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I need help with this question. Some ionic compounds dissolve to a significant extent in water; some do not. It is difficult to use theoretical methods to predict the extent to which an ionic compound will dissolve. It is therefore convenient to use “solubility rules” in order to know which ionic compounds will significantly dissolve in water. Can you explain to me, please?

I need help with this question. Some ionic compounds dissolve to a significant extent in water; some do not. It is difficult to use theoretical methods to predict the extent to which an ionic compound will dissolve. It is therefore convenient to use “solubility rules” in order to know which ionic compounds will significantly dissolve in water. Can you explain to me, please?

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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I need help with this question. Some ionic compounds dissolve to a significant extent in water; some do not. It is difficult to use theoretical methods to predict the extent to which an ionic compound will dissolve. It is therefore convenient to use “solubility rules” in order to know which ionic compounds will significantly dissolve in water. Can you explain to me, please?

water; some do not. It is difficult to use theoretical methods to predict the extent to which an ionic compound will dissolve. It is therefore convenient to use "solubility rules" in order to know which ionic compounds will significantly dissolve in water. Use the solubility rules table to determine which of the following compounds are water soluble. a) potassium bromide water soluble b) silver bromide water in soluble c) sodium sulfate water soluble d) sodium hydroxide Water Soluble e) copper(II) chromate water insoluble f) lead(II) hydroxide water insoluble g) iron(III) nitrate water soluble h) copper(I) hydroxide water insoluble Compound Nitrates Chlorides, Bromides, and lodides Sulfates Compound Hydroxides Phosphates, Carbonates, and Chromates Solubility Rules Table Water Soluble Example NaNO3 NaCl K₂SO4 Example Exceptions None FePO4 Compounds containing Agt, Pb²+, or Hg, and HgI2 Water Insoluble Compounds containing Pb²+, Sr²+, Ba²+, or Hgt Exceptions Compounds containing alkali Mg(OH)2 (Group I) metals or Ca²+, Sr²+, Ba²+, NH4+ Compounds containing alkali (Group I) metals or NH4+ Exception Example None AgCl PbSO4 Exception Example(s) NaOH K2CO3, Li3PO4, Na₂CRO4
Transcribed Image Text:water; some do not. It is difficult to use theoretical methods to predict the extent to which an ionic compound will dissolve. It is therefore convenient to use "solubility rules" in order to know which ionic compounds will significantly dissolve in water. Use the solubility rules table to determine which of the following compounds are water soluble. a) potassium bromide water soluble b) silver bromide water in soluble c) sodium sulfate water soluble d) sodium hydroxide Water Soluble e) copper(II) chromate water insoluble f) lead(II) hydroxide water insoluble g) iron(III) nitrate water soluble h) copper(I) hydroxide water insoluble Compound Nitrates Chlorides, Bromides, and lodides Sulfates Compound Hydroxides Phosphates, Carbonates, and Chromates Solubility Rules Table Water Soluble Example NaNO3 NaCl K₂SO4 Example Exceptions None FePO4 Compounds containing Agt, Pb²+, or Hg, and HgI2 Water Insoluble Compounds containing Pb²+, Sr²+, Ba²+, or Hgt Exceptions Compounds containing alkali Mg(OH)2 (Group I) metals or Ca²+, Sr²+, Ba²+, NH4+ Compounds containing alkali (Group I) metals or NH4+ Exception Example None AgCl PbSO4 Exception Example(s) NaOH K2CO3, Li3PO4, Na₂CRO4
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