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Chapter 14
General Chemistry 2 Spring Semester 2026
| Question | Answer |
|---|---|
| Define acid according to the Arrhenius definition | A substance that produces H+ ions in aqueous solution |
| Define base according to the Arrhenius definition | A substance that produces OH−ions in aqueous solution |
| Define neutralization | Acids and bases combine to form water |
| Define acid according to Brønsted–Lowry Acid–Base Theory | Proton (H+ ion) donor |
| Define base according to Brønsted–Lowry Acid–Base Theory | Proton (H+ ion) acceptor |
| Define conjugate acid-base pair | Two substances related to each other by the transfer of a proton |
| What does a conjugate acid-base pair differ by? | 1 proton |
| A base accepts what to become a conjugate ___ | A base accepts a proton and becomes a conjugate acid |
| A acid accepts what to become a conjugate ___ | An acid donates a proton and becomes a conjugate base |
| What always appear appear together in a na acid-base reaction? | Acids and bases |
| Define amphoteric. Give an example. | Substances that can act as acids or bases H2O |
| Define monoprotic acids. Give an example. | Contain only one ionizable proton |
| Define diprotic acids. Give an example. | Have two ionizable protons |
| Define triprotic acids. Give an example. | Have three ionizable protons |
| What may polyprotic acids yield? In what manner? What is written for each stage? | Polyprotic acids may yield more than one hydrogen ion per molecule.Ionize in a stepwise manner; that is, they lose one proton at a time An ionization constant expression can be written for each ionization stage |
| Define autoionization | Pure water acts as an acid and a base with itself |
| Define ion product constant for water, Kw | The equilibrium constant for the autoionization of water |
| What happens to strong acids when placed in an aqueous solution? | Strong acids fully ionize (fully dissociate) in aqueous solutions |
| What happens to weak acids when placed in an aqueous solution? | Weak acids partially ionize (dissociate) in aqueous solutions |
| What are the six strong acids? | HCl (hydrochloric acid) HBr (hydrobromic acid) HI (hydroiodic acid) HNO3 (nitric acid) HClO4 (perchloric acid) H2SO4 (sulfuric acid) |
| What are the six weak bases? | HF (hydrofluoric acid) CH3COOH (acetic acid) HCOOH (formic acid) H2SO3 (sulfurous acid) H2CO3 (carbonic acid) H3PO4 (phosphoric acid) |
| Define acid ionization constant. What variable is used? | The equilibrium constant for the ionization reaction of the weak acid |
| What happens as Ka gets larger? | Larger Ka means a stronger weak acid |
| What happens to pKa as Ka get larger? What about the weak acid? | The larger the Ka, the smaller the pKa, the stronger the weak acid |
| What happens to pKa as Ka get smaller? What about the weak acid? | The smaller the Ka, the larger the pKa, the weaker the weak acid |
| What do weak bases produce? How? What do they form? | Produce OH− by accepting protons from water, ionizing water to form OH− |
| What do most weak bases have? What does it do? | Most of the weak bases have a nitrogen atom with a lone pair, which accepts protons (H+) from water to make the substance a base |
| Define base ionization constant? What variable is used? | The equilibrium constant for the ionization of a weak base Kb |
| What happens to the pKb as Kb get larger? What about the weak base? | The larger the Kb, the smaller the pKb, the stronger the weak base |
| What happens to the pKb as Kb get smaller? What about the weak base? | The smaller the Kb, the larger the pKb, the weaker the weak base |
| When there is a mixture of a strong acid and a weak acid what does the [H3O+] total equal? | [H3O+] of the strong acid |
| When there is a mixture of a two weak acids what does the [H3O+] total equal? | [H3O+] of the higher Ka acid |
| Define percent ionization (for a weak acid) | The ratio of the ionized acid concentration to the initial acid concentration, multiplied by 100% |
| What results in a higher percent ionization for two acids of the same initial concentration | The stronger weak acids results in higher percent ionizaiton |
| Define binary acids | Contain hydrogen and only one other element (nonmetal) H−Y• Acid strength of binary acids |
| In what direction does binary acids increase when looking at the periodic table | Increases from left to right and top to bottom |
| Define oxyacids | Contain a hydrogen atom bonded to an oxygen atom that is bonded to another element |
| How does the oxyacid change as the number of oxygen atoms that are bonded to the same Y increase? | The stronger the oxyacid |
| If there are the same number of oxygen atoms, what affects the oxyacid? | For same number of oxygen atoms, the more electronegative (to the right, to the top) the element Y, the stronger the oxyacid |
| When the acid is strong what is its conjugate base? What is Ka? What is Kb? | The acid is strong, the conjugate base is pH neutral Ka is very large Kb is about 0 |
| When the acid is weak what is its conjugate base? | The acid is weak, the conjugate base is weak |
| When the acid is very weak what is its conjugate base? What is Ka? What is Kb? | The acid is very weak, the conjugate base is strong Ka is about 0 Kb is very large |
| Define salt | A chemical compound consisting of an assembly of cations and anions |
| An anion that is the conjugate base of a weak acid is what kind of base? | A weak base |
| An anion that is the conjugate base of a strong acid is ___ so it is ____ | An anion that is the conjugate base (A−) of a strong acid is so weak it is pH-neutral |
| Cations that are counterions of strong bases are ___ | pH neutral |
| Does a cation ionize in water? | No |
| What is the relationship between A- and H+ in water? | The conjugate base (A-) has a high affinity to H+ in water |
| Cations that are the conjugate acids of weak bases are what kind of acids? | Weak acids |
| Cations that are small, highly charged metals form what kind of solution? | Acidic solutions |
Created by:
KristenR2025