Chapter 15
Acids and Bases
By Boundless
![Thumbnail](../../../../../figures.boundless-cdn.com/9286/square/zn-reaction-with-hcl.jpeg)
Acids and bases will neutralize one another to form liquid water and a salt.
An Arrhenius acid dissociates in water to form hydrogen ions, while an Arrhenius base dissociates in water to form hydroxide ions.
A Brønsted-Lowry acid is any species capable of donating a proton; a Brønsted-Lowry base is any species capable of accepting a proton.
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Water is capable of acting as either an acid or a base and can undergo self-ionization.
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The acid dissociation constant (Ka) is the measure of the strength of an acid in solution.
![Thumbnail](../../../../../figures.boundless-cdn.com/30770/raw/phscalenolang.jpg)
A p-scale is a negative logarithmic scale.
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In water, strong acids completely dissociate into free protons and their conjugate base.
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A weak acid only partially dissociates in solution.
Percent dissociation represents an acid's strength and can be calculated using the Ka value and the solution's pH.
![Thumbnail](../../../../../figures.boundless-cdn.com/13135/square/sodium-hydroxide.jpeg)
Strong bases either dissociate completely in solution to yield hydroxide ions, or deprotonate water to yield hydroxide ions.
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In aqueous solution, a weak base reacts incompletely with water to yield hydroxide ions.
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The base dissociation constant (Kb) measures a base's relative strength.
![Thumbnail](../../../../../figures.boundless-cdn.com/30122/square/sodium_bicarbonate_(1).jpg)
When dissolved in water, a basic salt yields a solution with pH greater than 7.0.
![Thumbnail](../../../../../figures.boundless-cdn.com/30123/square/aniliniumchloride.jpg)
When dissolved in water, acidic salts form solutions with pH less than 7.0.
Some salts, such as ammonium bicarbonate (NH4HCO3), contain cations and anions that can both undergo hydrolysis.