(The Ka value for HF is 6.6 x 10*.) 3. Using the value of K, from the previous question, show how to calculate the value of K, for F, the conjugate base of HF.

Chemistry: Principles and Reactions
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Chapter14: Equilibria In Acid-base Solutions
Section: Chapter Questions
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(The Ka value for HF is 6.6 x 10.)
3. Using the value of K, from the previous question, show how to calculate the value of K, for F, the
conjugate base of HF.
4. A certain acid-base indicator is yellow in solution below pH 5.0 and red in solution above pH 7.0.
What color would you expect this indicator to be in solution at each of the following pH values?
a. pH = 3.0
b. pH = 6.0
c. pH 9.0
Transcribed Image Text:(The Ka value for HF is 6.6 x 10.) 3. Using the value of K, from the previous question, show how to calculate the value of K, for F, the conjugate base of HF. 4. A certain acid-base indicator is yellow in solution below pH 5.0 and red in solution above pH 7.0. What color would you expect this indicator to be in solution at each of the following pH values? a. pH = 3.0 b. pH = 6.0 c. pH 9.0
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