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Chapter 17: Problem 27

Define solubility, molar solubility, and solubility product. Explain the difference between solubility and the solubility product of a slightly soluble substance such as \(\mathrm{BaSO}_{4}\) .

Short Answer

Expert verified
Solubility is the capacity of a solute to dissolve in a solvent, and is usually measured in g/L. Molar solubility is the amount of moles that can be dissolved in a liter of solution and is usually measured in mol/L. The solubility product (Ksp) refers to the equilibrium between a solid and its ions in a solution. While solubility is the maximum amount of solute that can dissolve, the solubility product represents the equilibrium between the undissolved solute and the ions in the solution.

Step by step solution

01

Define Solubility

Solubility is a property referring to the ability of a given substance, the solute, to dissolve in a solvent. It is measured in terms of the maximum amount of solute that can be dissolved in a certain amount of solvent at a specific temperature.
02

Define Molar Solubility

Molar solubility is the number of moles of a substance (the solute) that can be dissolved per liter of solution before the solution becomes saturated. It is typically expressed in units of moles per liter (mol/L or M).
03

Define Solubility Product

The solubility product, often denoted Ksp, is a measure of the equilibrium between a solid and its respective ions in a solution. It is the product of the concentrations of the ions each raised to the power of their stoichiometric coefficient in the equilibrium equation.
04

Explain the difference between Solubility and Solubility Product

While solubility and the solubility product (Ksp) both pertain to how much solute can be dissolved in a solvent, they represent different concepts. Solubility refers to the maximum amount of solute that can dissolve in a certain volume of solvent at a given temperature. This is typically an experimental measurement. On the other hand, the solubility product is a value that represents the equilibrium between the undissolved solute and the ions in the solution. It is a constant at a given temperature for a given solute.

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Most popular questions from this chapter

Calculate the concentration of ions in these saturated solutions: (a) \(\left[\mathrm{I}^{-}\right]\) in AgI solution with \(\left[\mathrm{Ag}^{+}\right]=9.1 \times 10^{-9} \mathrm{M}\) (b) \(\left[\mathrm{Al}^{3+}\right]\) in \(\mathrm{Al}(\mathrm{OH})_{3}\) with \(\left[\mathrm{OH}^{-}\right]=2.9 \times 10^{-9} \mathrm{M}\)

Calculate the \(\mathrm{pH}\) of the \(0.20 \mathrm{M} \mathrm{NH}_{3} / 0.20 \mathrm{M} \mathrm{NH}_{4} \mathrm{Cl}\) buffer. What is the \(\mathrm{pH}\) of the buffer after the addition of \(10.0 \mathrm{~mL}\) of \(0.10 \mathrm{M} \mathrm{HCl}\) to \(65.0 \mathrm{~mL}\) of the buffer?

A sample of \(0.1276 \mathrm{~g}\) of an unknown monoprotic acid was dissolved in \(25.0 \mathrm{~mL}\) of water and titrated with \(0.0633 \mathrm{M} \mathrm{NaOH}\) solution. The volume of base required to reach the equivalence point was \(18.4 \mathrm{~mL}\). (a) Calculate the molar mass of the acid. (b) After \(10.0 \mathrm{~mL}\) of base had been added to the titration, the \(\mathrm{pH}\) was determined to be 5.87 . What is the \(K_{\mathrm{a}}\) of the unknown acid?

The solubility product of \(\mathrm{Mg}(\mathrm{OH})_{2}\) is \(1.2 \times 10^{-11}\) What minimum \(\mathrm{OH}^{-}\) concentration must be attained (for example, by adding \(\mathrm{NaOH}\) ) to make the \(\mathrm{Mg}^{2+}\) concentration in a solution of \(\mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}\) less than \(1.0 \times 10^{-10} M ?\)

Define buffer solution.
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