Textbook Question
Write balanced complete ionic and net ionic equations for each acid–base reaction.
b. HCHO2(aq) + NaOH(aq) →
c. HC2H3O2(aq) + LiOH(aq) →
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6. Chemical Quantities & Aqueous Reactions
Complete Ionic Equations
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An unknown sample is analyzed using the general qualitative analysis scheme shown in Figure 18.16. The sequence of reagents shown in the figure are used and a precipitate in only produced when (NH4)2HPO4 in NH3 is added. Which of the following describes a set of ions that might be present in the solution?
A
Mg2+
B
Ba2+ and Mg2+
C
Ba2+, Mg2+ and Na+
D
Ag+, Ba2+, Mg2+ and NH4+
Verified step by step guidance1
Identify the reagent that causes the precipitation: (NH4)2HPO4 in NH3.
Understand that (NH4)2HPO4 in NH3 is used to precipitate certain metal ions as their phosphates.
Recall that Ba2+ and Mg2+ can form insoluble phosphates, while Na+ and NH4+ do not form precipitates with phosphate.
Consider the solubility rules: Ba3(PO4)2 and Mg3(PO4)2 are insoluble in water, leading to precipitation.
Conclude that the presence of Ba2+ and Mg2+ ions in the solution is consistent with the observed precipitation when (NH4)2HPO4 in NH3 is added.
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