https://www.khanacademy.org/science/ap-chemistry-beta/x2eef969c74e0d802:equilibrium/x2eef969c74e0d802:solubility-equilibria/v/solubility-and-the-common-ion-effect 2022-09-05T08:18:59.810508578Z The common-ion effect The solubility of an ionic compound is decreased by the presence of a common ion (an ion that is also present in the compound); this is known as the common-ion effect. Jay video https://cdn.kastatic.org/ka_thumbnails_cache/7dccf10c-0750-4411-8e6d-fc3e292f1ce4_1280_720_base.png The common-ion effect The solubility of an ionic compound is decreased by the presence of a common ion (an ion that is also present in the compound); this is known as the common-ion effect. https://cdn.kastatic.org/ka-youtube-converted/fI3U9T7LigY.mp4/fI3U9T7LigY.mp4 608 Ionization equilibria and acid–base strength https://www.khanacademy.org/science/chemistry/acids-and-bases-topic/buffer-solutions/v/common-ion-effect 2021-01-04T18:35:20Z Common ion effect and buffers The common ion effect describes the effect on ​equilibrium that occurs when a common ion (an ion that is already contained in the solution) is added to a solution. The common ion effect generally decreases ​solubility of a solute. It also can have an effect on buffering solutions, as adding more conjugate ions may shift the pH of the solution. video https://cdn.kastatic.org/googleusercontent/JLtnMUG5v029jKRIRxRDEq_HbeEGqHJ5toMTmYYfQcODJf4AHt9SWuUOH7vRZzhrEX9MBx6WbTpde9V6EaWcY8TB Common ion effect and buffers The common ion effect describes the effect on ​equilibrium that occurs when a common ion (an ion that is already contained in the solution) is added to a solution. The common ion effect generally decreases ​solubility of a solute. It also can have an effect on buffering solutions, as adding more conjugate ions may shift the pH of the solution. https://cdn.kastatic.org/ka-youtube-converted/223KLPnJCBI.mp4/223KLPnJCBI.mp4 799 Ionization equilibria and acid–base strength https://www.khanacademy.org/science/chemistry/acids-and-bases-topic/copy-of-acid-base-equilibria/v/ka-and-acid-strength 2021-01-04T18:35:18Z Ka and acid strength How to write an equilibrium expression for an acid-base reaction and how to evaluate the strength of an acid using Ka video https://cdn.kastatic.org/googleusercontent/0w5OdvzBpJEgiioYkA2Ba_FaVaeLW-5dw4XjmK4oUU2bLvwwRA4dXF3nWZ3JLQPYh-qyCo1D1joNMldmkugmonlE Ka and acid strength How to write an equilibrium expression for an acid-base reaction and how to evaluate the strength of an acid using Ka https://cdn.kastatic.org/ka-youtube-converted/BeHOvYchtBg.mp4/BeHOvYchtBg.mp4 558 Ionization equilibria and acid–base strength https://www.khanacademy.org/science/ap-chemistry-beta/x2eef969c74e0d802:acids-and-bases/x2eef969c74e0d802:weak-acid-and-base-equilibria/v/weak-base-equilibria 2022-10-05T02:43:18.611402953Z Weak base equilibria Weak bases partially ionize in water to produce hydroxide ions. Because the ionization is not complete, the concentration of OH⁻ in a weak base solution is typically much less than the initial base concentration. The relative strength of a weak base is described by the base ionization constant, Kb, which is the equilibrium constant for the reaction of the weak base with water. Jay video https://cdn.kastatic.org/ka_thumbnails_cache/8fe22b44-8464-4a1b-a336-2aa8c81c7b80_1280_720_base.png Weak base equilibria Weak bases partially ionize in water to produce hydroxide ions. Because the ionization is not complete, the concentration of OH⁻ in a weak base solution is typically much less than the initial base concentration. The relative strength of a weak base is described by the base ionization constant, Kb, which is the equilibrium constant for the reaction of the weak base with water. https://cdn.kastatic.org/ka-youtube-converted/cvcgH3ohcNg.mp4/cvcgH3ohcNg.mp4 570 Ionization equilibria and acid–base strength https://www.khanacademy.org/science/grade-11-chemistry-snc-aligned/x203b0fc81a964b2d:acid-base-chemistry/x203b0fc81a964b2d:solubility-equilibria/a/weak-acid-base-equilibria 2021-04-29T07:49:41Z Weak acid-base equilibria Weak acid and base ionization reactions and the related equilibrium constants,  Ka and Kb. Relating Ka and Kb to pH, and calculating percent dissociation.  article