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Strong vs Weak Electrolytes Quiz - Can You Ace It?

Ready for electrolyte practice problems? Take the strong vs weak electrolytes test!

Difficulty: Moderate
2-5mins
Learning OutcomesCheat Sheet
Paper art illustration with lab glassware ions and compounds showing strong vs weak electrolytes on teal background

This strong vs weak electrolytes quiz helps you practice sorting substances as strong, weak, or nonelectrolytes. You'll work through short, quick, exam-style questions, check your mistakes, and lock in the rules so you're ready for class, labs, or the exam.

What defines a strong electrolyte in an aqueous solution?
It completely ionizes in water
It does not ionize in water
It only ionizes when molten
It partially ionizes in water
A strong electrolyte is defined by its complete ionization in water, producing maximum ions that can conduct electrical current. Unlike weak electrolytes, they dissociate fully into ions. This behavior leads to high conductance in solution.
Which of the following is a strong electrolyte?
CH3CH2OH
NH3
NaOH
C6H12O6
NaOH is a strong base that dissociates completely into Na+ and OH - ions in aqueous solution, making it a strong electrolyte. Organic molecules like ethanol and ammonia only partially ionize. Glucose doesn't ionize and is a non-electrolyte.
Which substance is a nonelectrolyte in water?
NaCl
Glucose (C6H12O6)
HCl
KOH
Glucose dissolves in water without forming ions, so it does not conduct electricity and is a nonelectrolyte. In contrast, HCl, KOH, and NaCl dissociate into ions and conduct electricity.
Acetic acid (CH3COOH) in water is best classified as:
Weak electrolyte
Strong electrolyte
Precipitate
Nonelectrolyte
Acetic acid is a weak acid that partially ionizes in water, producing a limited number of ions. Therefore, it's classified as a weak electrolyte. It does not fully dissociate like strong electrolytes.
Which 0.1 M aqueous solution would exhibit the highest electrical conductivity?
NaCl
C6H12O6
CH3COOH
HCl
0.1 M HCl is a strong acid that fully ionizes into H+ and Cl? ions, and H+ has very high mobility, giving it higher conductivity than NaCl. CH3COOH is a weak electrolyte, and glucose is a nonelectrolyte.
Approximately what is the pH of a 0.01 M acetic acid solution (Ka ?1.8×10??)?
~5
~3
~7
~2
Using the approximation pH ?½(pKa ? log?C), where pKa?4.74 and C=0.01 M, the result is around 3. A more precise calculation yields ~2.9, which rounds to 3.
Why does a 0.1 M acetic acid solution conduct electricity weakly?
It partially ionizes in water
Water's dielectric constant is low
It forms covalent bonds
It has high viscosity
Acetic acid is a weak acid that does not fully dissociate in water, resulting in fewer ions to conduct electricity. Viscosity and dielectric constant are not primary factors in this context.
Which compound is considered a weak base in aqueous solution?
NaOH
NH3
KOH
LiOH
Ammonia (NH3) partially ionizes to NH4+ and OH? in water, making it a weak base. Group 1 hydroxides like NaOH fully dissociate, classifying them as strong bases.
Hydrofluoric acid (HF) in water is classified as:
Strong electrolyte
Nonelectrolyte
Weak electrolyte
Precipitate
HF is a weak acid with a Ka?6.8×10??, meaning it only partially dissociates in water and conducts electricity weakly. This partial ionization is characteristic of weak electrolytes.
Which statement correctly describes the acid dissociation behavior of H2SO4?
First dissociation is strong; second is weak
It does not dissociate
Both dissociations are weak
Both dissociations are strong
Sulfuric acid's first proton dissociates completely (strong electrolyte), but the second dissociation has a Ka?1.2×10?² and does not fully ionize, making it a weak electrolyte for the second step.
If equal volumes of 0.1 M HCl and 0.1 M acetic acid are compared for conductivity, which is higher and why?
They conduct equally
Acetic acid, because it has higher molecular weight
HCl, because it fully ionizes
Acetic acid, because it forms multiple ions
HCl is a strong electrolyte that fully dissociates into H+ and Cl? ions, whereas acetic acid is a weak electrolyte with limited ionization. Therefore, the HCl solution shows higher conductivity.
What is the approximate degree of ionization for a 0.05 M benzoic acid solution (Ka = 6.3×10??)?
0.36%
80%
3.6%
36%
Using ???(Ka/C), ???(6.3×10??/0.05)=?(0.00126)=0.0355 or 3.55%. This small degree reflects benzoic acid's character as a weak electrolyte.
Which amphiprotic species in aqueous solution can act as a weak electrolyte by both donating and accepting protons?
Cl?
HCO??
SO?²?
Na?
Bicarbonate (HCO??) can both donate a proton (forming CO?²?) and accept a proton (forming H?CO?), partially ionizing in each reaction. This amphiprotic behavior leads to weak electrolyte properties.
How does molar conductivity at infinite dilution (??) change with dilution for strong vs weak electrolytes?
Both ?? decrease
Strong electrolytes: ?? decreases; weak electrolytes: ?? increases
Strong: ?? increases; weak: ?? decreases
Both ?? increase
Strong electrolytes exhibit decreasing molar conductivity with dilution due to reduced ionic interactions, while weak electrolytes show increasing ?? as dilution shifts the ionization equilibrium toward more ions. These trends follow Kohlrausch's laws.
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Study Outcomes

