Question

Predict whether the following solutions are acidic, basic, or neutral. (I don't understand how to determine this just by looking at them - Please explain!)

A. 0.100 M NaCLO

B. 0.100 M CsNO3

C. 0.100 M CH3NH4Cl

D. .0100 M CH3NH4IO3

E. 0.100 M NH3CN

Answer 1

A. 0.100 M NaCLO --> Na++ ClO- forms in solution

ClO- + H2O (forms hydrolysis) --> HClO + OH-

this is slightly basic , due to OH-

B. 0.100 M CsNO3

Cs + NO3- present, wont form any hydrolysis, thereofre neutral

C. 0.100 M CH3NH4Cl

CH3NH4Cl --> CH3NH4+ + Cl-

CH3NH4+ is acidic since it will donate H+

CH3NH4+ --> CH3NH3 + H+

acidic

D. .0100 M CH3NH4IO3

CH3NH4IO3 --> CH3NH4+ + IO3-

IO3- will not oform any compound in water

CH3NH4+ --> donates H+ and it will become acidic

E. 0.100 M NH3CN --> this won't exist, it is most likely NH4CN since we need a caiton/anion

NH3CN --> NH4+ and CN- is formed

NH4+ --> acidic

CN- --> CN- + H2O --> HCN --> basic

therefore, this dependson pKa values

CN- is a good base and NH4+ is a bad acid

pKa CN --> 10 approx

pKa NH4+ --> 9.25

expect

NH3+ and HCN , therefore, acidic