| A | B |
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| What are electrolytes? | Ionic compounds that dissociate into charged particles called ions. Conduct electricity. |
| Weak electrolytes are...? | Organic acids that only dissociate to a small extent. Weakly conduct electricity. |
| Non-electrolytes are...? | nondissociating molecules that remain neutral. Do not conduct electricity. |
| Define a true solution. | The solute particles being disolved are usually transparent. Particles stay in solution, molecules, atoms, ions. Filtering won't separate. No Tyndall effect. |
| Colloids or colloidal dispersions are what? | Colloidal particles are large molecules, groups of molecules, or ions. Homogeneous mixtures that do not separate or settle out. 1-200 nm. Ordinary paper won't filter. Yes - Tyndal effect. |
| Desdribe the Tyndall effect. | Large solute particles scatter a beam of light shined through a solution and make the beam visible. |
| Define a suspension. | Particles greater than 200 nm. Particles settle out or can be filtered out. Hetrogenous mixture. No Tyndall effect. |
| What is solubility? | A term used to describe the amount of a solute that can dissolve in a given amount of solvent. |
| In terms of solubility, what is an unsaturated solution? | A solution that does NOT contain the maximum amount of solute it is capable of. |
| In terms of solubility, what is a saturated solution? | A solution that contains all the solute that can dissolve. |
| In terms of solubility, what is a supersaturated solution? | A solution that contains solute in excess of that which it should contain at equilibrium. Unstable. |
| What are colligative properties of a solution? | It's where a property such as boiling or freezing point depends on the NUMBER of solute particles, not the types of particles. |
| What effect does adding a solute to water have on the boiling and freezing points? | Adding solute lowers the BP to below 0 degrees celsius and raises the boiling point to above 100 degrees celsius. |
| For every mole of any solute particles added to 1 Kg of water the FP of the water is lowered by _______, and the BP is raised by _________ ? | The FP is lowered by - 1.86 degrees celsius. The BP is raised by 0.51 degrees celsius. |
| Define osmosis. | The proccess where water and solvent molecules cross a semipermeable membrane to try to equalize their [ ] (concentration). |
| Because osmosis depends on the concentration of solute particles, not the type, it is a _________ property? | Colligative property. |
| In a hypertonic solution where is the concentration of SOLUTE highest, inside or outside the cell? | Outside is higher than inside. |
| If you inject a hypertonic solution what are the cells going to do? Give off or take in water? | Since the concentration of solute (particles) is greater outside the cell it gives up water to try to reach equilibrium. |
| What is the condition of the cell called after being exposed to a hypertonic solution? | Crenation. Shrivled up due to giving away it's water. |
| Describe an isotonic solution in terms of cells in the body. | Isotonic means the concentration of solute particles is the same inside and outside the cells. |
| When cells are exposed to an isotonic solution what happens to them? | Nothing. The solute is equal inside and outside the cell so it's happy. |
| What is the condition of the cell called after being exposed to a hypotonic solution? | Hemolysis or lysis due to absorbing wather. |
| If you inject a hypotonic solution what are the cells going to do? Give off or take in water? | Since the concentration of solute (particles) is greater inside the cell it takes in water to try to reach equilibrium. |
| Explain hemodialysis. | It is the dialysis of the blood using an artificial kidney machine. |
| Explain dialysis. | A process in which water and small particles pass through a semipermeable membrane. |
| What is the formula for computing Molarity (M)? | Molarity = moles (of solute) / Liters (of solution). |
| In a problem giving you molecular or formula weights and a mass in grams, how would you determine (compute) the # of moles? | # of moles = the mass (in grams) divided by the molecular or formula weight... m=mass/FW or MW. |
| If you're given molarity and liters of solution how would you compute the # of moles? | rearrange the formula to moles = molarity X Liters. |
| When you're mixing a solution which do you put in the volumetric flask first, the mass of solute or the water? | Mass first, then the solvent, usually water. |
| What does the symbol [ ] mean? That's two brackets facing each other. | The brackets [ ] mean "concentration". The concentration of something is [xxx], or what is the [ ] of the solution?. |
| Along with Molarity we can calculate concentrations by using percent by weight-volume. What is the formula for this process? | % by weight-volume = grams of solute / TOTAL mL (grams) of solution X 100 |
| When using the % weight-volume method to determine concentrations the solute is measured in _____ and the solvent is measured in ______ or _________? | Solute measured in grams, Solvent measured in grams or milliliters. |
| What is described as the universal solvent? | Water is the universal solvent. |
| Another way of describing the % weight-volume formula is % mass = ___________ ? | grams of solute / grams of solute and solvent, times 100 |
| What is the density of water? | 1.0 g/mL |
| If water has a density of 1.0 g/mL, how many grams are in 100 mL of water? | 100 grams |
| Do solutions contain fixed portions of compounds? | Yes, but no two solutions will likely be the same. Each solution can be tested to determine the exact amount of solute in the solution. |
| Are solutions heterogeneous or homogeneous? | True solutions and colloids are homogeneous. Suspensions are heterogeneous nonuniform mixtures. |
| Are suspensions really solutions? | Yes, because they are a solute in a solvent. And, they're in the solutions chapter in the book! |
