What is the largest difference between the Arrhenius and Bronted Lowry acid/base definitions? A 0.05 M solution of a weak base has a pH of 8.7. What is the Kb? What is the pH of 0.8 M NaF? (Ka (HF) = 6.3X104)

What is the largest difference between the Arrhenius and Bronted Lowry acid/base definitions? A 0.05 M solution of a weak base has a pH of 8.7. What is the Kb? What is the pH of 0.8 M NaF? (Ka (HF) = 6.3X104)

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

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 6RQ: Two strategies are also followed when solving for the pH of a base in water. What is the strategy...

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Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

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What is the largest difference between the Arrhenius and Bronted Lowry acid/base
definitions?
A 0.05 M solution of a weak base has a pH of 8.7. What is the Kb?
What is the pH of 0.8 M NaF? (Ka (HF) = 6.3X10-4)

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Two strategies are also followed when solving for the pH of a base in water. What is the strategy for calculating the pH of a strong base in water? List the strong bases mentioned in the text that should be committed to memory. Why is calculating the pH of Ca(OH)2 solutions a little more difficult than calculating the pH of NaOH solutions? Most bases are weak bases. The presence of what element most commonly results in basic properties for an organic compound? What is present on this element in compounds that allows it to accept a proton? Table 13-3 and Appendix 5 of the text list Kb values for some weak bases. What strategy is used to solve for the pH of a weak base in water? What assumptions are made when solving for the pH of weak base solutions? If the 5% rule fails, how do you calculate the pH of a weak base in water?
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