Acids and Bases Chemistry^3 Mindmap
- Created by: Strelly22
- Created on: 13-12-22 12:03
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- Acids and Bases
- Bronsted-Lowry acids and bases
- H2O [acid] + NH3 [base] < -> OH- [c base] + NH4 + [c acid]
- BL acid = proton donor
- BL base = proton acceptor
- acid-base reaction involves proton transfer
- the oxonium ion [H3O+] is responsible for acidic properties of aq solutions of acids
- acid-base reactions involve conjugate acid-base pairs
- conjugate base of an acid = acid - a proton
- conjugate acid of a base = base + a proton
- The strengths of acids and bases
- strong acid = powerful proton donor
- strong base = powerful proton acceptor
- Ka = [H3O+] [A-] / [HA]
- pKa = -log Ka
- pH = -log [H3O+]
- pOH = -log [OH-]
- Kw = [H3O+] [OH-]
- pH + pOH = 14
- Kb = [BH+] [OH-] / [B]
- pKb = -log Kb
- Ka x Kb = Kw
- lower the pKa, stronger the acid, greater the Ka
- lower the pKb, stonger the base, greater the Kb
- Buffer solutions
- Assumptions:
- 1) all A- ions come from the salt
- 2) almost all HA molecules put into the buffer remain unchanged
- pH = pKa + log [A-] / [HA]
- resistant to changes in pH on addition of small quantities of acid or base
- Assumptions:
- pH changes in acid-base titrations
- titration curve shows how the pH of solution changes during titration
- SA vs SB -> EP at pH 7
- SB vs WA -> EP > pH 7
- at half neutralization, pH = pKa
- SA vs WB -> EP < pH 7
- Oxoacids
- HmXOn
- increase in strength with increasing (n-m)
- variations of concs of acid and associated anions with pH is shown using speciation curves
- Acidic and basic oxides
- amphoteric = react with acids and bases
- on the basis of reactions with water or acids / bases
- Lewis acids and bases
- lewis acid = electron pair acceptor
- lewis base = electron pair donor
- Indicators
- chosen so pKin = pH at EP
- Bronsted-Lowry acids and bases
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