4) 99% 31 Sun Oct 29 ndow Hel MasteringChemist er16 HW # mView?offset-next&assignmentProblemID-85550273 Resources «previous 6 of 16 nex The common-ion effect and solubility The solubility of a slightly soluble salt can be greatly affected by the addition of a soluble salt with a common ion, that is, with one of the ions in the added soluble salt being identical to one of the ions of the slightly soluble salt. The general result of the addition of the common ion is to greatly reduce the solubility of the slighty soluble salt In other words, the addition of the common ion results in a shift in the equilibrium of Part B Calculate the molar solubility in NaOH Based on the given value of the Ksp, what is the molar solubility of Mg(OH)2 in 0.100 MNaOH? Express your answer with the appropriate units molar solublity 2.86 10 M Submlt My Answers Give Up Incorrect; Try Again Part C
The solubility of a slightly soluble compound can be greatly affected by the addition of a soluble compound with a common ion, that is, with one of the ions in the added soluble compound being identical to one of the ions of the slightly soluble compound. The general result of the addition of the common ion is to greatly reduce the solubility of the slightly soluble compound. In other words, the addition of the common ion results in a shift in the equilibrium of the slightly soluble compound.
Part B - Calculate the molar solubility in NaOH
Based on the given value of the Ksp, what is the molar solubility of Mg(OH)2 in 0.200 M NaOH?
Express your answer with the appropriate units.
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molar solubility =
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Part C
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The common-ion effect and buffer systems
A buffer is a mixed solution of a weak acid or base, combined with its conjugate. Note that this can be understood essentially as a common-ion problem: The conjugate is a common ion added to an equilibrium system of a weak acid or base. The addition of the conjugate shifts the equilibrium of the system to relieve the stress of the added concentration of the common ion. In a solution consisting of a weak acid or base, the equilibrium shift also results in a pH shift of the system.
It is the presence of the common ion in the system that results in buffering behavior, because both added H+ or OHâ ions can be neutralized.
Part D
What is the pH change of a 0.290 M solution of citric acid (pKa=4.77) if citrate is added to a concentration of 0.145 M with no change in volume?
Express the difference in pH numerically to two decimal places.