Which, if any, of the following salts will be neutral in an aqueous solution?
In which choice are the 0.1 M aqueous solutions of salts ranked according to decreasing pH?
a) FeCl2, FeCl3, MgCl2, KClO2
b. NH4Br, NaBrO2, NaBr, NaClO2
Can anyone explain to me how you got to your answers? I’m so lost in Chem 106. >_<
KBr because it is made via the reaction of a strong acid and a strong base
KOH + HBr –> KBr + H2O
KClO2 is a weak acid, MgCl2 is a slightly acidic salt, FeCl2 and FeCl3 are acidic salts, FeCl3 more acidic than FeCl2 due to # of Cl atoms
KClO2 > MgCl2 > FeCl2 > FeCl3
NaBrO2 > NaClO2 > NaBr > NH4Br
not 100% sure, has to do with the number of oxygens and the halide size. NaBr is a neutral salt, NH4Br = acidic salt with NH4+ grabbing an OH- from water leaving H+
HClO2 stronger acid than HBrO2 so, NaClO2 would be a weaker base than NaBrO2