acts like the Bronsted-Lowry acid? H3PO3 (aq) + H2O (l) --> H3O+ (aq) + PO33- (aq) Group of answer choices: H3PO3 PO33- H2O H3O+
Choose the letter of the correct answer. A substance that gives up or donates hydrogen ions during a chemical reaction. a. Bronsted-Lowry acid c. Conjugate acid Bronsted-Lowry base d. Conjugate base A substance that accepts hydrogen ions during a chemical reaction. a. Bronsted-Lowry acid c. Conjugate acid Bronsted-Lowry base d. Conjugate base A way to measure the strengths of acids and bases. a. Bronsted-Lowry acid c. pH scale Bronsted-Lowry base d. Ion-concentration constant What is the pH of a solution with a hydrogen-ion concentration of 3.75 x 10-3 M? 2.42 c. 9.96 b. 4.22 d. 6.99 Calculate the pH of a solution with [OH-] = 1.0 x 10-2 M and identify if it’s acidic or basic. pH = 2.0 acidic c. pH = 2.0 basic b. pH = 12.0 acidic d. pH = 12.0 basic Please answer all questions and show your solutions
Identify whether each species functions as a Brønsted-Lowry acid or a Brønsted-Lowry base in this net ionic equation. H2CO3 (aq) + HSO3- ⇌ HCO3- + H2SO3 (aq) Brønsted-Lowry Brønsted-Lowry Brønsted-Lowry Brønsted-Lowry In this reaction: The formula for the conjugate acid or base of H2CO3 is The formula for the conjugate acid or bace of HSO3- is
In water solution, acetylsalicylic acid acts as a weak acid:CH3COOC6H4COOH (aq) + H2O (l) ⇌ H3O+ (aq) + CH3COOC6H4CO2- (aq) Are the following Brønsted-Lowry acids or Brønsted-Lowry base H2O (l) CH3COOC6H4COOH (aq) H3O+ (aq) CH3COOC6H4CO2- (aq)
The pH of a 0.0200 M solution of an unknown acid is 2.56. What is the Ka of this acid? To solve this problem: Write the acid dissociation equilibrium for the generic acid “HA” Set up an ICE chart ( with x = the concentration of H3O+ at equilibrium) Write the expression for Ka. Fill this in with the concentrations of H3O+, A- and HA at equilibrium, in terms of x. What is x? Can you find it from the given information? You should be able to use the pH to get the concentration of H3O+, which is x. Do this. Now that you know x, plug in into the Ka expression and find Ka.
H3C—N̈H2 reacts with BF3 in a combination reaction, forming H3C—NH2—BF3 with a covalent bond between N and B. What is the role of H3C—N̈H2 in this reaction? a. Lewis acid b. Brønsted-Lowry base c. Brønsted-Lowry acid d. Lewis base
Which of the following statements is/are TRUE? Select one or more: a.NaHCO3 can be a Brønsted base but not an Arrhenius base. b.There are 2 conjugate acid-base pairs in a Brønsted-Lowry acid-base equation. c.The stronger the acid mixed with water, the less concentrated its conjugate base. d.Both H2PO4– and CH3COO– are considered amphiprotic species.
Consider the four statements below and indicate which ones are true (correct): (1) The reacting species for strong acids is H3O+ while that for weak acids is the molecular species (2) Of the four chlorine oxyacids (HClOx) only chloric acid is a strong acid. (3) Five of the six strong acids are monoprotic. (4) In the Bronsted-Lowry model for acids, and acid donates a proton while a base accepts a proton. Group of answer choices 3 1 4