Acids & Bases

Arrhenius

Acid - When ionized produces $H^+$ ions; specifically, acids increase the concentration of $H^+$ ions in aqueous solutions.
Base - When ionized produces $OH^-$ ions; bases increase the concentration of $OH^-$ ions in aqueous solutions.
- Basic solutions are called alkaline.

Bronsted-Lowry

Acid - Donates protons ( $H^+$ ions); a substance that acts as a proton donor.
Base - Accepts protons; a substance that acts as a proton acceptor.
Conjugate Base - What remains after an acid has donated its proton; it is the species formed after an acid loses a proton.
Conjugate Acid - What remains after a base has accepted a proton; it is the species formed when a base gains a proton.
- Sometimes use $H_3O^+$ , called hydronium ion, instead of $H^+$ .
- Protons are highly reactive, so in the presence of water protons will combine with the water to make $H_3O^+$ .

Acids

Taste sour; although tasting acids is dangerous and not recommended.
React with metals to make hydrogen gas; this is due to the acid corroding the metal.
Conduct Electricity; acids are electrolytes, which means they conduct electricity in aqueous solutions.
Neutralizes bases; acids react with bases in a neutralization reaction to form water and a salt.
Turns litmus and universal indicator red; litmus paper turns red in the presence of an acid, and universal indicator shows a red to yellow color.

Bases

Taste bitter; tasting bases is dangerous and not recommended.
Feel slippery; bases feel soapy to the touch.
Conduct electricity; like acids, bases are electrolytes and conduct electricity in aqueous solutions.
Neutralizes acids; bases react with acids in a neutralization reaction to form water and a salt.
Turns litmus and universal indicator blue; litmus paper turns blue in the presence of a base, and universal indicator shows a blue to violet color.

Other

Acid and base come into contact and neutralize to produce water and salt.
- Neutralization reaction
Salts are ionic compounds (made of a metal and nonmetal).
- Formed when metal transfers electrons to nonmetal; the metal loses electrons and becomes a cation (positive).
- The nonmetal gains electrons and becomes an anion (negative).
- Acids start with one or more Hydrogen Ions

Naming

Strong and Weak Acids and Bases

What makes an acid or base strong or weak is the amoung that it ionizes.
A strong acid or base will ionize completely (all of the acid or base will produce ions)
A weak acid or base will only ionize slightly.
The six strong acids are HCl, HBr, HI, HNO3, H2SO4, HClO4
- Hydrochloric acid, Hydrobromic Acid, Hydroiodic Acid, Nitric Acid, Sulfuric Acid, Perchloric Acid
  - CluB rhiNO3 Is SO4 ClO4se
Strong bases include LiOh, NaOH, KOH, RBOH, and CSOH
- Ca(OH)2, Sr(OH)2, and Ba(OH)2
Molarity is used to determine if asn acid or base is concentrated or dilute; it is defined as the number of moles of solute per liter of solution. A higher molarity indicates a more concentrated solution, while a lower molarity signifies a dilute solution.

Titration Calculations

n = M V
Short cut: $\frac{MaVa}{Ca}=\frac{MaVa}{Ca}$
- C is the coefficient of the substance
- Ex: $\frac{\left(Ma\right)\left(60.0mL\right)}{\left(1\right)}=\frac{\left(0.200M\right)\left(30.0mL\right)}{\left(1\right)}$

Buffers

A buffer is a solution that will resist a change in pH
- By containing a weak conjugate acid-base pair
If you add an acid to a buffer, the base will neutralize it.
If you add a base, the acid will neutralize it.

Self Ionization of OH

Neutral means [H] = [OH]
Acid means [H] > [OH]
Base means [H] < [OH]
pH Scale Calculations
- $pH=-\log_{10}\left\lbrack H^{+}\right\rbrack$
- $pOH=-\log_{10}\left\lbrack OH^{-}\right\rbrack$
- $Kw=\left\lbrack H^{+}\right\rbrack\left\lbrack OH^{-}\right\rbrack=1.00\cdot10^{-14}$
- $14.00=pH+pOH$