Solubility Product (Ksp)

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Questions and Answers

What does a smaller value of the solubility product constant (Ksp) indicate?

  • The system is not at equilibrium.
  • Higher ion concentrations in a saturated solution, indicating greater solubility.
  • A faster rate of dissolution of the solid compound.
  • Lower ion concentrations in a saturated solution, indicating lower solubility. (correct)

Which of the following is the correct Ksp expression for aluminum hydroxide ($Al(OH)_3$)?

  • Ksp = [Al][OH]
  • Ksp = [Al$^{3+}$][OH$^-$]$^3$ (correct)
  • Ksp = [Al][OH]$^3$
  • Ksp = [Al$^{3+}$][3OH$^-$]

A saturated solution of $PbCl_2$ has a lead(II) ion concentration of $1.6 \times 10^{-2}$ M. What is the Ksp for $PbCl_2$?

  • $1.0 \times 10^{-4}$
  • $1.6 \times 10^{-5}$
  • $2.0 \times 10^{-4}$
  • $5.1 \times 10^{-5}$ (correct)

The Ksp of $Ag_2CrO_4$ is $1.1 \times 10^{-12}$. What is the concentration of chromate ions ($CrO_4^{2-}$) in a saturated solution?

<p>$6.5 \times 10^{-5}$ M (D)</p> Signup and view all the answers

The Ksp for $Fe(OH)_3$ is $2.8 \times 10^{-39}$. What is the molar solubility of iron(III) hydroxide in water?

<p>$1.0 \times 10^{-10}$ M (A)</p> Signup and view all the answers

What is the purpose of an ICE chart in Ksp calculations?

<p>To determine the equilibrium concentrations of ions in a saturated solution. (B)</p> Signup and view all the answers

If the molar solubility of $AgCl$ in pure water is $1.34 \times 10^{-5}$ mol/L, what is its Ksp value?

<p>$1.80 \times 10^{-10}$ (A)</p> Signup and view all the answers

For the dissolution of $BaF_2(s) \rightleftharpoons Ba^{2+}(aq) + 2F^-(aq)$, which expression correctly relates the molar solubility, s, to the Ksp?

<p>Ksp = 4s^3 (C)</p> Signup and view all the answers

For a sparingly soluble salt $M_xN_y$ that dissociates in water according to the equation $M_xN_y(s) ightleftharpoons xM^{y+}(aq) + yN^{x-}(aq)$, which of the following expressions correctly represents the Ksp?

<p>$K_{sp} = [M^{y+}]^x[N^{x-}]^y$ (A)</p> Signup and view all the answers

Which of the following correctly describes the relationship between the solubility of a salt and its Ksp value?

<p>As solubility increases, the Ksp value increases. (B)</p> Signup and view all the answers

Consider a solution containing $Mg^{2+}$ ions. If $NaOH$ is added, causing $Mg(OH)_2$ to precipitate, what condition must be met for precipitation to occur?

<p>The ion product, Q, must be greater than the Ksp. (E)</p> Signup and view all the answers

The Ksp of $AgCl$ is $1.6 imes 10^{-10}$. What will happen if you mix $50 mL$ of $2.0 imes 10^{-5} M$ $AgNO_3$ with $50 mL$ of $2.0 imes 10^{-5} M$ $NaCl$?

<p>No precipitate will form because the ion product is less than the Ksp. (B)</p> Signup and view all the answers

The solubility of $PbCl_2$ in water is found to be $s$ mol/L at a certain temperature. Which of the following expressions represents the Ksp for $PbCl_2$ in terms of $s$?

<p>$K_{sp} = 4s^3$ (A)</p> Signup and view all the answers

How does the addition of a common ion affect the solubility of a sparingly soluble salt?

<p>It decreases the solubility of the salt. (D)</p> Signup and view all the answers

Which of the following statements is correct regarding the Ksp of a slightly soluble ionic compound at a given temperature?

