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General Chemistry
Solubility
| Question | Answer |
|---|---|
| Salt dissociates from the surface, where atoms have the least what? | The least ionic interactions with neighboring ions in the lattice |
| Which kind of ions have the greatest contact with the solvent? | Surface ions, so they are more susceptible to solvation |
| Besides the surface ions, which ions dissolve the fastest in order? | Corners dissolve away the fastest, followed by edges and then faces |
| Define dissolving | The breakdown of intermolecular forces btwn. molecules as a solid becomes a solute within a solvent. The molecule remains intact when dissolving into solution |
| Define dissociation | The breakdown of ionic bonds btwn. atoms within lattice structure as a salt turns into a solute within the solvent. The crystal lattice of the salt breaks apart when it dissociates into solution |
| Define solvent | The species in greatest concentration into which the solute dissolves, or salt dissociates. A solvent must be a fluid |
| Define solute | The species not in highest concentration that dissolves into the solvent, or in the case of a salt, dissociates |
| Define solubility | A measurement of the degree of dissolving that a solute undergoes within a particular solvent. Entropy favors the dissolving process |
| What occurs as the solubility of a compound increases? | It can be deduced that lattice energy of the solid is decreasing, the solvation energy of the solute form is increasing, or both effects are taking place |
| Define saturated | Describes a state of a solution at the point where no more solid (solute) can dissolve into solution |
| What happens when an aqueous salt solution is saturated? | The rate of dissociation of the salt equals the rate of precipitation |
| Define supersaturated | Describes a state of a solution where the amount of solid (solute) that is dissolved into solution is beyond the maximum amount at that given temperature. |
| How can supersaturation be achieved? | By first heating a solvent, then adding solute to the solution until the solution is saturated at that temperature. Slowly cooling this solution causes the amount of solute in it to exceed what should dissolve at the reduced temperature |
| Define solubility product (Ksp) | The equilibrium constant for a dissociation reaction, determined from the molar solubility, according to standard rules for calculating equilibrium constants |
| Define molar solubility | The quantitative measurements of the maximum number of moles of a solid (solute) that can dissolve into enough solvent to make 1 liter of solution under ambient conditions |
| Define gram solubility | The quantitative measurements of the maximum number of grams of solid (solute) that can dissolve into enough solvent to make 100 mL of solution under ambient conditions |
| What is the common ion effect? | This results in the reduction in the amount of solid (solute) that can dissolve into solution due to the presence in the solution of an ion that is also present in the solid |
| What is the difference between Le Chatelier's principles and the common ion effect? | With the Le Chatelier's principles, the addition of 1 of the products (ions) causes precipitation (reduced solubility). With the common ion effect, the ion causing the reduced solubility is present in solution at the beginning of the reaction |
| Define lattice | A repeating 3-D pattern of atoms or groups of atoms in a crystal |
| What is the Ksp calculation for solubility reaction of MX(s)? | x^2 |
| What is the Ksp calculation for solubility reaction of MX2(s) and M2X(s)? | 4x^3 (3root Ksp/4) |
| What is the Ksp calculation for solubility reaction of MX3(s) and M3X(s)? | 27x^4 (4root Ksp/27) |
| When a question is asking for the compound with the highest solubility, what is it referring to? | It is referring to the compound that produces the greatest amount of dissociated salt, which refers to greatest molar solubility, NOT SOLUILITY PRODUCT |
| How do you know which compound will precipitate from a solution first? | The compound with the smallest x (molar solubility) precipitates from solution first |
| What are some cations that will always form soluble salts? | Sodium and ammonium |
| What happens when a precipitate forms? | The reaction quotient Q exceeds the equilibrium constant Ksp Ksp < Q |
| What happens when no precipitate is formed? | The reaction quotient Q is less than the equilibrium constant Ksp Ksp > Q |
| What is Ksp? | It is the Keq for salts dissociating into ions. Measure solubility |
| How much is a millimolar (mM)? | 1 × 10-3 M |
| How much is a micromolar (µM)? | 1 × 10-6 M |
| How much is a nanomolar (nM)? | 1 × 10-9 M |
| Define simple diffusion | Refers to the tendency for solutes to diffuse directly through a membrane and down their concentration gradient; from an area of high solute concentration to an area of low concentration. Importantly, not all molecules can diffuse across the cell membrane |
| What are examples of compounds that can go use simple diffusion? | Those that do tend to be small or nonpolar, with typical examples including gases such as oxygen and carbon dioxide |
Created by:
Gabbgabb04
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