Ready for an electrifying challenge? Dive into our free electrochemistry test and discover how well you understand electrode potentials, conductance, and salt bridges. Whether you're gearing up for an important electrochemistry exam or simply curious, this quiz covers everything from the electrochemical series quiz basics to tougher electrode potential questions. You'll also explore the secrets of a perfect salt bridge quiz setup while sharpening your grasp of electrolysis and electrolytic cell mechanics with additional resources. Perfect for chemistry enthusiasts and students alike, this interactive quiz motivates you to push your limits. Start now and see if you can ace it!
What is the standard electrode potential E° for the standard hydrogen electrode?
0 V
+1.00 V
-0.34 V
+0.34 V
By international convention, the standard hydrogen electrode is assigned a potential of exactly zero volts under standard conditions. This serves as the reference point for all other electrode potentials. All other standard electrode potentials are measured relative to this reference. Learn more.
Which component of a galvanic cell maintains electrical neutrality by allowing the flow of ions?
Salt bridge
Voltmeter
Diaphragm
Cathode compartment
The salt bridge connects the two half-cells and allows ions to flow to maintain charge balance as the redox reaction proceeds. Without the salt bridge, charge buildup would quickly stop the cell reaction. It typically contains an inert electrolyte like KCl or KNO3. Learn more.
In a galvanic cell, reduction always occurs at which electrode?
Cathode
Anode
Salt bridge
Electrolyte
By definition, the cathode is the electrode where reduction (gain of electrons) occurs. Electrons flow toward the cathode through the external circuit. The anode is where oxidation (loss of electrons) takes place. Learn more.
What is the SI unit of electrical conductance?
Siemens (S)
Ohm (?)
Farad (F)
Henry (H)
Conductance is the reciprocal of resistance and is measured in siemens (S). One siemens equals one ampere per volt. The unit was formerly called the mho (ohm spelled backwards). Learn more.
Which of the following substances shows the highest conductance in aqueous solution at equal molar concentration?
HCl
NaCl
CH3OH
C6H12O6
HCl is a strong acid that fully dissociates into H? and Cl? ions, providing the greatest number of charge carriers per mole. NaCl also dissociates completely but has lower ionic mobility compared to HCl in water. Methanol and glucose are non-electrolytes, so they conduct poorly. Learn more.
In a Zn|Zn2+ || Cu2+|Cu cell, electrons flow from zinc to copper through the:
External conducting wire
Salt bridge
Electrolyte
Voltmeter
Electrons are transferred through the external circuit from the anode (zinc) to the cathode (copper). The salt bridge only allows ionic movement, not electrons. A voltmeter can measure the potential difference but electrons travel along the wire. Learn more.
Which ion migrates toward the anode through a typical salt bridge?
Anions
Cations
Neutral molecules
Electrons
As oxidation at the anode produces positive ions in solution, anions from the salt bridge migrate toward the anode compartment to neutralize the excess charge. Cations move toward the cathode. Electrons move through the external circuit, not the bridge. Learn more.
Under standard conditions, the concentration of all aqueous species is:
1 M
0.1 M
Saturated
0.01 M
Standard state for solutes in electrochemistry is defined as 1 molar concentration at 1 atm pressure and 25°C. This applies to all aqueous ions when reporting standard electrode potentials. Deviations require calculation via the Nernst equation. Learn more.
According to the Nernst equation, if the concentration of reactants decreases, what happens to the cell potential?
It decreases
It increases
It remains unchanged
It becomes negative
Lowering reactant concentrations shifts the reaction Q value higher, causing a decrease in cell potential according to the Nernst equation: E = E° – (RT/nF)lnQ. This reflects the reduced driving force for electron flow. Learn more.
Why does molar conductivity of an electrolyte increase upon dilution?
Reduced interionic interactions increase ion mobility
Viscosity of the solution increases
Number of ions decreases
Temperature drops
Dilution decreases interionic attractions, allowing ions to move more freely under an electric field, thereby increasing molar conductivity (?m = ?/C). Fewer interactions lead to higher mobility per mole of electrolyte. Learn more.
In the electrochemical series, a more positive standard electrode potential indicates a stronger:
Oxidizing agent
Reducing agent
Solvent
Electrolyte
A more positive E° value means the species has a greater tendency to gain electrons (be reduced), making its oxidized form a stronger oxidizing agent. The reverse is true for reducing agents. Learn more.
