--- Description of the model used in "Acid-Base Solutions" This simulation models 5 types of aqueous solutions: - Pure Water - Strong Acids - Weak Acids - Strong Bases - Weak Bases Constants: W = concentration of water = 55.6 mol/L Kw = equilibrium constant of water = 1E-14 Variables: C = concentration of the acid or base in mol/L Ka = strength of acid Kb = strength of base Generic symbols: A = the molecule that separates from hydrogen (H) when a weak or strong acid (HA) dissociates M = the metal ion that separates from hydroxide (OH-) and remains in solution after a strong base (MOH) dissociates B = a weak base molecule that can accept a hydrogen atom to form BH+ Concentration: The notation [X] indicates the concentration of molecule X. Pure Water: [H3O] = sqrt(Kw) [OH] = [H3O] [H2O] = W Strong Acids: [HA] = 0 [A-] = C [H3O+] = C [OH-] = Kw / [H3O+] [H2O] = W - C Weak Acids: [HA] = C - [H3O+] [A-] = [H3O+] [H3O+] = ( -Ka + sqrt( Ka^2 + 4*Ka*C ) ) / 2 [OH-] = Kw / [H3O+] [H2O] = W - [A-] Strong Bases: [MOH] = 0 [M+] = C [H3O+] = Kw / [OH-] [OH-] = C [H2O] = W Weak Bases: [B] = C - [BH+] [BH+] = ( -Kb + sqrt( Kb^2 + 4*Kb*C ) ) / 2 [H3O+] = Kw / [OH-] [OH-] = [BH+] [H2O] = W - [BH+] pH: pH ranges from 0 to 14 in this simulation, and is computed as a function of [H3O+]: pH = -log10( [H30+] ) Conductivity: For the purposes of this simulation, conductivity is modeled as a number between 0 and 1 inclusive. This value has no units and determines the brightness of the light bulb. Conductivity is computed as a linear function of pH, as follows: pH_min = 0 pH_max = 14 C_open_circuit = 0 C_max = 1 C_neutral = conductivity of a neutral (pH=7) solution (a small constant > 0) if open circuit, conductivity = C_open_circuit else if pH < 7, conductivity = C_neutral + ( ( 1 - C_neutral ) * ( 7 - pH ) / ( 7 - pH_min ) ) else if pH >= 7, conductivity = C_neutral + ( ( 1 - C_neutral ) * ( pH - 7 ) / ( pH_max - 7 ) ) ---