The following equation describes the equilibrium that exists when the weak acid propionic acid (C2H5 CO,H) dissolves in water. (In acting as an acid, the -CO2H group supplies H+ to form H30*.)C2H; CO,H(aq) +H2O(l) 2 H,0+ (aq) + C2 H; CO2-(aq)a Which of the four species are Bronsted-Lowry acids?(Select all that apply.)O H20O C2H; CO2-O H3o+O C2H; CO,Hb Which of the four species are Brønsted-Lowry bases?(Select all that apply.)O H2OO C2H;CO2O H30+O C;H; CO,H

We have to identify the Bronsted Lowry acids and bases for the following given reaction as follows…

Answered: The following equation describes the…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 7P

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What is the pH of a grapefruit that contains 0.007 M citric acid solution (CsH2O-)? CH;O;(aq) + H;O(2) = CH;0, (aq) + H3Oʻ(aq) K, = 7.5 x 104 Round your answer to 2 decimal places.
3. A 0.0560 g quantity of acetic acid is dissolved in enough water to make 50.0 mL of solution. Calculate the concentrations of H;O*, CH;COO and CH;COOH at equilibrium. What is the pH of the solution? (Ka = 1.8x10) CH;COOH(aq) = CH;COO (aq) + H;O* (aq) a) Calculate the initial concentration of CH;COOH. (C:12; H:1; 0:16) b) Calculate the concentration of CH;CoO (aq) and H;O* (aq) at equilibrium. c) Calculate pH of the solution.
Based on the Lewis structures of the reactants and product of the following equation, identify the Lewis acid and the Lewis base in it: CO, + OH → HCO, =c=0: + :0-H H-0- O: O Lewis acid: CO,; Lewis base: HCO, O Lewis acid: OH; Lewis base: CO, O Lewis acid: CO; Lewis base: OH-
For the following acid-base reaction, (1) predict the products, showing both reactants and products complete Lewis structures and arrows showing electron flow; (2) label each structure with the lowing: Bronsted acid, Bronsted base, conjugate acid, conjugate base; (3) give a brief definition of a ronsted acid and Bronsted base; (4) predict the direction of the equilibrium and justify your answer. HC0OH + CH3 Nta PRん106Y pkb = 3.36
8) What is the pH of a 0.035 M HNO, solution? HNO3 (aq) + H,0 (1) H;O* (aq) + NO; (aq)
The ionization constant of lactic acid, CH,CH(OH)CO,H, an acid found in the blood after strenuous exercise, is 1.36 x 10-4. What is the concentration of hydronium ion in the solution of 0.102 M lactic acid? CH;CH(OH)CO,H (aq) + H,O (1) → H;O• (aq) + CH;CH(OH)CO, (aq) O 0.00372 M O 0.0165 M O 0.00549 M O 0.227 M
н (ад) + Crz0; (ag) + СHон() acid Сf" (ag) + Co:(s) + H.0()
8:35 : Question 22 of 23 Submit Which one of the following correctly shows the weak acid equilibrium for trichloroacetic acid, CCl,COOH? A) CCl,COOH (aq) = CCl;CO* (aq) + OH- (aq) В) Cli,COOH (аq) + H,0 (I) — СCl,COOH, (aд) + ОН- (аф) C) CCl,COOH (aq) + H20 (1) = CCI,COO- (aq) + H30* (aq) D) CCl;COOH (aq) + H2O (I) CCl,CO(OH), (aq) + H* (aq) Tap here or pull up for additional resources
Phenylamine is an aromatic amine that is used in the manufacture of dyes. When absorbed through the skin itcauses the Fe+2 in hemoglobin to become oxidized into Fe+3, resulting in the formation of methemoglobin whichcannot bind to or transport oxygen. Phenylamine is soluble in water and acts as a weak base.C6H5NH2 (aq) + H2O (ℓ) ⇋ C6H5NH3+ (aq) + OH- (aq)a. When you measure the concentrations of the ionized substances you find them to be:[C6H5NH2] = 0.234 mol/L [C6H5NH3+] = 2.8 x 10-5 mol/L [OH-]= 2.8 x 10-5 mol/LIf the Kb is 4.27 x 10-10, is the reaction at equilibrium? If not, which direction does it need to move (rightor left) to reach equilibrium? Explain. b. At equilibrium the concentrations of the ionized substances are:[C6H5NH2] = 0.0537 mol/L [C6H5NH3+] = 4.79 x 10-6 mol/L [OH-]= 4.79 x 10-6 mol/LIf this reaction is taking place in a 2.0L container, and 1.5 moles of phenylamine were added to thereaction, what will the new concentrations of the three ionic species be when…
4. A student has prepared 0.05 M solution of CH3-C=CH and has added to it 0.05 M solution of potassium tert-butoxide (K" O-C(CH3)3). (i) Write the equation for the acid-base reaction that might occur. (ii) With curved arrows track the movements of electron pairs. (iii) Assign Base, Acid, Conjugate acid for the base, Conjugate base for the acid. (iv) Calculate the percentage of deprotonated methyl acetylene taking into account that pKa of the conjugate acid of potassium tert-butoxide equals 18 and pKa of methyl acetylene equals 24.
In the reaction HSO4 (aq) + OH (aq) – so,2-(aq) + H20 (1), the conjugate acid- base pairs are HSO4 and So,2-; H20 and OH HSO4 and H30*; S04 2-and OH HSO4 and OH; so,2-and H20 HSO4 and H20; OHTand SO,2- HSO4 and OH; so,2-and H30*
Consider the following reaction: CH, ÇH, + :çi-A-Ci: H,C- A-: H,C- 50 CH3 Based on the reaction above, the reactant which acts as a Lewis base is CAICL CAICIs o(CH);CCI O(CH),C* The product which is a Lewis acid is OAICI O(CH,),cCI CAICI o(CH)C" The following salts can replace AICla in the reaction, except OBeCl OMgCl OFeCl ocrCls

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