Protons

• Acids are good 


  conductors of electricity
• Strong acids


  disassociate completely into ions in water
• Boron is stable with just 6 electrons but can: accept 2 more although it’s an exception to the octet rule
• Bases are proton


  acceptors
• Acids are proton


  donors
• Older (Arrhenius’ definition) concluded that all acids have: [H+] and all bases have [OH-]
• More relevant Brønsted & Lowry theory proposes that: Brønsted & Lowry acids are proton donors and Brønsted & Lowry bases are proton acceptors. Lewis acids are electron pair acceptors and Lewis base are electron pair donors
• Acid disassociation is as follows: HA + H2O → A- + H3O+
• Hydronium (H3O+) is the: main ion in acidic solution and follow iconic acid base behavior theory. It can also be expressed as [H+]
• Binary acids are made of a halide and hydrogen and increase in strength: across a period and down a group. They include HF, HCl, HBr, and HI
• Oxyacids acids are polyatomic ions including: HNO3, H2SO4, H2CO3, and H3PO4
• Weak acids have strong: conjugate base pairs and vise versa
• Strong acids have weak: conjugate base pairs and vise versa
• A conjugate pair is made up of a substance and its form after: protonation or deprotonation
• Conjugate pairs should only differ by

  1 proton
• Organic acids are almost exclusively

  weak acids
• Acids chip away


  bases by donating protons
• Mineral testing for calcite (CaCO3) includes a drop of: acid that causes the solution to bubble in calcite presence due to the reaction forming gas (CO2)
• Monoprotic acids can only donate

  1 H+
• Diprotic acids can donate only

  2 H+
• Triprotic acids can donate only

  3 H+
• Alkali or alkali earth metals and oxygen or hydroxides make: common bases
• Some weak bases are: NaHCO3 (sodium hydrogen carbonate),Na2CO3 (sodium carbonate), NH3 (ammonia), and CH3CH2NH2 (ethanamine)
• Amphiprotic substances include: HCO3- (hydrogen carbonate ion), HSO4- (hydrogen sulfate ion), H2PO4- (dihydrogen phosphate), HPO4(2-) (hydrogen phosphate), and H2O (water)
• Amphiprotic means to be able to either: donate or accept protons
• Amphoteric means to be able to either: display acid or base behavior
• All amphiprotic substances are amphoteric but not: all amphoteric substances are amphiprotic
• The disassociation of a strong acid is: exothermic the acid is happy and stable as an ion
• NH4+ is a coordinate bond where H is: not very happy because its electron are lost to the more electronegative oxygen
• the pH scale is between 0 to 14 but can extend to: infinity and negative infinity
• Lithmus indicator turns blue in the presence of


  base
• Lithmus indicator turns red in the presence of

  acid
• pH is calculated with [H+] with the formula: pH=-log[H+] where base = 10
• pOH is calculated with [OH-] with the formula: pOH=-log[OH-] where base = 10
• [OH-] is calculated with pOH with the formula

  [OH-]=10^(-pOH)
• [H+] is calculated with pH with the formula

  [H+]=10^(-pH)
• To convert from pOH to pH, you: subtract it from 14 [14-pOH=pH] and vise versa
• For strong acids and bases, the initial concentration of: [H+] or [OH-] is the same as the substance due to complete disassociation.
• Methyl orange turns red in the presence of


  base
• Methyl orange turns yellow in the presence of

  acid