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Quizzes > Science > Chemistry

Ultimate Solubility Quiz: Test Your Chemistry Skills

Ready to ace the solubility rules quiz? Start testing now!

Difficulty: Moderate
2-5mins
Learning OutcomesCheat Sheet
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Ready to become a solubility pro? Dive into our free solubility quiz and challenge your chemistry skills! This interactive chemistry solubility quiz covers solubility rules trivia, from predicting which substances dissolve to analyzing solubility curves. Whether you're brushing up on ap chem solubility rules or eager to test solubility knowledge, you'll sharpen your understanding of ionic compounds and aqueous solutions. Perfect for curious students, this solubility rules quiz delivers instant feedback and clear explanations. Explore substances dissolve and compare in our ap chem solubility rules challenge. Are you ready? Start now!

Salts containing which of the following anions are almost always soluble in water?
Phosphate (PO?³?)
Carbonate (CO?²?)
Oxide (O²?)
Nitrate (NO??)
According to standard solubility rules, all nitrate salts are soluble regardless of the cation. This is because the nitrate ion does not form strong lattice forces in the solid that water cannot overcome. Other polyatomic ions like carbonate and phosphate are generally insoluble except with alkali metals or ammonium. Chemguide Solubility Rules
Most salts of Group 1 alkali metals (like sodium and potassium) are:
Insoluble
Very soluble
Moderately soluble
Sparingly soluble
Group 1 metal salts are highly soluble because their lattice energies are low and water stabilizes the ions well. This applies to compounds such as NaCl, KNO?, and Li?SO?. As a result, you will always find these salts fully dissolved in aqueous solution under normal conditions. LibreTexts: Solubility Rules
Which of the following chlorides is insoluble and will precipitate out of aqueous solution?
AgCl
NaCl
MgCl?
KCl
Silver chloride is one of the common exceptions among chlorides: it is poorly soluble in water and forms a white precipitate. In contrast, alkali metal and most alkaline earth metal chlorides are soluble. This follows the solubility rules for halide salts. Chemguide on Silver Halides
Which of the following sulfate salts is essentially insoluble in water?
BaSO?
NH?SO?
K?SO?
Na?SO?
Barium sulfate is known to be virtually insoluble due to its very low solubility product constant (Ksp). It is widely used in analytical chemistry as a precipitating agent. Other sulfates like those of sodium, potassium, and ammonium are fully soluble. Chemguide Sulfate Solubility
Given Ksp of PbCl? is 1.7×10?? at 25 °C, what is the molar solubility (s) of PbCl? in pure water?
0.003 M
0.014 M
0.027 M
0.10 M
For PbCl?, Ksp = [Pb²?][Cl?]² = s·(2s)² = 4s³. Solving 4s³ = 1.7×10?? gives s ? 0.014 M. This calculation uses the stoichiometry of the dissolution equilibrium. LibreTexts: Solubility Product
When equal volumes of 0.10 M BaCl? and 0.10 M Na?SO? are mixed, which compound precipitates?
Na?SO?
BaSO?
BaCl?
NaCl
Mixing Ba²? and SO?²? leads to formation of BaSO?, which is insoluble (Ksp ? 1.1×10?¹?). Other products remain soluble. The ionic product exceeds Ksp, causing BaSO? to precipitate. Chemguide Sulfate Solubility
Which of the following is considered a sparingly soluble salt?
NH?Cl
K?SO?
LiNO?
Ag?CrO?
Silver chromate has a low solubility product (Ksp ? 1.1×10?¹²), making it sparingly soluble. In contrast, alkali metal salts and ammonium salts are generally quite soluble. This is why Ag?CrO? often appears as a bright red precipitate. LibreTexts: Solubility Products
Carbonate salts are generally insoluble except those containing which of the following cations?
Lead (Pb²?)
Iron (Fe³?)
Sodium (Na?)
Calcium (Ca²?)
Most carbonates are insoluble except those of Group 1 metals (e.g., Na?, K?) and ammonium. Sodium carbonate dissolves readily in water, whereas carbonates of alkaline earth or transition metals do not. This follows the general solubility rules for carbonates. Chemguide Carbonate Solubility
Which condition will increase the solubility of CaCO? in water?
Adding more CaCl?
Removing CO? from the atmosphere
Lowering the pH of the solution
Increasing the pH of the solution
Acidic conditions convert CO?²? to HCO?? or H?CO?, shifting the dissolution equilibrium forward and dissolving more CaCO?. Raising pH or adding Ca²? drives precipitation instead. Removing CO? has little effect on solubility unless it's part of the carbonate buffering. LibreTexts: Carbonate Equilibria
What happens to the solubility of CaF? when HCl is added to a saturated solution?
Solubility decreases
Solubility increases
Solubility remains unchanged
Initially decreases then increases
Introducing H? shifts the equilibrium by reacting with F? to form HF, reducing free fluoride ions. This drives more CaF? to dissolve to reestablish equilibrium, thus increasing solubility. LibreTexts: Common Ion and pH Effects
A solution contains 0.01 M Ag? and 0.05 M Br?. Given Ksp(AgBr) = 5×10?¹³, will AgBr precipitate?
Yes, Qsp > Ksp
No, Qsp < Ksp
No, Qsp = Ksp
Cannot determine without pH
The reaction quotient Qsp = [Ag?][Br?] = 0.01×0.05 = 5×10??, which is much larger than Ksp (5×10?¹³). Because Qsp > Ksp, precipitation will occur until equilibrium is reestablished. LibreTexts: Solubility Product Concepts
Given Ksp of Ca(OH)? is 5.02×10?? at 25 °C, what is its molar solubility in pure water?
0.0050 M
0.0160 M
0.0107 M
0.0204 M
For Ca(OH)?, Ksp = [Ca²?][OH?]² = s·(2s)² = 4s³. Solving 4s³ = 5.02×10?? yields s ? 0.0107 M. This calculation uses the stoichiometric release of two hydroxide ions per formula unit. LibreTexts: Solubility Product Calculations
In a highly basic solution (pH 14), sulfide ions are added to a Ni²?/Co²? mixture. Which metal sulfide precipitates first?
CoS
NiS
Neither precipitates
Both precipitate simultaneously
Cobalt sulfide has a lower Ksp (?1×10?²³) than nickel sulfide (?3×10?²¹), so CoS reaches its solubility limit first and precipitates before NiS under identical conditions. This principle underlies selective precipitation separation. LibreTexts: Selective Precipitation
How does the addition of excess NH? affect the solubility of AgCl in water?
Solubility increases due to complex formation
Precipitation of AgOH occurs
No change
Solubility decreases due to common ion effect
Ammonia forms the complex ion [Ag(NH?)?]?, reducing free Ag? concentration and driving more AgCl to dissolve. This increases overall solubility despite the common ion effect on Cl?. Complex formation can dramatically shift equilibria. Chemguide on Complex Ion Formation
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Study Outcomes

