Asked by ryancon
Explain with a chemical equation why the pH of the salt solution is or is not the same as pure water: NaCl, NaC2H3O2, NH4Cl
We're working with salt and buffer solutions but the equations confuse me the most. Anything helps!!
We're working with salt and buffer solutions but the equations confuse me the most. Anything helps!!
Answers
Answered by
DrBob222
In NaCl, neither Na^+ nor Cl^- are hydrolyzed (react with water); therefore, NaCl solution is the same pH as H2O.
NaC2H3O2 is sodium acetate (I'll use NaAc) and Ac^- is hydrolyzed.
Ac^- + HOH ==> HAc + OH^- so the solution is basic because of the OH.
NH4Cl the NH4^+ is hydrolyzed.
NH4^+ + H2O ==> NH3 + H3O^+ so the solution is acidic.
Said another way, the Ac^- is a stronger base than H2O.
Said another way, the H2O is a stronger base then NH4^+
NaC2H3O2 is sodium acetate (I'll use NaAc) and Ac^- is hydrolyzed.
Ac^- + HOH ==> HAc + OH^- so the solution is basic because of the OH.
NH4Cl the NH4^+ is hydrolyzed.
NH4^+ + H2O ==> NH3 + H3O^+ so the solution is acidic.
Said another way, the Ac^- is a stronger base than H2O.
Said another way, the H2O is a stronger base then NH4^+
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