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^+
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!!
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