HA is a weak acid. Which equilibrium corresponds to the equilibrium constant Kp for A ?а.А (aq) + ОН - (aq)НОА 2-(aq)b."A "aq) + H2О ()НА (ag) + ОН (aq)С.НА (aq) + ОН - (aq)H20 (1) + H+ (aq)d."A (aq) + Hз0 + (aq)НА (aq) + H20 ()е.НА (aq) + H20 () — Н2А + (аq) + ОН (аq)

Here, Equilibrium constant ( Kb ) for A- ion so A- ion abstracting H+ ion from water this is called…

Answered: HA is a weak acid. Which equilibrium…

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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What is the pH of a 0.652 M solution of hydroxylammonium, a weak acid with a K, of 1.1 x 10-6? Oa. 0.19 Ob. 3.07 Ос. 7.2 х 10-7 Od. 5.96 Oe. 6.14
a. A hydrochloric acid solution has a pH value of 3. Which of the following substances would increase the pH value of the solution when mixed with it? (1) Dilute ammonia solut(2) Dilute (3) WaterA(1) and (2) onlyB(1) and (3) onlyC(2) and (3) only D 1,2,3 b. Which of the following statements about a concentrated acid is correct?A. It can react with copper metal.B. It cannot react with copper(II) oxide.C. It is an acid that fully ionizes in water.D. It must contain hydrogen ions when in aqueous form. c. which of the following states of hydrogen chloride will not turn dry blue litmus paper red? (1) HCl gas(2) HCl in water(3) HCl in methylbenzene (an organic solvent)A. (1) onlyB. (2) onlyC. (1) and (2) onlyD. (1) and (3) only
Calculate the pOH of [H*]= 2.5 x 10-5 M. none 4.0 x 10-10 9.40 O 4.60 14.0
Exp. D: Calculate the molar concentrations for the species present in a 1.000 M solution of NaHCO3. HCO,¹ CO3²- Species Approx. Molar Concentration Show calculations: Nat H* 1. Calculate the pH of the sodium bicarbonate solution. OH CO₂
Sodium bisulfate, NaHSO4, is used in some household cleansers as a source of HSO4- ion, a weak acid. What is the pH (just H3O+) of a 0.75-M solution of HSO4- that completely dissociates? What happens to the pH if it does not completely dissociate? HSO4-1+ H2O à SO42- + H3O+ Table SO3 SO2 O2 Initial 0 M 0 M Change -2x Equilibrium 0.58
MED PH +POH 1 = -log₁ PH+ Por pk 55. Of the following salts, which one forms a solution with the highest pH? A) KCI B) NH4Cl C) NaBr D) KCN ад, Гонт = 1/ A) HA (aq) + H₂O (1) B) A (aq) + H3O+ (aq) C) HA (aq) + OH- (aq) D) A (aq) + OH- (aq) (E)) A (aq) + H₂O (1) 56. HA is a weak acid. Which equilibrium corresponds to the equilibrium constant K for A? E) Ca(NO3)2 H₂A+ (aq) + OH(aq) HA (aq) + H₂O (1) H₂O (1) + H+ (aq) HOA²- (aq) HA (aq) + OH (aq) A) 3870 B) 9.88 C) 12.28 D) 6.16 E) 7.21 57. Why does the rate of a gas-phase reaction increase when the temperature of the system is increased? A) Increasing the temperature makes the molecules move faster, which results in more molecular collisions. B) Increasing the temperature gives the molecules more energy, so more reactant molecules have enough energy to react together. C) Increasing the temperature makes the volume increase, which provides more space for the product molecules to occupy. (D) Statements A and B are correct. 58. What is the…
23. Consider a generic polyprotic acid H2YO3. What is an appropriate combination of acid dissociation constants for this acid? Kal Ka2 A. 2.1 x 104 8.9 x 10-5 В. 3.2 х 10-6 2.2 x 10-10 С. 4.5 х 10-10 6.7 x 10-6 D. 5.3 x 10-5 1.8 x 10-4
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A 0.121 M solution of acetic acid has a pOH of 11.20. What is the Ka of acetic acid? Oa. 2.5 x 10-6 Ob. 2.1 x 10-5 Oc. 3.3 x 10-22 Od. 1.6 x 103 Oe. 1.3 x 102
7. Determine the pH of the 3.4M HNO₂. The Ka = 4.0 x 10-4. HNO2(aq) + H₂O(1) NO₂ (aq) + H3O+ (aq)
Given the following Ka values, which one belongs to the strongest acid? The weakest acid?a. 6.2 x 10-8b. 1.8 x 10-5c. 7.5 x 10-3d. 4.9 x 10-10e. 6.8 x 10-4

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