Hydrogen fluoride (HF) behaves as a weak acid in aqueous solution. Two equilibriainfluence which fluorine-containing species are present in solution. Answer Parts1-3 below.HF(g)+H,0(1)= H,0"(aq) +F (aq) K=1.10 × 10-3F (aq)+HF(g)HF, (ag) K =2.60 × 10¬1Part 1.Is fluoride in pH 7.00 drinking water more likely to be present as F (aq)or HF2 (aq)?Choose one:F-(aq)HF2 (ag) Part 2What is the equilibrium constant for this equilibrium?2HF(g) + H,0(1) H,0*(aq) + HF, (aq)x 10Part 3What is the pH of HF2 in a 0.165 M solution of HF?pH

pH is used to determine the concentration of hydronium ion.

Hydrogen fluoride (HF) behaves as a weak acid in aqueous solution. Two equilibria influence which fluorine-containing species are present in solution. Answer Parts 1-3 below. HF(g) + H,0(1) = K =1.10 × 10-3 H,0"(aq) +F (aq) F (aq)+HF(g) HF, (aq) K-2.60 x 10-1 Part 1. Is fluoride in pH 7.00 drinking water more likely to be present as F"(aq) or HF2 (aq)? Choose one: F(aq) HF2 (ag)

Hydrogen fluoride (HF) behaves as a weak acid in aqueous solution. Two equilibria influence which fluorine-containing species are present in solution. Answer Parts 1-3 below. HF(g) + H,0(1) = K =1.10 × 10-3 H,0"(aq) +F (aq) F (aq)+HF(g) HF, (aq) K-2.60 x 10-1 Part 1. Is fluoride in pH 7.00 drinking water more likely to be present as F"(aq) or HF2 (aq)? Choose one: F(aq) HF2 (ag)

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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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.
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