6) When the reversible reaction HC;H;O2 (aq) E> H*(aq) + C2H3O2(aq) is at equilibrium at roomtemperature, pH of the reaction mixture is 5.What will be the change in pH when you add a large amount of solid acetate (C2H30,Na) to thereaction mixture?a) pH will not change because C2H;O,Na is not a part of the reaction equation.b) pH will not change because acetic acid and sodium acetate form a bufferc) pH will decrease because the reaction will shift towards reactantsd) pH will increase because the reaction will shift towards reactants

The given chemical reaction in equilibrium is: HC2H3O2(aq) <------> H+(aq) + C2H3O2-(aq) ; pH…

Answered: 6) When the reversible reaction HC;H;O2…

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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When the reversible reaction HC2H;O2 (aq) E> H(aq) + C2H3O2 (aq) is at equilibrium at room temperature, pH of the reaction mixture is 5. What will be the change in pH when you add a large amount of NaOH (aq) to the reaction mixture? a) pH will not change because NaOH is not a part of the reaction equation. b) pH will not change because acetic acid and NaOH form a buffer. c) pH will increase because NaOH will completely neutralize acetic acid. d) pH will decrease because NaOH will completely neutralize acetic acid. In the reversible reaction A (aq) + B(aq) E > C(aq), reactant A is very expensive. What are two ways to get it to react as fully as possible to form as much C as possible? a) remove C as it forms, and use an excess of A b) add another reactant that will form a precipitate with B c) remove C as it forms, and use an excess of B d) add another reactant that will form a precipitate with A
6) Acetic Acid, HCH3COO, is a weak acid that reacts with water in the reaction below: HCH3COO(aq) + H2O (l) ⇌ CH3COO-(aq) + H3O+(aq)Explain what happens to the equilibrium and the pH with the addition of NaCH3COO(s).
COHSOH(ag) + H2On + CeHsO (aq) + H3O*(a9) Ka= 1.12 x 10-10 (a) Phenol is a weak acid that partially dissociates in water according to the equation above. Write the equilibrium-constant expression for the dissociation of the acid in water. (b) What is the pH of a 0.75 M CaHsOH(ag) solution? (C) For a certain reaction involving CaHsOH(ag) to proceed at a significant rate, the phenol must be primarily in its deprotonated form, C3H5O (eg). In order to ensure that the CsHsOH(aq) is deprotonated, the reaction must be conducted in a buffered solution. On the number scale below, circle each pH for which more than 50 percent of the phenol molecules are in the deprotonated form (CoHsO (aq). Justify your answer. 1 2 3 4 5 6 7 8 9 10 11 12 13 14 Justification: (d) CeHsOH(ag) reacts with NaOH(ag). Write a net ionic equation representing this reaction (aka: invasion equation). (e) What is the pH of the resulting solution when 30 mL of 0.40 M CSH5OH(aq) is added to 25 mL of 0.60 M NAOH. Show all work…
5. What concentration of acetate ion (CH3CO2') in 0.500 M CH3CO2H produces a buffer solution with pH = 5.00? (Ka = 1.8 x 10-5) CH;CO2H (aq) H20 (I) CH;CO, (aq) H30* (aq) + 6. A buffer solution is formed by adding 0.500 mol of sodium acetate (CH3CO2NA) and 0.500 mol of acetic acid (CH;CO2H) to 1.00LH,0. What is the pH of the solution at equilibrium? (K, 1.8 x 10°)
6a
4, . Consider the following equilibrium: base + -H H-Base Which of the following base(s) would favour the product in this reaction? Он CH;O NH3 NH2 CH3CO2 (1) (II) (III) (IV) (V) (a) | (b) IV (c) I, IV and V (d) I and II (e) IIl and IV
Give detailed Solution with explanation needed
Given below is the dissociation of NH3 in water having a Kb value of 1.8 × 10-5. The reaction started with the equilibration of 0.65 M NH3. A common ion that is 0.25 M NH4Cl, was added to the initial solution and waited for some time for the reaction to reach equilibrium once again. NH3(aq) + H2O(l) ↔ NH4+(aq) + OH-(aq) Determine the pH of the solution given after the addition of the common ion. The Kw of water is 1.0 × 10-14.
Give good solution
1
The K, for acetic acid (CH, COOH) is 1.737 x 10-5. What is the pK, for this acid? pK = Use the calculated pK, to determine the pH at which [CH, COOH] = [CH,COO"]. pH =
5. Which one of the following equations would make more products upon addition of acid (H)? Briefly explain. H,SO,(aq) 2 HSO, (aq) + H (aq) HCl(aq) 2H(aq) + Cl'(aq) NH, (aq) + OH(aq) 2 NH;(aq) +H,O(1) 2 Fe,0;(s) 2 2 FeO(s) + O>(g) H(aq) + NH;(1)2 NH, (aq)

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