Which salt is most suitable for a salt bridge in a Cu–Zn galvanic cell?
KNO3
AgNO3
NaCl
KCl
KNO3 is preferred because NO3– is inert with respect to both Cu2+ and Zn2+. Cl– can form complexes or precipitates, and Ag+ would plate out on electrodes. KNO3 maintains ionic strength without side reactions. Learn more.
Which expression correctly relates conductance (G) to conductivity (?) for a uniform solution?
G = ?·A/L
G = ?·L/A
? = G·L/A
G = L/(?·A)
Conductance G depends on conductivity ?, cross-sectional area A, and distance between electrodes L: G = ?A/L. This shows that larger A or ? and smaller L increase conductance. Learn more.
In a concentration cell, the electromotive force depends on:
Ratio of ion concentrations in the two half-cells
Absolute pressures of gases
Electrode surface area
Salt bridge type
A concentration cell has identical electrodes and E° = 0, but a nonzero Ecell arises from a concentration gradient. The Nernst equation shows dependence on the concentration ratio. Learn more.
In the cell notation Fe3+ | Fe2+ || Cu2+ | Cu, what is the half-reaction at the anode?
Fe2+ ? Fe3+ + e–
Fe3+ + e– ? Fe2+
Cu ? Cu2+ + 2e–
Cu2+ + 2e– ? Cu
The anode reaction is oxidation: Fe2+ is oxidized to Fe3+ releasing an electron. The cathode reaction is Cu2+ gaining electrons to form Cu. Cell notation always lists the anode half-cell on the left. Learn more.
Why does the conductivity of an electrolyte solution decrease at lower temperature?
Ion mobility decreases due to higher viscosity
Ion concentration drops
Dielectric constant decreases
Ion charge changes
Lower temperature increases viscosity, slowing ion movement and reducing conductivity. Concentration remains the same, but mobility is temperature dependent. The dielectric constant effect is smaller. Learn more.
Calculate the standard EMF for the cell Zn | Zn2+ (1 M) || Ag+ (1 M) | Ag given E°(Ag+/Ag)=+0.80 V and E°(Zn2+/Zn)=–0.76 V.
1.56 V
0.04 V
1.00 V
1.76 V
Standard EMF is E°cathode – E°anode = 0.80 – (–0.76) = 1.56 V. Zinc is oxidized and silver is reduced under standard conditions. This formula applies when concentrations are 1 M and pressure is 1 atm. Learn more.
For the cell Pt | H2 (1 atm) | H+ (0.01 M) || Ag+ (1 M) | Ag at 298 K, calculate Ecell.
0.92 V
0.80 V
1.00 V
0.70 V
E°cell = E°Ag – E°H2 = 0.80 – 0.00 = 0.80 V. Using Nernst: E = 0.80 – (0.0592/2)log([H+]²/[Ag+]²) = 0.80 + 0.118 = 0.918 V ? 0.92 V. This reflects non?standard [H+]. Learn more.
Which mechanism explains rapid proton conduction in water?
Grotthuss mechanism
Frenkel defect
Debye–Hückel
Bridging conduction
Protons hop through a network of hydrogen-bonded water molecules in the Grotthuss mechanism, enabling high proton mobility. This jump?relay of protons is faster than physical diffusion. It is critical in acid conductance. Learn more.
In a lead-acid battery, the negative electrode undergoes which reaction during discharge?
Pb + SO4²– ? PbSO4 + 2e–
PbO2 + 4H+ + SO4²– + 2e– ? PbSO4 + 2H2O
Pb2+ + 2e– ? Pb
PbSO4 ? Pb + SO4²–
At the negative plate (anode) discharge, lead reacts with sulfate ions to form lead sulfate and releases electrons: Pb + SO4²– ? PbSO4 + 2e–. The positive plate uses PbO2. Learn more.
Which factor has the least effect on the limiting molar conductivity of an electrolyte?
Concentration
Ionic charge
Ionic radius
Temperature
Limiting molar conductivity (?m?) is measured at infinite dilution, so concentration effects are negligible. It mainly depends on ionic charge, size, and temperature through mobility. Learn more.
For a concentration cell Ag+ (0.001 M) | Ag || Ag+ (1 M) | Ag, what is Ecell at 298 K?
