Practice Test: Chapter 4

Matching skip

Short Answer skip

1. net ionic equation
   
2. solute
   
3. electrical conductivity
   
4. reducing agent
   
5. precipitation reaction
   

Multiple Choice skip

1. Describe the H2O molecule
   1. In virtually every case, when solid containing ions dissolves in water, ions separate. Move around independently. 1. Compound produced must have 0 net charge, contain both anions and cations. 2. Must compounds only 1 type of cation and 1 anion. Whichever of products more soluble becomes solution. Least soluble = precipitate. Solubilities of ionic substances. Slightly soluble interchangeable with insoluble. Focus on actual components of solution before any reaction occurs then figure out how these components will react with each other
   2. Ability to dissolve many substances. Bent (V-shape). Covalent bonds between O and H's. O more electronegative than H, attracts more e-. O -, H+
   3. Electron acceptor. Reduced
   4. 2 solutions mixed, insoluble substance sometimes forms. Solid forms separate from solution
   5. Point where indicator actually changes color
2. finding a precipitate
   1. Proton donor
   2. Solid formed, must know identities of reactants and products
   3. In virtually every case, when solid containing ions dissolves in water, ions separate. Move around independently. 1. Compound produced must have 0 net charge, contain both anions and cations. 2. Must compounds only 1 type of cation and 1 anion. Whichever of products more soluble becomes solution. Least soluble = precipitate. Solubilities of ionic substances. Slightly soluble interchangeable with insoluble. Focus on actual components of solution before any reaction occurs then figure out how these components will react with each other
   4. Moles of solute per volume of solution, in liters. M = molarity = moles of solute / liters of solution
3. oxidizing agent
   1. Point in titration where enough titrant has been added to react exactly with analyte
   2. Same as balacing in acid PLUS: 8. Add OH- ions to cancel H+. 9. Reduce H2O again
   3. The same as moles of solute constant. Always holds up in dilution
   4. Electron acceptor. Reduced
   5. Ability to conduct an electric current. Arises from presence of ions. Extent to which solution can conduct an electric current depends directly on the number of ions present
4. Must know 2 things to perform stoichiometric calculations
   1. Point where indicator actually changes color
   2. 2 solutions mixed, insoluble substance sometimes forms. Solid forms separate from solution
   3. Acid-base reaction. When base reacts exactly with acid, acid has been neutralized
   4. Solution whose concentration is accurately known
   5. 1. Nature of reaction (Exact forms the chemicals take when dissolved) 2. Amounts of chemicals (concentrations)
5. hydration
   1. Conduct only a small current. Relatively few ions. Exhibit small degree of ionization in water. Acetic acid, HC2H3O2. Non-acidic Hydrogens written later in the formula. Reaction happens in both directions- Double arrows
   2. Contain OH-. Become cation + OH-
   3. Electron donor. Oxidized
   4. Positive ends attracted to negative other molecules and vice versa. Ionic substances dissolve in water by breaking down into individual cations and anions
   5. Proton donor

True or False skip

1. weak acids
   Ability to conduct an electric current. Arises from presence of ions. Extent to which solution can conduct an electric current depends directly on the number of ions present

   True   False

2. steps for balancing redox reactions in acidic solution
   1. Divide into 1/2 reactions. 2. Balance for any element other than H or O. 3. Balance each for O by adding H2O. 4. Balance for H by adding H+. 5. Balancing for charge by adding e-. 6. Multiply 1/2 reactions by integer to cancel e-. 7. Cancel like items on reactant and product sides

   True   False

3. standard solution
   Point where indicator actually changes color

   True   False

4. acids
   Substances that produce H+ ions when dissolved in water. Polar nature of water causes them to ionize

   True   False

5. weak bases
   Point in titration where enough titrant has been added to react exactly with analyte

   True   False