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Chapter 14a: Acids & Bases - Coggle Diagram
Chapter 14a: Acids & Bases
Strong Acids
Hydrochloric Acid (HCl)
Perchloric Acid (HClO4)
Hydroiodic Acid (HI)
Hydrobromic Acid (HBr)
Sulfuric Acid (H2SO4)
Nitric Acid (HNO3)
Strong Bases
Lithium Hydroxide (LiOH)
Sodium Hydroxide (NaOH)
Potassium Hydroxide (KOH)
Caesium Hydroxide (CsOH)
Rubidium Hydroxide (RbOH)
Calcium Hydroxide Ca(OH)2
Barium Hydroxide Ba(OH)2
Strontium Hydroxide Sr(OH)2
Acid-Base Definitions
Arrhenius
Acid: produces H+ ions in solution
Base: Produces OH- ions in solution
Bronsted-Lowry
Acid: proton donor (H+)
Base: proton acceptor (H+)
Conjugates
a compound on the product side of the equilibrium equation that was formed by the reactant side of the equilibrium equation
Each acid in the reactants has a conjugate base
Each base in the reactants has a conjugate acid
Amphoteric
A substances that can act as both an acid and a base
When a substance has a H to donate and a place to put another H at the same time
Lewis
Acid: electron pair acceptor
Base: Electron pair donor
pH
On a logrithmic scale
[H+] and [OH-] ions determine the acidity and pH of solution
6.5 or lower is acidic
6.5-7.5 is neutral (water)
7.5 and up is basic
pH + pOH = 14
Kw= pH + pOH
pH= -log[H+]
pOH= -log[OH-]
Can use pH to find concentration
10^ -pH = [H+}
10^ -pOH = [OH-]
pH of strong acids and strong bases are full arrow dissociations
Weak Acids
Ka values tells us the relative strength of the weak acid
the higher the Ka value the stronger the acid because it has a higher [H+}
Polyprotic Acids
acids with multiple protons
only one H+ moves at a time
there are successive ionziations happening, which means they are all happening at once, but each ionization has their own Ka and pH