0.1776 V
0.0592 V
0.354 V
0 V
Ecell = (0.0592/n)·log([Ag+]high/[Ag+]low) = (0.0592/1)·log(1/0.001) = 0.0592·3 = 0.1776 V at 25 °C. A concentration gradient drives the potential. Learn more.
What is the major limitation of using conductance to determine electrolyte concentration at high ionic strength?
Nonlinear behavior due to interionic interactions
Viscosity changes become negligible
Temperature dependence disappears
Conductance becomes zero
At high ionic strength, ions interact strongly, deviating from ideality and causing nonlinear conductance-concentration relationships. Calibration curves become complex. Dilute solutions minimize these effects. Learn more.
Why is KCl often chosen as the electrolyte in a salt bridge for minimizing liquid junction potential?
K+ and Cl– have nearly equal ionic mobilities
KCl precipitates unwanted ions
KCl reacts with electrode metal
KCl is a weak electrolyte
Liquid junction potential arises from unequal ion mobilities at the interface. K+ and Cl– mobilities are almost the same, minimizing the potential difference. This makes KCl ideal for salt bridges. Learn more.
What effect does adding a common ion have on the electrode potential of a half-cell reaction according to Le Chatelier’s principle?
It shifts equilibrium, decreasing the potential
It increases the potential indefinitely
It has no effect under any condition
It makes the potential equal to standard immediately
Adding a common ion shifts the half?reaction equilibrium away from product formation, reducing the reaction quotient Q and lowering the electrode potential via the Nernst equation. This reflects Le Chatelier’s principle. Learn more.
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Study Outcomes
Interpret Electrochemical Series Trends -
After completing this electrochemical series quiz, readers will be able to read and interpret the ordering of species in the electrochemical series and identify their oxidation - reduction tendencies.
Analyze Standard Electrode Potentials -
Participants will learn to calculate, compare, and analyze standard electrode potentials, preparing them to tackle electrode potential questions with confidence.
Predict Redox Reaction Spontaneity -
Users will be able to determine the feasibility of redox reactions by applying Nernst equation principles and potential differences in an electrochemistry test context.
Evaluate Ionic Conductance -
Quiz takers will understand the factors influencing ionic conductance in electrolytic solutions, including ion mobility, concentration effects, and conductivity measurements.
Explain Salt Bridge Functionality -
Examine the role and design of salt bridges in galvanic cells, ensuring charge neutrality and maintaining circuit continuity as illustrated in this salt bridge quiz.
Apply Electrochemistry Concepts to Exam Questions -
Integrate core electrochemistry principles to answer complex MCQs, refine test-taking strategies, and boost performance on an electrochemistry exam.
Cheat Sheet
Understanding the Electrochemical Series -
Review the electrochemical series to rank metals by their standard reduction potentials (E°). A helpful mnemonic is "LEO the lion says GER" (Loss of Electrons is Oxidation, Gain of Electrons is Reduction). This ordering, as per IUPAC and NIST data, predicts spontaneous reactions in electrochemistry tests.
Calculating Standard Electrode Potentials -
Use E°cell = E°cathode - E°anode to determine overall cell potential under standard conditions (1 M, 25 °C). For example, combining a Cu2+/Cu electrode (E°=+0.34 V) with a Zn2+/Zn electrode (E°= - 0.76 V) yields E°cell = 1.10 V. Mastery of this formula is vital for any electrochemical series quiz question.
Role and Composition of Salt Bridges -
Salt bridges maintain charge balance by allowing ion flow between half-cells, preventing voltage collapse. Commonly filled with KCl or KNO3 gel to avoid interfering with electrode reactions, as recommended by university lab protocols. Understanding their function is crucial for designing galvanic cells in an electrochemistry exam.
Conductance vs. Conductivity -
Conductance (G) measures an electrolyte's ability to carry current (unit Siemens), while conductivity (κ) is an intrinsic property normalized to cell geometry. The relation G = κ·A/L (area A, length L) helps convert lab measurements into material properties, as outlined in analytical chemistry texts. Practice calculating κ from conductance data to ace salt bridge and conductance questions.
Applying the Nernst Equation -
The Nernst equation, E = E° - (RT/nF)·ln(Q), adjusts cell potential for nonstandard conditions; at 25 °C it simplifies to E = E° - (0.0592/n)·log(Q). Use this to predict how concentration changes shift electrode potentials in an electrochemistry test. Real-world examples include pH sensors and concentration cells in industry publications.
