Question

# State whether each of the following aqueous solutions would be acidic, basic, or neutral and explain...

State whether each of the following aqueous solutions would be acidic, basic, or neutral and explain your answer.

Include the appropriate net-ionic equations to show why a given solution is acidic or basic. Use Ka or Kb values if needed.

a. HCO2H

b. 50:50 mixture of HCO2H + NaHCO2

c. ((CH3)2NH2)Cl

d. 50:50 mixture of (CH3)2)NH + ((CH3)2NH2)Cl

a) HCO2H

The solution of formic acid is acidic as in aqueous solution it give H+ ions.

HCO2H + H2O <------------> HCO2- + H3O+

b) acidic solution of a bufffer

HCO2H + H2O <------------> HCO2- + H3O+

HCO2- + H2O <------------> HCO2H + OH-

c) [(CH3)2NH2]Cl

The aqueous solution of thisis acidic in nature as it is a salt of weak base(CH3)2NH and strong acid HCl.

the ionic equation is

[(CH3)2NH2]+ + Cl- + H2O <--------------> (CH3)2NH + H3O+ + Cl-

and the net ionic equation i

[(CH3)2NH2]+ + H2O <--------------> (CH3)2NH + H3O+

d)

A 50: 50 mixtrue of weak base (CH#)2NH and its salt [(CH3)2NH2]Cl behaves as a buffer is a basic bufer .

Thus the solution is basic in nature.

The net ionic equations in water is

[(CH3)2NH2]+ + H2O <--------------> (CH3)2NH + H3O+

(CH3)2NH2 + H2O <--------------> [(CH3)2NH2]+ + OH-

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