| A | B |
|---|
| Given H2O , NaOH, HC2H3O2 ,or CH4 , choose which is the strong (or stronger) Base. | Sodium Hydroxide, NaOH |
| What are the products of the neutralization reaction between sodium hydroxide ( NaOH ) and sulfuric acid? | Na2SO4 and H2O |
| What is the molarity of a solution made by dissolving 17.0 g lithium iodide ( LiI ) in enough water to make 500 mL of solution? | 0.254 M |
| What is the molarity of a solution made by dissolving 34.0 g sodium chloride ( NaCl ) in enough water to make 500 mL of solution? | 1.16 M |
| Calculate the molarity of a water solution of CaCl2 , given that 5.04 L of the solution contains 612 g of CaCl2 . | 1.09 M |
| Calculate the molarity of a water solution of KCl , given that 2.50 L of the solution contains 350 g KCl . | 1.88 M |
| What would the final volume of a solution containing 9.0 moles of a solute in 500.0 mL of a solution? | 18 M |
| What is the quantity ( moles of solute) divided by ( Volume of solution in Liters) called? | Molarity....Symbolized by bolded capital M ( often with line under generally) |
| What is the quantity described by ( moles of solute) divided by ( mass of the solvent in Kg ) ? | Molality, symbolized generally as an unbolded scripted small cased m |
| molarity | moles solute/ volume solution |
| molality | moles solute/ mass of solvent |
| a measure of the amount of solute in a given amount of solvent or solution | concentration |
| The net amount of energy absorbed as heat by the solution when a specific amount of solute dissolves in a solvent | enthalphy of solution |
| State of Matter with very little if any molecule interactions as compared to other States of Matter | Gas State. Molecules, in the gaseous state, are so far apart that virtually no intermolecular forces of attraction nor repulsion is observed |
| What happens to the ENERGY as a gas dissolves in a liquid, why? | Energy is RELEASED because attraction between the solute gas and solvent molecules outweighs the energy needed to separate solvent molecules |
| When a solute particle is surrounded by solvent molecules | solvated |
| What happens to the solubility of gases in water as temperature varies? | If a rise in Temperature occurs, gas solubilty in water decreases. If Temperature drops, gas solubilty in water INCREASES |
| Liquids that ARE able to dissolve one another in any proportion | miscible |
| Liquids that ARE NOT soluble within one another...This is such that two liquids can not dissolve either way the "other" liquid.. | immiscible |
| Rapid escape of a GAS from a LIQUID as it is dissolved by the liquid | effervescence |
| Solution process with water acting as the solvent | hydration |
| The amount of a substance that is required to form a saturated solution with a specific amount of solvent at a specific temperature is called the substance's what? | solubility |
| Created when a substance is dissolved in water to form a solution that DOES NOT conduct electricity. | nonelectrolyte |
| Called this when a substance dissolved in water forms a solution that DOES conduct electricity. | electrolyte |
| This property can be used to distinguish between a colloid and a solution. This occurs when when light is SCATTERED by the colloidal particals that are dispersed in a transparent ( seemingly clear) liquid. | Tyndall Effect |
| Mixture madeup of tiny particles intermediate in size between those in solution and those in suspension AND that are SUSPENDED in a liquid, gas, or solid. | colloids |
| This type of mixture occurs when the particles in a solvent are so LARGE that they settle out unless the mixture is continually agaitated or stirred. | Suspension Mixture |
| Homogeneous mixture of two or more substances in a single phase | solution |
| The dissolving medium in a solution | solvent |
| The dissolved medium in a solution, these particles are so small they can not be seen. | solute |
| Capable of being dissolved | soluble |
| Diffuse , or spread out, due to their constant random molecular motion | gases |
| The behavior of MOST GASES is nearly IDEAL except at very high PRESSURES and very low temperatures. | Kinetic-Molecular Theory |
| tool that measures atmospheric pressure | barometer |
| States that in a gas mixture, the TOTAL PRESSURE of the GAS MIXTURE will be equal to the SUM of all the partial pressures from each individual gas within that mixture | Dalton's Law of Gas Partial Pressures |
| What will happen to the rate of reaction if temperature is LOWERED? | Generally, the rate of reaction will be SLOWER if temperature decreases |
| What will happen to the rate of reaction if the SURFACE AREA of reactants ( left side of Chemical Reaction) is increased? | Increased exposed surface area onto the REACTANTS generally will INCREASE (speed up) the rate of reaction |
| This MUST OCCUR before ANY two or more gas particles to react. | They must COLLIDE |
| Minimal Energy REQUIRED for an EFFECTIVE COLLISION | Activation Energy |
| A substance that is NOT used up in a reaction but does serve to increase the RATE of REACTION | catalyst |