<p>The Ksp value is constant as long as the temperature remains constant. (B)</p> Signup and view all the answers

For $CaF_2$, $Ksp = 3.9 imes 10^{-11}$. Determine the molar solubility of $CaF_2$ in a solution containing 0.10 M $NaF$.

<p>$3.9 imes 10^{-9} M$ (B)</p> Signup and view all the answers

Match each sparingly soluble compound with its correct Ksp expression:

<p>Silver Chloride (AgCl) = Ksp = [Ag+][Cl-] Lead(II) Iodide (PbI2) = Ksp = [Pb2+][I-]^2 Iron(III) Hydroxide (Fe(OH)3) = Ksp = [Fe3+][OH-]^3 Barium Sulfate (BaSO4) = Ksp = [Ba2+][SO42-]</p> Signup and view all the answers

Match the following scenarios with the correct mathematical setup to calculate molar solubility:

<p>Ksp of AgCl is $1.8 \times 10^{-10}$ = $x = \sqrt{1.8 \times 10^{-10}}$ Ksp of $MgF_2$ is $6.4 \times 10^{-9}$ = $x = \sqrt[3]{\frac{6.4 \times 10^{-9}}{4}}$ Ksp of $Ag_2CrO_4$ is $1.1 \times 10^{-12}$ = $x = \sqrt[3]{\frac{1.1 \times 10^{-12}}{4}}$ Ksp of $CaF_2$ is $3.2 \times 10^{-11}$ = $x = \sqrt[3]{\frac{3.2 \times 10^{-11}}{4}}$</p> Signup and view all the answers

Match each sparingly soluble compound with the correct expression relating its molar solubility (s) to its Ksp:

<p>AgCl = Ksp = s^2 PbI2 = Ksp = 4s^3 Ag2S = Ksp = 4s^3 Al(OH)3 = Ksp = 27s^4</p> Signup and view all the answers

Match the given Ksp values to their corresponding Magnesium Hydroxide ion concentrations, given $[Mg^{2+}] = x$:

<p>Ksp = $4.0 \times 10^{-12}$ = $[OH^-] = 2 \times \sqrt[3]{\frac{4.0 \times 10^{-12}}{4}}$ Ksp = $1.0 \times 10^{-11}$ = $[OH^-] = 2 \times \sqrt[3]{\frac{1.0 \times 10^{-11}}{4}}$ Ksp = $2.0 \times 10^{-13}$ = $[OH^-] = 2 \times \sqrt[3]{\frac{2.0 \times 10^{-13}}{4}}$ Ksp = $8.0 \times 10^{-10}$ = $[OH^-] = 2 \times \sqrt[3]{\frac{8.0 \times 10^{-10}}{4}}$</p> Signup and view all the answers

Match the sparingly soluble salts to their approximate molar solubility in water:

<p>Silver chloride (AgCl), Ksp = $1.6 \times 10^{-10}$ = $1.3 \times 10^{-5}$ M Lead(II) chloride ($PbCl_2$), Ksp = $1.6 \times 10^{-5}$ = $1.6 \times 10^{-2}$ M Silver chromate ($Ag_2CrO_4$), Ksp = $1.1 \times 10^{-12}$ = $6.5 \times 10^{-5}$ M Calcium fluoride ($CaF_2$), Ksp = $4.0 \times 10^{-11}$ = $2.1 \times 10^{-4}$ M</p> Signup and view all the answers

Reaction of Calcium Hydroxide ($Ca(OH)_2$) in solution produces hydroxide. Match each amount of $Ca(OH)_2$ dissolved with the concentration of hydroxide, given the dissolution:

<p>0.005 M = 0.010 M 0.025 M = 0.050 M 0.100 M = 0.200 M 0.500 M = 1.000 M</p> Signup and view all the answers

Match each condition or change with its effect on the solubility of $Mg(OH)_2$:

