CHEMDUNN

This episode explores molecular polarity, explaining how electronegativity differences create polar bonds and why molecular geometry determines overall polarity. The hosts distinguish between bond polarity and molecular...

Faraday's Law relates the amount of chemical change in an electrolytic cell to the total electric charge passed through it. The amount of product is directly proportional to the charge. Using Faraday's constant (96,485...

Electrolysis uses electrical energy to drive a nonspontaneous redox reaction, the opposite of a voltaic cell. An electrolytic cell requires a power source, where the anode is positive and the cathode is negative...

This episode explains how to calculate non-standard cell potentials (voltage) using the Nernst equation. Real-life batteries operate under non-standard conditions where concentrations change, causing voltage to drop...

The standard cell potential (E°cell) for a voltaic cell is calculated using E°cell = E°cathode − E°anode, where E° values come from standard reduction potential tables. A positive E°cell indicates a spontaneous reaction...

Voltaic (or Galvanic) cells convert chemical energy into electrical energy using a spontaneous redox reaction. The reaction is split into two half-cells: the anode (where oxidation occurs) and the cathode (where...

To balance redox reactions, they are split into oxidation and reduction half-reactions. The goal is to conserve both mass and charge. In acidic solutions, H2O balances oxygen, and H+ balances hydrogen. In basic...

Redox (Oxidation-Reduction) reactions involve the transfer of electrons. Oxidation is the loss of electrons (LEO), and Reduction is the gain of electrons (GER). These processes always occur simultaneously. Oxidation...

Gibbs Free Energy (ΔG) predicts reaction spontaneity using the equation: ΔG = ΔH - TΔS. A negative ΔG means the reaction is spontaneous (happens on its own). This value combines enthalpy (ΔH), which is heat change, and...

This episode defines entropy (S) as a measure of the disorder or the number of ways energy and matter can be arranged in a system. Entropy naturally increases when a substance changes phase from solid to liquid to gas...

This episode explains that not all salts are neutral; their pH depends on the origin of their ions. A salt is formed from an acid-base neutralization reaction. When dissolved, ions from weak acids or weak bases can...

Indicators are weak acids or bases that change color based on the solution's pH. The color change happens because the indicator exists in an equilibrium between two forms, each having a different color. The goal is to...

This episode introduces titration, a technique used to determine an unknown concentration (analyte) using a solution of known concentration (titrant). The focus is the strong acid–strong base titration, where reactants...

A buffer is a solution that resists changes in pH when small amounts of acid or base are added. It must contain a weak acid and its conjugate base (or a weak base and its conjugate acid). When acid (H+) is added, the...

Weak acids and bases partially dissociate in water, establishing equilibrium. Their strength is measured by the acid dissociation constant (Ka) and the base dissociation constant (Kb). A larger Ka or Kb indicates a...