Homework Help is Here – Start Your Trial Now!
Science
Chemistry
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?

Principles of Modern Chemistry
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter11: Solutions
Section: Chapter Questions
Problem 66AP: Relative solubilities of salts in liquid ammonia can differsignificantly from those in water. Thus,...
See similar textbooks
icon
Related questions
Question
100%

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
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 3 steps with 2 images

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Gravimetric Analysis
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
Recommended textbooks for you
Principles of Modern Chemistry
Principles of Modern Chemistry
Chemistry
ISBN:
9781305079113
Author:
David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:
Cengage Learning
General Chemistry - Standalone book (MindTap Cour…
General Chemistry - Standalone book (MindTap Cour…
Chemistry
ISBN:
9781305580343
Author:
Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:
Cengage Learning
Introductory Chemistry: A Foundation
Introductory Chemistry: A Foundation
Chemistry
ISBN:
9781285199030
Author:
Steven S. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry: The Molecular Science
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
Publisher:
Cengage Learning
Introductory Chemistry: A Foundation
Introductory Chemistry: A Foundation
Chemistry
ISBN:
9781337399425
Author:
Steven S. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
SEE MORE TEXTBOOKS