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| Question | Answer |
| A Strong Electrolyte | A strong electrolyte totally ionized when dissolved in water. HCl is an example of a strong electrolyte |
| A Bronsted-Lowry base | a base is a molecule that accepts a protonwhen it encounters an acid base (proton donor). By this definition, NH3 can be a bronsted base |
| A conjugate acid of a bronsted-lowery base | The conjugate acid of a bronsted-lowry base is the potential proton donor formed when a bronsted-lowty base accepts a proton. For example, the NH4+is a conjugate acid in the reaction, NH3 + proton -> NH4+ |
| Neutralization in terms on bronsted lowry concept | Neutralization, according to the BL concept, occurs when a reaction involving an acid and its conjugate base in combined with a second reaction involving a base and its conjugate acid. NH3 + H2O -> NH4+ + OH- |
| An amphiprotic solute | an amphriprotic solute can act either as an acid or a base depending on the situation an amino acid in an amphiprotic solute. |
| A zwitterion | a switterion is a chemical species that bears both positive and negative charges. Free amino acids such as glycine, can exist as zwitterionin solution. |
| Autoprotolysis | autoprotolysis is the act of self-ionization to produce botha. conjugate acid and a conjugate base |
| A weak acid | a weak acid only partially dissociates such that there are undissociated molecules and ions in aqueous solution. Acetic acid HOAc is an example of a weak acid |
| La Chatlier's principle | the lachatelier principle states that the position of a n equlibrium always shifts in such a direction that it relieves the stress. A common ion like sulfate added to a solution containing sparingly soluble BaSO4 is an example |
| the common ion effect | the common ion effect is responsible for the reduced solubility of an ionic precipitate when one of the soluble components reacting to form the precipitate. Chloride ion added to an AgCl solution decreases the solubility of Ag+ because of the common ion effect. |
| an amphiprotic solvent | an emphiprotic solvent can act either as an acid or a base depending on the solute. Water is an example of an amphiprotic solvent since it can act as a proton donor or proton acceptor |
| A differentiating solvent | a differentitating solvent reveals different strenghts of acid. By this definition, anhydrous acetic acid is a differentiating solvent because perchloric acid dissociated 5000 times more than hydrochloric acid. |
| A leveling solvent | a leveling solvent shows no difference between strong acids. Perchloric acid and hydrochloric acid ionize completly in water; thus, water is a leveling solvent. |
| a mass-action effect. | A mass-action effect arises when a shift in a chemical equilibrium occurs due to the introduction o fone of the participating chemical species (i.e. additon of one of the reactants or products) |
| Briefly explain why there is no term in an equlibrium-constant expression for water or for a pure solid, even though one (or both) appears in a balanced net ionic equation for the equlibrium. | For dilute aqueous solutions, the concentration of water remains constant and is assumed to be independent of the equilibrium. This its concentration is included within the equlibrium constant. For a pure solid, the concentration of a chemical species in a solid phase is constant. As long as some solid exsists as a second phase, its effect on the equlibrium is constant and is included within the equilibrium constant. |
| Difference between activity and activity coefficient | activity aA is the effective concentration of a chemical species A in solution. The activity coefficient is the numerical facror necessary to convery the molar concentraiton of the chemical specifes. A to activity as shown aA = yA[A] |
| thermodynamic and cencentration equilibrium constants. | The thermodynamic equilibirum constant refers to an ideal system within which each chmical species is unaffected by any others. A concentration equilibrium constant takes into account the influence exerted by solute species upon one another. The thermodynamic equlibrium is numerically constant and independent of ionic strength. The concentration equilibrium constant depends on molar concentration of reactants and products as well as other chemical species that may not participate in the equlibrium. |
| List several general properties of activity coefficients | 1. activity coefficient depends on the solution ionic strengths 2. in very dilute solutions, the activity coefficient becomes smaller as the charge of the chemical species increases. 3. For a given ionic strength, the activity coefficient becomes smaller as the charge of the chemical species increases. 4. At any ionic strength, the activity coefficients are approximately equal for a chemical species having the same charge state. |
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