Part A : Part B: Question 7) What can you conclude about the pH of most solution

Question

Part A :

Part B:

Question 7) What can you conclude about the pH of most solutions that we ingest? When do we ingest solutions in the other half of the pH range?

Part C :

Question 8

a) Write a mass action or equilibrium constant expression for the hydrolysis of sodium acetate, NaC2H3O2.
Answer: Kb of C2H3O2-(aq) = [OH-(aq)]^1 [HC2H3O2(aq)]^1 / [C2H302-(aq)]^1

b.) derive a relationship between the equilibrium constant for hydrolysis in 5a and the equilibrium constant for the dissociation of acetic acid, HC2H3O2.
Answer:   HC2H302(aq) + H2O(l) ?? H3O+(aq) + C2H3O2-(aq)
K = [H3O+(aq)]^1 [C2H3O2-(aq)]^1 / [HC2H302(aq)]^1

c.) Evaluate the equilibrium constant for hydrolysis in 8b using Kw and the equilibrim constant for the dissociation of HC2H3O2 calculated in Part C.

d.) Compare your calculated equilibrium constant for hydrolysis in 8c with the value that can be calculated from your pH data in part A.

Please help me with question 7 and question 8 (c) (d). Please show all the answers and explain, thanks.

Explanation / Answer

7. Most of the solutions we ingest are weakly acidic in nature.

Solutions in the other half of the pH range i.e. weakly basic are ingested when we suffer from acidity (too much acid intake/ production by body). The base will react with the excessive acid to form salt via a neutralization reaction. Strongly acidic (pH < 3.5) and strongly basic (pH > 11.5) are not normally consumed as they are highly corrosive.

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