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 your text to look up Ka or Kb values if needed. HCO2H = formic acid; (CH3)2 = dimethyl amine.)

A. KCl

B. HCO2H

C. 50:50 mixture of HCO2H + NaHCO2

D. ((CH3)2NH2)Cl

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

F. 50:50 mixture of 0.1 M NaNO3 + 0.1 M HNO3

A. K+ + OH- + H+ + Cl- ---> KCl(aq) + H2O (l)

KCl is a neutral salt as it is the salt of strong base KOH and strong HCl.

B. HCOOH (aq) ---> H+(aq) + HCOO- (aq)

Very less ionization, weak acid, equillibrium lies to the left.

C. HCOOH + NaHCO3 ---> HCOONa (aq) + CO2 (g)+ H2O(l)

CO2 gas evolved and the solution will be slightly basic.

D. (CH3)2NH + HCl ---> ((CH3)2NH2)Cl + H2O ----> (CH3)2NH2+ (aq)+ Cl- (aq)

This a salt of a strong acid HCl and a week base dimethyl amine, so the aqueous solution will be slightly acidic.

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

It will be slightly basic.

F. 50:50 mixture of 0.1 M NaNO3 + 0.1 M HNO3

This is a mixture of salts of strong acid and base and another strong acid which will make it acidic solution.