Which of the following solutions will not form a precipitate when added to 0.10M NaOH?
a) 0.10 M MgBr2
b) 0.10 M NH4Br
c) 0.10 M FeCL2
http://en.wikipedia.org/wiki/Solubility_table#P
To determine which solution will not form a precipitate when added to 0.10M NaOH, we need to identify the compound that will remain soluble in the presence of NaOH. This can be done by considering the solubility rules for common ionic compounds.
a) 0.10 M MgBr2:
To determine if MgBr2 will form a precipitate, we need to check the solubility of magnesium salts. According to the solubility rules, most salts containing the magnesium ion (Mg2+) are soluble, including magnesium bromide (MgBr2). Therefore, MgBr2 is likely to form a precipitate when added to NaOH.
b) 0.10 M NH4Br:
To determine if NH4Br will form a precipitate, we need to check the solubility of ammonium salts. According to the solubility rules, most ammonium salts are soluble, including ammonium bromide (NH4Br). Therefore, NH4Br is likely to form a precipitate when added to NaOH.
c) 0.10 M FeCl2:
To determine if FeCl2 will form a precipitate, we need to check the solubility of iron salts. According to the solubility rules, most salts containing the iron ion (Fe2+) are not soluble with hydroxide ions (OH-). Therefore, FeCl2 is not likely to form a precipitate when added to NaOH.
Based on this analysis, the solution that will not form a precipitate when added to 0.10M NaOH is c) 0.10 M FeCl2.