15.0g NH4Cl (ammonium chloride) salt is dissolved in 500.mL pure water. a) will

Question

15.0g NH4Cl (ammonium chloride) salt is dissolved in 500.mL pure water.

a) will the salt solution be acidic, basic, or neutral?

b)what will be the pH of the salt solution? (Kb=1.8x10^-15 of ammonia)


I know a) is acidic, please show how you solved for b)

Explanation / Answer

a) KCl ---> K+ and Cl- (strong base is KOH, strong acid is HCl, so neutral). b) NH4C2H3O2 ---> NH4+ is a strong base conjugate, just trust me..., and C2H3O2 is sorta nebulous, but not in the list of strong acids so.... predict basic solution. Balanced rxn would be: NH4C2H3O2 + H2O ---> (NH4)+(OH)- + (H)+(C2H3O2)- (I'm just showing the ionic charges so you can tell how they go together... you don't have to put them in your balanced equation Another way to write these is NH4C2H3O2 + H2O ---> NH4+(aq) + C2H3O2-(aq) the (aq) means aqueous and means it is dissolved in water

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