Using the solubility rules in Table 4.1 as a guide, predict whether an insoluble product forms when each of the following pairs of solutions is mixed. Write the balanced chemical equation if a precipitation reaction does occur.
(a) Pb(NO₃)₂ and sodium carbonate
(b) Ammonium bromide and AgClO₄
(c) Potassium hydroxide and copper(II) chloride
(d) Aammonium bromide and cobalt(II) sulfate

Strategy

Write the formulas of the new potential ionic compounds by making a table of cations and anions and their combinations. Use the solubility rules to determine whether any of the combinations are insoluble.

Table 4.1

Transcribed Image Text:

TABLE 4.1 Compounds Soluble Ionic Compounds Group 1A cations and NH Nitrates (NO3) Solubility Rules for lonic Compounds in Water Exceptions Perchlorates (CIO) Acetates (CH3COO-) Chlorides, bromides, iodides (Cl, Br, I) Sulfates (SO²) Insoluble Ionic Compounds Carbonates (CO3) Phosphates (PO) Hydroxides (OH-) 2+ Ag+, Hg₂+, Pb²+ Hg₂+, Pb²+, Sr²+, Ba²+ Group 1A cations,. NH Group 1A cations, NH Group 1A cations, NH, Sr²+, Ba²+