<p>Increase in pH = Decreases solubility Decrease in pH = Increases solubility Addition of $MgCl_2$ = Decreases solubility Addition of $NaOH$ = Decreases solubility</p> Signup and view all the answers

Given differing $K_{sp}$ values, match the salt with its relative solubility

<p>$K_{sp} = 1.0 \times 10^{-5}$ = Highest Solubility $K_{sp} = 1.0 \times 10^{-8}$ = Moderately High Solubility $K_{sp} = 1.0 \times 10^{-12}$ = Moderately Low Solubility $K_{sp} = 1.0 \times 10^{-16}$ = Lowest Solubility</p> Signup and view all the answers

Flashcards

Solubility Product (Ksp)

Quantifies the degree to which a substance dissolves, representing the equilibrium between a solid and its ions in a saturated solution.

Saturated Solution Equilibrium

Represents the dynamic equilibrium of a solid dissolving into its ions in a solution.

Writing Ksp Expressions

Ksp = [Products]^coefficients. Solids are excluded.

Ksp Magnitude

Lower Ksp indicates lower ion concentrations.

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Calculating Ksp

  1. Write the equilibrium reaction.
  2. Measure the [ion].
  3. Calculate the [other ion(s)] based on stoichiometry.
  4. Calculate Ksp.
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Molar Solubility

Moles/liter of a substance that dissolves in a solution. Determined using an ICE chart.

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Predicting Ion Concentrations from Ksp

  1. Write the equilibrium reaction.
  2. Create an ICE chart.
  3. Substitute equilibrium concentrations into the Ksp expression.
  4. Solve for X (molar solubility).
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Molar Solubility (X)

The 'X' value calculated from the Ksp expression using an ICE chart, representing the molar solubility of the compound.

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Solubility

The process where ionic compounds disperse into a solution due to ion-dipole interactions with water molecules.

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Insoluble Ionic Compounds

Ionic compounds that do not dissolve in solution and remain in solid form.

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Ksp Definition

The equilibrium constant (Ksp) for the dissolution of a solid substance into an aqueous solution.

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Solids in Ksp

The Ksp expression excludes solids because their concentration remains constant.

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CaCO3 Dissociation

CaCO3(s) ⇌ Ca^2+(aq) + CO3^2-(aq). Ksp = [Ca^2+][CO3^2-].

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Mg(OH)2 Dissociation

Mg(OH)2(s) ⇌ Mg^2+(aq) + 2OH-(aq). Ksp = [Mg^2+][OH^-]^2.

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Mg(OH)2 Ksp Calculation

Dissolves according to: Mg(OH)2(s) ⇌ Mg^2+(aq) + 2OH-(aq). If [Mg^2+] = 3.7 x 10^-6 M, then [OH-] = 7.4 x 10^-6 M. Ksp = 2.0 x 10^-13.

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CuBr Molar Solubility

Used to find molar solubility by setting up an ICE chart with the equation CuBr(s) ⇌ Cu^+(aq) + Br-(aq).

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Ksp Expression

The product of ion concentrations, each raised to the power of their stoichiometric coefficient.

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Low Ksp Value

Lower solubility of a compound.

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Calcium Carbonate Ksp

CaCO3(s) ⇌ Ca^2+(aq) + CO3^2-(aq); Ksp = [Ca^2+][CO3^2-]

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Magnesium Hydroxide Ksp

Mg(OH)2(s) ⇌ Mg^2+(aq) + 2OH^-(aq); Ksp = [Mg^2+][OH^-]^2

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Ca(OH)2 Molar Solubility

Using the balanced equation Ca(OH)2(s) ⇌ Ca^2+(aq) + 2OH^-(aq), the [Ca^2+] = X and [OH^-] = 2X, where X stands for molar solubility. Ksp = [Ca^2+][OH^-]^2 = [X][2X]^2 = 4X^3

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Study Notes

  • Solubility occurs when ionic compounds disperse in a solution due to ion-dipole interactions with water molecules.
  • Insoluble ionic compounds do not dissolve and remain solid, precipitating if their components meet in solution.
  • Even so-called "insoluble" compounds dissolve to a minuscule degree.
  • The solubility product, or Ksp, quantifies the degree of dissolution for a substance.
  • Ksp describes the dynamic equilibrium between dissolution and precipitation of ions.

