Question

1)Consider the following reaction including the hypothetical K value.

HC2H3O2	+	H2O	↔↔	C2H3O2-	+	H3O+	K = 8.74⋅10−38.74⋅10-3

What type of compound is HC₂H₃O₂? (acid/base) (strong/ weak )

2)

Consider the following reaction.

HF	+	H2O	↔↔	F-	+	H3O+	K = 5.69⋅10−35.69⋅10-3

What substance is behaving as the base?

Select an answer HF H2O F- H3O+   

What substance is the conjugate base?

Select an answer HF H2O F- H3O+

3)Consider the following reaction.

NH3	+	H2O	↔↔	NH4+	+	OH-	K = 7.15⋅10−37.15⋅10-3

What substance is behaving as the acid?

Select an answer NH3 H2O NH4+ OH-   

What substance is the conjugate acid?

Select an answer NH3 H2O NH4+ OH-

4)Consider the following steps in the dissociation of phosphoric acid.

Step 1	H3PO4	+	H2O	↔↔	H2PO4-	+	H3O+
Step 2	H2PO4-		H2O	↔↔	HPO42-		H3O+
Step 3	HPO42-		H2O	↔↔	PO43-		H3O+

In which step does H₂PO₄^- act as an acid? Select an answer step 1, step 2, step 3

In which step does H₂PO₄^- act as a conjugate base? Select an answer step 1 , step 2, step 3

Answer 1

acidity are species that are proton donor in aqueous solution

and base are proton acceptor

the strength of an acid orbase depends upon the degree of dissociation as well as dissociation constants it should be large for strong acids.

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