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Quizzes > Science > Chemistry

Ultimate Solubility Quiz: Test Your Chemistry Skills

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

Editorial: Review CompletedCreated By: Uvejs QelaUpdated Aug 25, 2025
Difficulty: Moderate
2-5mins
Learning OutcomesCheat Sheet
Paper art style flasks molecules text challenge yourself free solubility quiz chemistry skills fun dark blue background

This solubility quiz helps you practice solubility rules, predict what dissolves, and read solubility curves. Work through short questions on ionic compounds and precipitates, explore why substances dissolve , and try an AP Chemistry solubility warm-up . Get instant feedback so you can spot weak spots before a test or lab.

According to solubility rules, which compound is most likely soluble in water?
BaCO3
PbSO4
AgCl
NaNO3
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Sodium chloride dissolves in water primarily because the ion-dipole interactions overcome the lattice energy of the crystal.
True
False
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Which anion generally forms insoluble salts with most cations, except when paired with alkali metals or NH4+?
Carbonate (CO3 2-)
Nitrate (NO3-)
Acetate (CH3COO-)
Perchlorate (ClO4-)
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All chlorides are soluble in water without exception.
False
True
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Which compound is least soluble in water at room temperature based on common rules?
NaClO4
K2SO4
NH4Cl
CaCO3
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Which salt will increase the solubility of AgCl in water via complex ion formation?
KNO3
NH4NO3
NaCl
NH3(aq)
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Adding a common ion decreases the solubility of a sparingly soluble salt.
True
False
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Which has the highest molar solubility if their Ksp values are identical?
M2X (2:1 salt)
MX2 (1:2 salt)
MX (1:1 salt)
M2X3 (2:3 salt)
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Lead(II) iodide is more soluble in hot water than in cold water.
False
True
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Which solution will best precipitate CaCO3 from a saturated CaCO3 solution?
Add Na2CO3
Add distilled water
Add NH4Cl
Add sugar
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Which salt will precipitate first when [Ag+] is gradually increased in a solution containing equal [Cl-] and [Br-]? (Ksp AgCl=1.8e-10; AgBr=5.0e-13)
AgCl
AgBr
Both precipitate simultaneously
Neither will precipitate
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Which compound is more soluble in acidic solution due to carbonate protonation?
AgCl
PbI2
CaCO3
BaSO4
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Given Ksp(PbCl2) = 1.7e-5 at 25 C, what is the molar solubility s in pure water?
s = 1.2e-2 M
s = 2.6e-2 M
s = 4.3e-3 M
s = 1.6e-2 M
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A saturated solution of CaF2 has [Ca2+] = 2.1e-4 M. What is Ksp?
1.8e-11
3.7e-11
4.4e-8
2.1e-4
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A buffer solution always increases the solubility of any salt containing the conjugate base of the buffer acid.
True
False
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For a saturated solution of Ca3(PO4)2, the relationship between Ksp and molar solubility s is Ksp = 27s5.
True
False
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Salting out proteins relies on reduced water activity at high ionic strength, decreasing protein solubility.
False
True
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In qualitative analysis, H2S precipitates many Group II metal sulfides from acidic solution due to low Ksp values.
True
False
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The common ion effect can be analyzed quantitatively using the Henderson-Hasselbalch equation for acid-base equilibria influencing solubility of basic salts.
False
True
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Selective precipitation can separate Ag+, Pb2+, and Ca2+ using Cl-, SO4 2-, and CO3 2- in sequence.
False
True
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0

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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