ap_chem:acid_bases - wiki.epix.icu

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====== Acid and Bases ======
===== Acid =====
  * Acidic in taste
  * Acids disassociate one proton (H<sup>+</sup>) at a time
  * Types of acids: Monoprotic((1 H<sup>+</sup>)), Diprotic((2 H<sup>+</sup>)), and Polyprotic((many H<sup>+</sup>))
  * **Bronsted-Lowry Acids** are important and they donate H<sup>+</sup> in water

===== Base =====
  * Bitter/poisonous
  * Slippery when wet
  * Most cleaners are basic == **alkaline**
  * **Bronsted-Lowry Bases** are similar to their acid counterparts, they accept an H<sup>+</sup>

===== Strong vs Weak Acids and Bases =====
  * Strong acids/bases completely ionize or disassociate in water, weak ones do not
  * Less than 1% of a weak acid/base will dissociate

Note: Weak acids are extremely dangerous, HF on your skin will put amputation in your near future.

==== Strong Acids ====
  * HCl
  * HBr
  * HI
  * HlO<sub>4</sub>
  * H<sub>2</sub>SO<sub>4</sub>
  * HNO<sub>3</sub>

==== Strong Bases ====
All group I + II Hydroxides are strong bases((examples include LiOH, NaOH, Ca(OH)<sub>2</sub>, Ba(OH)<sub>2</sub>, etc.))

===== Amphiprotic =====
Also called Amphoteric, these are ions that behave as either acids or bases. Water is an example of one.

===== pH scale =====
pH is a logarithmic scale to measure the acidity of a solution. Acids are between 0-7, bases are 7-14, and an exact value of 7 represents a neutral substance.

==== Calculating pH (and pOH) ====
These equations can be used to calculate the pH of a substance. pOH is useful for determining the basicness of a solution.
  * $\text{pH} = -\log{H^+}$
  * $\text{pOH} = -\log{OH^-}$

Taking the inverse log(($10^x$ or $\log{x}^{-1}$)) can return the amount of H<sup>+</sup> and OH<sup>-</sup> as indicated by the formulas above.
  * $H^+ = 10^{-\text{pH}}$
  * $OH^- = 10^{-\text{pOH}}$

==== Relationship between pH and pOH ====
Since the pH scale goes between 0 and 14, $\text{pH} + \text{pOH} = 14$. Also, using the rules in the section above, it can also be determined that $H^+ \times OH^- = 1 \times 10^{-14}$. This all assumes that the temperature is **25 °C**. You can still use this if the temperature isn't stated.
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