GC2 Test 4
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35 terms
Terms | Definitions |
|---|---|
 Arrehinus definition of an acid | an acid is a substance that produces H+/H3O+ (hydrogen/hydromium ion) when placed in water, a process called ionization |
| According to the Arrehinus concept, a strong acid... and a weak acid.... | ionizes to an extent of 100% ionizes to an extent of less than 100% |
| Examples of Arrehinus acids include... | HCl, HBr, HI, HC2H3O2, etc. |
| Arrehinus definition of a base | a base is a substance that produces OH- (hydroxide ions) when placed in water |
| According to the Arrehinus concept, a strong base... | produces OH- ions to 100% |
| Bronsted/Lowry definition of an acid | an acid is a substance that can donate a proton |
| Bronsted/Lowry definition of a base | a base is a substance that can accept a proton |
| According to the Bronsted/Lowry concept, a strong acid... and a weak acid... | has a large tendency to donate H+ has a small tendency to donate H+ |
| According to the Bronsted/Lowry concept, a strong base... and a weak base... | has a large tendency to accept H+ has a small tendency to accept H+ |
| Strong acids have... | weak conjugate bases |
| Weak acids have... | strong conjugate bases |
| Strong bases have... | weak conjugate acids |
| Weak bases have... | strong conjugate acids |
| H2O is amphiprotic, which means... | it can act as either an acid or a base depending on what it's with |
| Water is the conjugate base of... | H3O+, hydromium ion |
| Water is the conjugate acid of... | OH-, hydroxide ion |
| Examples of Bronsted/Lowry acids include... | HF, H3O+, NH4+, H2O |
| Examples of Arrehinus bases include... | NaOH, KOH, Ca(OH)2, Ba(OH)2 |
| Examples of Bronsted/Lowry acids include... | F-, H2O, NH3, OH- |
| Lewis definition of an acid... | a molecule or ion that can accept an electron pair (electrophile: seeks electrons), has an atom in it with an empty orbital |
| Lewis definition of a base... | a molecule or ion that has an inshared pair of electrons on an atom (nucleophile: seeks a nucleus to bond with) |
| Acid/Base reaction according to the Lewis concept... | Base (donates e-) + Acid (accept e-) --> Product (new single covalent bond from the shared e-) |
| K[H2O] = ... | [H+][OH-] = 1 x 10^-14 |
| pH + pOH = ... | 14 |
| pH = ... | -log[H+] |
| pOH = ... | -log[OH-] |
| [H+] = ... | 10^-pH |
| [OH-] = ... | 10^-pOH |
| Method 1 to find concentration of either [H+] or [OH-]... | [H+] = 10^-pH [OH-] 10^-pOH |
| Method 2 to find concentration of either [H+] or [OH-] (teacher's method)... | [H+] = 1*10^-4 / [OH-] [OH-] = 1*10^-4 / [H+] |
| Checking RA, method 1... | show that [HA]0 - x = [HA]0 |
| Checking RA, method 2... | 2% rule, y = 0.2[HA]0 If x < y, RA is valid |
| For weak acids, as [HA]0 decreases... | %I increases |
| The strong acids include... | HCl, HNO3, H2SO4, HBr, HI, HClO4 |
| If [H3O+] = 1... If [H3O+] > 1... | pH = 0 pH < 0 |
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