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Which of the following ionic compounds will be more
Chapter 17, Problem 68QP(choose chapter or problem)
Which of the following ionic compounds will be more soluble in acid solution than in water:
\(\text { (a) } \mathrm{BaSO}_{4}\)
\(\text { (b) } \mathrm{PbCl}_{2}\)
\(\text { (c) } \mathrm{Fe}(\mathrm{OH})_{3} \text {, }\)
\(\text { (d) } \mathrm{CaCO}_{3} \text { ? }\)
Questions & Answers
QUESTION:
Which of the following ionic compounds will be more soluble in acid solution than in water:
\(\text { (a) } \mathrm{BaSO}_{4}\)
\(\text { (b) } \mathrm{PbCl}_{2}\)
\(\text { (c) } \mathrm{Fe}(\mathrm{OH})_{3} \text {, }\)
\(\text { (d) } \mathrm{CaCO}_{3} \text { ? }\)
ANSWER:
Step 1 of 5
There is a relationship of dynamic equilibrium with that of the dissolving solids. This is referred to as the solubility equilibrium. When no more solids can be dissolved in any solution then this solution is referred to as the saturated solution.