Please use this textbook link:

https://openstax.org/details/books/chemistry-atoms-first-2e

Click left tab "View Online" for free use after opening link above to answer these questions, providing examples and showing work with explanations when asked:

 

1. Define acids and bases, identify acid base reactions, explain what a conjugate acid-base pair represents and determine the conjugates of acids and bases (provide examples also of this last part of the question). (Book 14.1)

2. Determine relative strengths of conjugate bases based on the strength of the parent acid. Determine relative strengths of conjugate acids based on the strength of their parent base. Determine the equilibrium position for an acid base reaction based on the strength of the acid and base. (This question requires examples of work with explanations as well to solve for each) (Book 14.3)

 

3. Apply Kw at 25^oC and at different temperatures. (Book 14.1)

 

4. Explain what pH represents and the pH scale. Explain how to calculate pH and pOH. Explain how indicators work and what they are useful for. (Book 14.3)

 

5. Explain the difference between a strong and weak acid. Write some aqueous acid dissociation reactions with explanations. (Book 14.3)

 

6. Calculate the pH, Ka, % dissociation, of strong and weak acid solutions. Show work and provide explanations. (Book 14.3)

 

7. Explain the difference between a strong and a weak base. Perform pH calculations for strong base solutions, with explanations. (Book 14.3)

 

8. Show examples of aqueous weak base dissociation reactions and perform pH calculations on weak bases. Provide example also with explanations. (Book 14.3)

 

9. Explain pKa and pKb and their relationship to one another and acid or base strength. (Book 14.3)

 

10. Determine Ka and Kb for conjugate acids and bases based on their parent Kb and Ka. Show work and provide explanations.(Book 14.3)

 

11. Determine acidity or basicity of a salt solution. Show work and provide explanations (Book 14.4)

 

12. Explain how chemical structure influences the strength of acids and bases. (Book 14.3)

 

13.Explain what Lewis Acids and Bases are. (Book 15.2)

Acid base questions 

Step-by-step explanation

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1) An acid is any hydrogen-containing substance that is capable of donating a proton (hydrogen ion) to another substance. A base is a molecule or ion able to accept a hydrogen ion from an acid. Acidic substances are usually identified by their sour taste. 
identification of acid-base reaction : 

To determine whether a substance is an acid or a base, count the hydrogens on each substance before and after the reaction. If the number of hydrogens has decreased that substance is the acid (donates hydrogen ions). If the number of hydrogens has increased that substance is the base (accepts hydrogen ions).

In the Brønsted-Lowry definition of acids and bases, a conjugate acid-base pair consists of two substances that differ only by the presence of a proton (H?). A conjugate acid is formed when a proton is added to a base, and a conjugate base is formed when a proton is removed from an acid. 
HOCN and OCN^- are an example of a conjugate acid-base pair. The only difference between the two is a proton (H⁺). All acids have a conjugate base and all bases have a conjugate acid.

2) The relative strengths of acids may be determined by measuring their equilibrium constants in aqueous solutions. In solutions of the same concentration, stronger acids ionize to a greater extent, and so yield higher concentrations of hydronium ions than do weaker acids. The equilibrium constant for an acid is called the acid-ionization constant, K_a  and vice versa for base as a parent group having base ionization constant as Kb. The pKa values are mostly used in order the predict the position of the equilibrium of an acid-base reaction, as well as for choosing an acid or a base to protonate or deprotonate certain species.

For example. The reaction between acetic acid and sodium hydroxide is a simple acid-base reaction that you have probably used in your general chemistry course for the acid-base titration experiment:

CH3COOH + NaOH ? CH3COONa + H2O 

3) Endothermic processes are favoured by an increase in temperature and so as the temperature rises the equilibrium moves further to the right hand side and Kw gets larger. As Kw gets larger, so do the values of the hydrogen ion concentration and the hydroxide ion concentration. The value of Kw at 25 degrees Celsius is specifically 10^−14. Kw is an example of an equilibrium constant.
According to Le Chatelier, if you increase the temperature of the water, the equilibrium will move to lower the temperature again. It will do that by absorbing the extra heat.

That means that the forward reaction will be favoured, and more hydrogen ions and hydroxide ions will be formed. The effect of that is to increase the value of K_w as temperature increases.

4) pH is a measure of how acidic/basic water is. The range goes from 0 - 14, with 7 being neutral. pHs of less than 7 indicate acidity, whereas a pH of greater than 7 indicates a base. pH is really a measure of the relative amount of free hydrogen and hydroxyl ions in the water.  The pH scale is logarithmic and inversely indicates the concentration of hydrogen ions in the solution.

In order to calculate the pH, take the negative log of the hydronium ion concentration. To find the pOH, simply subtract the pH from 14. In order to calculate the pOH, take the negative log of the hydroxide ion concentration. To find the pH, simply subtract pOH from 14. 

Acid-base indicators are most often used in a titration to identify the endpoint of an acid-base reaction. They are also used to gauge pH values and for interesting color-change science demonstrations.