Pre-lab question #3-2: Consider the following equilibrium for nitrous acid, HNO2, aweak acid:HNO2 (aq) + H2O () → H30* (aq) + NO2 (aq)If NANO2 is added, in which direction will the equilibrium shift?A (no effect/right/left)

When there is a balance between direct and reverse reaction, chemical equilibrium is achieved. The…

Pre-lab question #3-2: Consider the following equilibrium for nitrous acid, HNO2, a weak acid: HNO2 (aq) + H2O () → H3O* (aq) + NO2'(aq) If NANO2 is added, in which direction will the equilibrium shift? A (no effect/right/left)

Pre-lab question #3-2: Consider the following equilibrium for nitrous acid, HNO2, a weak acid: HNO2 (aq) + H2O () → H3O* (aq) + NO2'(aq) If NANO2 is added, in which direction will the equilibrium shift? A (no effect/right/left)

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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Pre-lab question #3-4: Consider the following equilibrium for nitrous acid, HNO2, a weak acid: HNO2 (aq) + H2O () → H30* (aq) + NO2 (aq) If acid solution is made more dilute, in which direction will the equilibrium shift? A (no effect/right/left)
Question 5 (1 point) Equimolar quantities of potassium fluoride and hydrofluoric acid are placed into solution. The equilibrium established is as follows: HF(aq) + H2O(l) F¯(aq) + H30+(aq) What happens to the above equilibrium if some acetic acid is added to the solution? Acetic acid ionizes so pH significantly increases. Acetic acid isn't in the equilbrium equation so it will have no effect on the pH of the solution. The acetic acid creates more hydronium ion so the equlibrium shifts left and pH is not changed significantly. The acetic acid creates more hydronium ion so the reaction shifts right and pH is not changed significantly.
Question 5 (1 point) Equimolar quantities of potassium fluoride and hydrofluoric acid are placed into solution. The equilibrium established is as follows: HF(aq) + H2O(l) | F˜(aq) + H¸O*(aq) What happens to the above equilibrium if some acetic acid is added to the solution? Acetic acid ionizes so pH significantly increases. Acetic acid isn't in the equilbrium equation so it will have no effect on the pH of the solution. The acetic acid creates more hydronium ion so the equlibrium shifts left and pH is not changed significantly. The acetic acid creates more hydronium ion so the reaction shifts right and pH is not changed significantly.
Calculate the value for the equilibrium constant of this reaction: NH4+(aq)+HCO3(aq)→NH3(aq)+H2CO3(aq) where [NH4-]=0.25 M, [HCO3]=0.42 M, [NH3]=0.0078 M, and [H2CO3]=0.018 M. Answer The correct answer is: 1.3x10-3
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For the reaction below, Kc = 1.10 × 10-8. Note Kc is sometimes called K. What is the equilibrium concentration of OH- if the reaction begins with 0.610 M HONH,? HONH2 (aq) + H2O (1) HONH3+ (aq) + OH(aq)