Equation for the dissociation of a compound can be represented as shown below:: → This arrow means the dissociation is complete (100%), irreversible, and that the compound is a strong electrolyte -> This arrow means the dissociation is incomplete (less than 100%), reversible, and that he compound is not a strong electrolyte Compound HCI Dissociation HCI + H2O (1) → H3O+ (aq) + Cl(aq) This fype of dissociation is described as 100% dissociation, complete and irreversible and the compound is said to be a strong electrolyte True False

Equation for the dissociation of a compound can be represented as shown below:: → This arrow means the dissociation is complete (100%), irreversible, and that the compound is a strong electrolyte -> This arrow means the dissociation is incomplete (less than 100%), reversible, and that he compound is not a strong electrolyte Compound HCI Dissociation HCI + H2O (1) → H3O+ (aq) + Cl(aq) This fype of dissociation is described as 100% dissociation, complete and irreversible and the compound is said to be a strong electrolyte True False

Introduction to General, Organic and Biochemistry

11th Edition

ISBN:9781285869759

Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Chapter8: Acids And Bases

Section: Chapter Questions

Problem 8.80P

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The question is in the photo attatched. Additonal information: intial pH measurment: 3.30 inital volume: 0.0L weak acid concentration: 0.042M weak acid volume: 0.25L NaOH concentration: 0.1M NaOH volume at equilibrium: 0.105L HA (aq) + NaOH (aq) -> NaA (aq) + H2O(l) HA being the unknown acid.
(a) Given that Ka for acetic acid is 1.8 x 10-5 and that hypochlorous acid is 3.0 x10-8 , which is a stronger acid? (b) Which is the stronger base, the acetate ion or the hypochlorite ion? (c) calculate the Kb values for the CHCOO- and ClO- .
Consider the following equilibrium between pentanoic acid and its conjugate base: | CH3CH,CH,CH2C0- H20 + H30+ CH;CH2CH,CH,C-OH Will lowering the pH shift the equilibrium to the right or to the left?
One way to determine the predominant species at equilibrium for an acid-base reaction is to say that the reaction arrow points to the acid with the higher value of pK. For example, NH, + H,0 NH, + H,O+ pK. pk, 9.24 pK-1.74 NH,+ + OH--→ NH, + H,0 рк, 9.24 pK, 15.7 Explain why this rule works.
8:43 1 ll 5GE Question 10 of 25 Submit Construct the expression for Kb for the weak base, CsH;N. CsH,N(aq) + H20(1) = OH (aq) + CsH;NH* (aq) 1 Based on the definition of Kb, drag the tiles to construct the expression for the given base. Kp = 5 RESET [H,O] [H;O*] [OH] [C;H;N] [C;H;NH*] [C;H,N¯] 2[H;O] 2[H;O*] 2[ОН] 2[C;H;N] 2[C;H;NH*] 2[C5H&N¯] [H,O]? [H;O*]? [OH]? [CsH;N]? [C;H;NH*]? [C;H,N¯]?
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Predict the products of the following acid-base reactions, and predict whether the equilibrium lies to the left or to the right of the reaction arrow: (a) O2-(aq) + H2O(l)<---> (b) CH3COOH(aq) + HS-(aq)<---> (c) NO2-(aq) + H2O(l)<--->
The dissociation constant of H2O at 25° C : O is 1.0 x 10-14 M2 O is 107 M-2. O is 10-7 M2. O is 1014 M-2. O cannot be measured.
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. Give an example of a Lewis acid-base pair and a frustrated Lewis acid-base pair. What is the difference between these two systems? What is the mechanism for the reaction with H2?
Write equilibrium-constant expressions for each of the following: A) the base dissociation of ethyl-amine, CH3CH2NH2. B) the acid dissociation of hydrogen cyanide, HCN. C) the dissociation of H3AsO4 to H3O^+ and AsO4^3-. D) the reaction of CO3^2- with H2O to give H2CO3 and OH^-.
Ff.283.