7th Edition

ISBN: 9781119360889

Author: HYSLOP

Publisher: VST

Concept explainers

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 equilibri…

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.

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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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Textbook Question

Chapter 16, Problem 167RQ

Your blood at 37 °C needs to be maintained within a narrow pH range of 7.35 to 7.45 to maintain optimal health. What possible conjugate acid-base pairs are present in blood that can buffer the blood and keep it within this range?

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Chapter 16, Problem 166RQ

Chapter 16, Problem 168RQ

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Adding a few drops of a strong acid to water will lower the pH appreciably. However, adding the same number of drops to a buffer does not appreciably alter the pH. pH = 7.0 pH = 3.0 Water pH = 7.0 pH = 6.9 Buffer art A ovide an explanation for this. atch the words in the left column to the appropriate blanks in the sentences on the right. can be neutralized small can not be neutralized Submit is not dissolved Feedback large Review | Constants I Periodic Table Request Answer Reset Help When strong acid is added to a buffer, there is a small pH change because the added acid by one of the components in the buffer. Therefore, the effect on the [H3O+] in the solution is When strong acid is added to pure water, there is a large pH change because the added acid in pure water. This will result in a effect on the [H3O+] in the solution. Next >

Using the table of the weak base below, you have chosen Ammonia as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.65 M in this salt. The desired pH of the buffer should be equal to 8.8. Values of K, for Some Common Weak Bases Conjugate Acid Name Formula Ammonia Methylamine Ethylamine Aniline NH3 CH;NH2 CH;NH2 C,H;NH2 C;H;N NH,+ CH;NH3+ CH5NH3* CH;NH3* C;H;NH+ 1.8 × 10-5 4.38 × 10-4 5.6 x 10-4 3.8 × 10-10 Pyridine 1.7 x 10-9 2. Compute for pKb. (Write your answer in 2 decimal places).

Consider a solution that initially contains 0.40 mol fluoride anion and 0.30 mol of hydrogen fluoride. If 0.40 mol of HCl are added to this solution, which of the following statements is FALSE? You will still have a buffer solution at the end, since you’ll still have significant amounts of both weak base and conjugate weak acid The pH will have shifted to a lower pH You’ll essentially have a weak acid solution situation, with 0.7 mol HF at the end. You will no longer have a buffer solution, since all of the weak base will have reacted with the HCl. The buffer capacity was exhausted. none of the above

Chapter 16 Solutions

EBK STUDY GUIDE TO ACCOMPANY CHEMISTRY:

Ch. 16 - Prob. 1PE Ch. 16 - Practice Exercise 16.2 An aqueous solution of...Ch. 16 - Practice Exercise 16.3 Water draining from old...Ch. 16 - Because rain washes pollutants out of the air, the...Ch. 16 - Practice Exercise 16.5 Find the values of and ...Ch. 16 - Practice Exercise 16.6 Calculate the . (Hint: is...Ch. 16 - Practice Exercise 16.7 Calculate the , and pH in a...Ch. 16 - For each of the following acids, write the...Ch. 16 - For each of the following acids, write the...Ch. 16 - Practice Exercise 16.10 Use Table 16.2 to find all...

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