1. You will use Figure 6.18 and the solubility chart Table 6.3 in your textbook for this question. a) You will select tw
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1. You will use Figure 6.18 and the solubility chart Table 6.3 in your textbook for this question. a) You will select two pairs of ionic compounds using ions from Table 6.3 or Figure 6.18. The 1st pair of compounds when combined in water should lead to no reaction. The 2nd pair of compounds when combined in water should lead to a reaction. Explain your selection using the rules of solubility from Figure 6.18 or Table 6.3 1st pair: 2nd pair:
Nitrate NO₂ Chlorate CIO, Perchlorate CIO Acetate C,H,O, Chloride CI Bromide Br lodide |- Sulfate Hydroxide SO OH Sulfite So, Carbonate CO, Phosphate PO,³- Sodium Ammonium Potassium Silver Magnesium Calcium Barium Iron(II) Zinc Copper(II) Lead(II) Iron(III) Aluminum NH, Na K Ag Mg Ca Ba Fe Zn² CuPb² Fe³ AP Soluble Insoluble Figure 6.18 A graphical approach to the solubility rules is presented here. Notice that compounds containing the alkali metals, NH4+, NO3, CIO3, C1O4, and C2H3O2 are always soluble.
TABLE 6.3 Solubility Rules Compounds Containing These lons Are Nearly Always Soluble Alkali metals Ammonium Large -1 oxyanions Compounds Containing These lons Are Usually Soluble 2+ Halides (except Pb²+,. 2+ 2+ 2+ Sulfate (except Ba Ca², Pb Ag) Not Soluble Most other ions Agt) 5 + Li, Na, K, Rb NH4 NO3, C1O3, C1O4, C2H302 F, Cl, Br, I SO4²- 2-