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Questions and Answers
Which of the following ionic compounds has the following Ksp expression? Ksp = 4s³
Which of the following ionic compounds has the following Ksp expression? Ksp = 4s³
- CaCl₂ (correct)
- Fe(OH)₃
- I'm not sure
- AgBr
What is the solubility of CaCl₂ in a solution that contains 0.100 M Ca²⁺?
What is the solubility of CaCl₂ in a solution that contains 0.100 M Ca²⁺?
0.025 M
Predict the outcome (if any) when the following solutions are mixed together. Give a balanced chemical equation. Sodium bromide and lead nitrate.
Predict the outcome (if any) when the following solutions are mixed together. Give a balanced chemical equation. Sodium bromide and lead nitrate.
- PbBr₂ (s) precipitates, 2NaBr (aq) + Pb(NO₃)₂ (aq) ⟶ PbBr₂ (s) + 2NaNO₃ (aq) (correct)
- No reaction occurs
- Both PbBr₂ (s) and NaNO₃ (s) precipitate, 2NaBr (aq) + Pb(NO₃)₂ (aq) ⟶ PbBr₂ (s) + 2NaNO₃ (s)
- NaNO₃ (s) precipitates, 2NaBr(aq) + Pb(NO₃)₂ (aq) ⟶ NaNO₃ (s) + PbBr₂ (aq)
The solubility of a compound is always affected by pH.
The solubility of a compound is always affected by pH.
How many of the following compounds would be less soluble in a pH = 10.00 buffer than in pure water? PbCl₂, Ba(OH)₂, Hg₂I₂, CaF₂?
How many of the following compounds would be less soluble in a pH = 10.00 buffer than in pure water? PbCl₂, Ba(OH)₂, Hg₂I₂, CaF₂?
Flashcards
Solubility
Solubility
The amount of solute that dissolves per litre of saturated solution.
Saturated solution
Saturated solution
A solution where no more solute can dissolve at a given temperature.
Solubility (s)
Solubility (s)
The concentration of solute in a saturated solution; often expressed in mol/L
Ksp
Ksp
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Solubility of BaCrO4
Solubility of BaCrO4
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Solubility of Ag2CrO4
Solubility of Ag2CrO4
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Solubility Question Types
Solubility Question Types
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Exothermic crystallization
Exothermic crystallization
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Hand warmers
Hand warmers
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Study Notes
Introduction to Solubility
- Science knows no country, knowledge belongs to humanity.
- This was stated by Louis Pasteur.
Solubility
- Solubility is the amount of solute that dissolves per liter of saturated solution.
- Slightly soluble ionic compounds only dissolve partially in solution.
- An equilibrium is formed between the solid and ions.
Solubility Equilibrium
- Saturated solution has solubility.
- Using the values of ions to calculate equilibrium (Ksp)
Examples of Solubility Equilibria and Ksp Values
- A table of different solutes along with their solubility equilibrium reaction and Ksp value at 25°C is provided.
Solubility: Type 1 Example
- Consider PbCl₂ dissolving in water.
- Calculate Ksp if molar solubility is 0.00130 mol/L.
- This shows a calculation process for Ksp using molar solubility.
Solubility: Type 2 Example
- Consider Ag₂CrO₄ dissolving in water.
- Calculate molar solubility if Ksp is 1.1×10⁻¹².
- This shows a calculation process for molar solubility using Ksp.
Solubility: Practice
- Identify the ionic compound with Ksp = 4s3 from a list of options.
- Shows the calculations behind finding the correct answer.
Precipitation Reaction
- Precipitation reaction occurs when two aqueous salt solutions are mixed and a precipitate forms.
- It's not a true equilibrium.
Predicting Precipitation
- Ways to predict if a precipitate will form is by knowing the solubility of inorganic compounds.
- Two categories: soluble and sparingly (slightly) soluble.
Solubility Rules
- Table outlining soluble and insoluble ionic compounds, and important exceptions.
Solubility: Practice Question
- Predict the outcome when sodium bromide and lead nitrate solutions are mixed.
- Shows the balanced chemical equation.
- The rules are referred to for determining if the outcome is soluble or insoluble.
Solubility and Q
- Q has the same formula as Ksp.
- Values are initial concentrations.
- Solutions and their characteristics based on how Q relates to Ksp: unsaturated, saturated, and supersaturated.
Solubility: Practice
- Determine the minimum [Cl⁻] required to begin precipation of Hg₂Cl₂ given [Hg₂²⁺] is 0.010 M
Solubility: Example 1
- Calculate the minimum [Cl⁻] required to begin precipitation of Hg₂Cl₂ given [Hg₂²⁺] is 0.010 M
Solubility
- The exothermic crystallization of supersaturated sodium acetate solutions is the chemistry behind reusable hand warmers.
Solubility: Example 2
- Calculate molar solubility of PbCrO₄ in 0.100 M Na₂CrO₄ if Ksp = 2.8 x 10⁻¹³.
Solubility: Practice
- Improve the quality of X-ray photos by adding compounds to a BaSO₄ suspension to control the Ba²⁺ concentration since Ba²⁺ is toxic.
- Determining the best compound from a list.
Solubility
- pH can affect the solubility of some compounds.
- Consider the Co(OH)₂ equilibrium example.
Solubility: Practice
- Determine how many compounds in a list would be less soluble in a pH 10.00 buffer than in pure water.
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Description
This quiz covers the fundamental concepts of solubility, including the definition, the formation of saturated solutions, and the principles of solubility equilibrium. It includes calculations related to the solubility product constant (Ksp) as well as practical examples for better understanding.