  1. Define Strong vs Weak Electrolytes -

    Understand the fundamental differences in ionization and dissociation that distinguish strong electrolytes from weak electrolytes in aqueous solutions.

  2. Classify Electrolyte Strength -

    Analyze the molecular and ionic structures of compounds to accurately classify them as strong or weak electrolytes.

  3. Predict Conductivity Behavior -

    Apply principles of electrolyte dissociation to predict how solution concentration and ion mobility influence electrical conductivity.

  4. Interpret Common Electrolyte Lists -

    Use a curated list of strong and weak electrolytes to quickly identify and recall the strength of familiar acids, bases, and salts.

  5. Solve Electrolyte Practice Problems -

    Reinforce your understanding by working through targeted quiz questions, enhancing your ability to determine electrolyte strength under various conditions.

Cheat Sheet

  1. Complete vs Partial Dissociation -

    Strong vs weak electrolytes differ by the extent of ionization in water: strong electrolytes like NaCl or HCl dissociate nearly 100% into ions, whereas weak electrolytes such as acetic acid (CH₃COOH) only partially ionize (typically 1 - 10%). A quick mnemonic is "ALL or SOME": strong electrolytes are ALL-ionized; weak ones only SOME. Recall the general acid dissociation equation HA ⇌ H❺ + A❻ and associated Ka value to quantify ionization.

  2. Common Strong Electrolytes List -

    Familiarize yourself with key strong electrolytes: all soluble salts of Group 1 metals (e.g., NaCl, KNO₃), nitrates (NO₃❻), and perchlorates (ClO₄❻), plus strong acids (HCl, HNO₃, H₂SO₄) and strong bases (NaOH, KOH). A reliable strong and weak electrolytes list from your university's chemistry department can cement this knowledge. These compounds serve as benchmarks in electrolyte practice problems to test conductivity predictions.

  3. Characteristics of Weak Electrolytes -

    Weak electrolytes like HF, NH₃, and CH₃COOH have low dissociation constants (Ka or Kb typically <10❻³), so they establish equilibrium with significant amounts of undissociated molecules. In weak vs strong electrolytes comparisons, note that lower Ka values indicate weaker ionizers, leading to reduced conductivity. Practice by writing equilibrium expressions and predicting direction shifts when concentration or temperature changes.

  4. Percent Dissociation & ICE Tables -

    To quantify weak electrolyte strength, use percent dissociation = (amount dissociated/initial concentration)×100%, which is often approximated with an ICE table under the assumption x≪C₀. For example, solving CH₃COOH ⇌ H❺ + CH₃COO❻ with Ka=1.8×10❻❵ and initial C₀=0.1 M gives x≈√(Ka·C₀). Regularly solving these electrolyte practice problems builds intuition on when to apply approximations.

  5. Conductivity & pH Measurements -

    Electrical conductivity and pH directly reflect electrolyte strength: strong electrolytes yield high conductivity and pH extremes for acids/bases, while weak ones produce lower conductivity and intermediate pH values. A simple lab exercise uses a conductivity meter and pH probe to compare equal concentrations of HCl vs CH₃COOH, demonstrating real-time differences. Consistent practice interpreting these measurements sharpens your mastery of electrolyte concepts.

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