Solubility Product (Ksp)

  • Ksp is the equilibrium constant for the dissolution of a solid substance into an aqueous solution.
  • The general formula of Ksp is the product of ion concentrations raised to the power of their stoichiometric coefficients in the balanced equilibrium equation.
  • For silver chloride (AgCl), the equilibrium is AgCl(s) ⇌ Ag+(aq) + Cl-(aq).
  • The Ksp expression is Ksp = [Ag+][Cl-].
  • Solids are not included in the Ksp expression.
  • Smaller Ksp values indicate lower ion concentrations and lower solubility.
  • Extremely water-insoluble compounds have Ksp values like 10^-30 or smaller.

Writing Solubility Products

  • Calcium carbonate (CaCO3) dissociates into Ca^2+ and CO3^2- ions: CaCO3(s) ⇌ Ca^2+(aq) + CO3^2-(aq).
  • Ksp for calcium carbonate is Ksp = [Ca^2+][CO3^2-].
  • Magnesium hydroxide (Mg(OH)2) dissociates into Mg^2+ and 2OH- ions: Mg(OH)2(s) ⇌ Mg^2+(aq) + 2OH-(aq).
  • Ksp for magnesium hydroxide is Ksp = [Mg^2+][OH^-]^2.
  • For apatite: Ksp = [Ca^2+]^5[PO4^3-]^3[OH^-].
  • Ionic compounds previously deemed insoluble are categorized as slightly soluble.

Calculating Ksp

  • Ksp can be experimentally determined by measuring ion concentrations in a saturated solution.
  • A saturated solution of magnesium hydroxide, or milk of magnesia, is used as an example.
  • Magnesium hydroxide dissolves according to: Mg(OH)2(s) ⇌ Mg^2+(aq) + 2OH-(aq).
  • If [Mg^2+] = 3.7 x 10^-6 M, then [OH^-] = 2 x 3.7 x 10^-6 M = 7.4 x 10^-6 M since there are two hydroxide ions for every magnesium ion.
  • Ksp = [Mg^2+][OH^-]^2 = (3.7 x 10^-6)(7.4 x 10^-6)^2 = 2.0 x 10^-13.
  • Ksp is a unitless constant.

Predicting Ion Concentrations

  • Given the Ksp value, the molar solubility of a substance can be predicted; this is the concentration of the dissolved solid in moles per liter.
  • Copper(I) bromide (CuBr) has a Ksp of 6.3 x 10^-9.
  • The equilibrium is CuBr(s) ⇌ Cu^+(aq) + Br-(aq).
  • Molar solubility is the moles per liter of the formula unit that will dissolve.
  • An ICE chart can be used to find molar solubility.
  • Ksp = [Cu^+][Br^-] = X^2, where X is the change in concentration of the ions and also equals the final concentration.
  • X = √(Ksp) = √(6.3 x 10^-9) = 7.9 x 10^-5 M, which is the molar solubility of copper(I) bromide.

Calculations with Exponents

  • Calcium hydroxide (Ca(OH)2) has a Ksp of 8.0 x 10^-6.
  • The equilibrium is Ca(OH)2(s) ⇌ Ca^2+(aq) + 2OH-(aq).
  • Ksp = [Ca^2+][OH^-]^2.
  • Using an ICE chart, [Ca^2+] = X and [OH^-] = 2X at equilibrium.
  • Ksp = (X)(2X)^2 = 4X^3.
  • X = ∛(Ksp/4) = ∛((8.0 x 10^-6)/4) = 1.3 x 10^-2 M, which is the molar solubility.
  • Molar solubility refers to the moles of solid that will dissolve per liter of water.

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