Chemistry Flashcards
Strong acids List
HCl (aq), HBr (aq), HI (aq) ((Monoprotic acid) H2SO4 (Diprotic acid) HNO3 HClO4 (perchloric acid) HClO3 (chloric acid)
Strong bases list
all group 1 & 2 metal hydroxides except Mg(OH)2) NaOH KOH Ca(OH)2 Ba(OH)2
Moderately strong acid
H3PO4 (Triprotic acid)
Weak Acids List
Usually derived from “Carbon” Acids: CH3COOH Acetic Acid (HAc), CH2O2 formic acid, acetylsalicylic acid (aspirin), protonated bases (drugs)), H2CO3
Weak Bases List
NH3
transition metals form weak bases such as Ni(OH)2, Fe(OH)2, Fe(OH)3, Cu(OH)2. Mg(OH)2
Arrhenius Definition of Acids/Bases
Acid: Any substance that when put in wate will increase the hydronium ion (H3O+) concentration.
Base: Any substance that when put in water will increase the hydoxide ion (OH-) concentration.
Bronsted-Lowry Acid Base Theory
Acid: Any compound that can donate a proton in a proton transfe reaction.
Base: Any compound that can accept a proton in a proton transfer reaction.
Lewis Acid Base Theory
Acid: An elelectron pair acceptor (usually metals)
Base: An electron pair donor
Avogadro’s Number
6.022x10^23 (# of particles in a mole)
Molar Mass
(Grams of a substance/molar mass) = moles of a substance
Molarity (M)
Molarity = (Moles of a solute)/(Liters of a solution)
Weak acids have a Ka ___ 1
Ka < 1
Strong acids have a Ka ___ 1
Ka > 1
Bases almost always have a ______ charge than the acid
more negative/ lower
What dictates the movement of acid/base drugs across the membrane?
Charge. pH of a solution and the pK of a drug dictates charge. Only uncharged molecules go through the membrane easily.
Ka is _____ with a stronger acid and pKa is _____.
Ka is higher, pKa is lower. Means there is more H+ dissociation and that more acid would be required to put the proton (H+) back onto the conjugate base.
Ka is _____ with a weaker acid and pKa is _____.
Ka is lower, pKa is higher. Means there is less H+ dissociation and that less acid would be required to put the proton (H+) back onto the conjugate base.
Definitions of pKa.
The pKa is the pH at which both the acid (HA or HB+) and the conjugate (A- or B) base are maintained in equal amounts.
10^pH-pK = [A-]/[HA] = 1/1
10^pH-pK = [B]/[HB+] = 1/1
(above is the Henderson-Hasselbach Equation )
pKa is a measure of the hydrogen ion concentration required to put a proton back on the conjugate base of the acid.
What is a buffer?
A buffer is essentially a weak base that acts as a protonated acid by adding a weak acid.
Buffers work to compensate when hydrogen ion is added or removed to a solution that was in equilibrium.
They are designed to maintain constant pH by preventing changes in the [H+] by absorbing or providing extra [H+]
Buffers are made from weak acids and their salts.
Is pure water buffered?
Pure water is not buffered .
Water is an extremely weak acid and not highly ionized. Any change in the [H+] or [OH-] will cause a change in the pH of the solution.
What is a neutralization reaction?
The reaction of a bonsted acid and a bronsted base can yield water and a salt. 1 OH- from the base will react with 1 acidic proton (H+) from the acid.