  1. Understand fundamental solubility principles -

    Explain how solubility is governed by molecular interactions and thermodynamics, laying a strong foundation for success in the solubility rules quiz.

  2. Apply solubility rules to predict precipitation -

    Use standard solubility guidelines to accurately forecast which ionic compounds will precipitate when solutions are mixed in the solubility quiz scenarios.

  3. Analyze solute - solvent interactions -

    Identify and evaluate interactions like hydrogen bonding and ionic attraction to determine factors that enhance or inhibit compound solubility.

  4. Differentiate between soluble and insoluble compounds -

    Classify salts and compounds based on recognized solubility criteria, improving accuracy in your chemistry solubility quiz results.

  5. Recall key exceptions in solubility rules -

    Memorize common exceptions to general solubility guidelines to avoid pitfalls when tackling solubility rules trivia.

  6. Evaluate quiz performance to reinforce learning -

    Review your solubility quiz results to identify strengths and gaps, helping you test solubility knowledge and focus further study.

Cheat Sheet

  1. Fundamental Solubility Rules -

    Learn that nitrates (NO₃❻), alkali metals, and ammonium (NH₄❺) are always soluble, while halides (Cl❻, Br❻, I❻) are generally soluble except with Pb²❺, Hg₂²❺, and Ag❺. Use the mnemonic "PMS" (Lead's Plaster, Mercury's Mirror, Silver's Shield) to recall these key exceptions in your solubility rules quiz.

  2. Temperature Dependence of Solubility -

    Most solid solutes become more soluble as temperature rises, whereas gases like O₂ and CO₂ decrease in solubility with warming. For example, KNO₃'s solubility nearly doubles from 13 g/100 mL at 0 °C to 245 g/100 mL at 100 °C, a useful trend to remember for precipitation predictions.

  3. Solubility Product Constant (Ksp) -

    The Ksp expression, Ksp = [M❿❺]^a[X^m❻]^b for a salt M_aX_b, quantifies saturation; e.g., AgCl has Ksp = [Ag❺][Cl❻] = 1.8×10❻¹❰. Practice calculating molar solubility and precipitate formation to sharpen your chemistry solubility quiz skills.

  4. Common Ion Effect -

    Introducing a common ion shifts the dissolution equilibrium via Le Châtelier's principle and lowers solubility; for instance, adding NaCl reduces AgCl's dissolution in water. Understanding this effect is crucial when tackling mixed”ion problems in a solubility quiz.

  5. "Like Dissolves Like" Principle -

    Polar solvents dissolve polar solutes through dipole - dipole and hydrogen bonds, while nonpolar solvents favor nonpolar solutes via dispersion forces. Remembering "like dissolves like" helps you quickly predict solubility outcomes in every chemistry solubility quiz scenario.

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