Term
Which procedure is used to determine when a solution is saturated?
|
|
Definition
| Add a crystal of the solute. |
|
|
Term
| After crystallization takes place, the liquid in contact with the crystals is... |
|
Definition
|
|
Term
| If a substance is only slightly soluble in water, then which of the following terms could not be used to describe a solution of the substance in water? |
|
Definition
|
|
Term
| Evaporation of a solvent from a solution of a solid in a liquid causes the solution to become: |
|
Definition
|
|
Term
| The molecule H-O-H is said to be polar. |
|
Definition
|
|
Term
| The molecule Cl-Cl is said to be polar. |
|
Definition
|
|
Term
| Fill in the blanks: With regard to solubility based on the polarities of solute and solvent, _______. |
|
Definition
|
|
Term
| Solutions that conduct electricity: |
|
Definition
| Contain either dissolved ionic solids or acids. |
|
|
Term
| Which of the following species will conduct electricity? |
|
Definition
| K2CrO4(aq), H20, KBr (aq) |
|
|
Term
| Which one of the following solutions will have the highest electrical conductivity? |
|
Definition
|
|
Term
| When 34 grams of potassium carbonate are dissolved in enough water to make 750 mL of solution, what is the concentration of the potassium ion in this solution? |
|
Definition
| 34g× 1/99.1g = 0.3431 mol × 2= 0.68 |
|
|
Term
| A 0.01 M barium hydroxide solution would have an OH ion concentration of approximately |
|
Definition
|
|
Term
| If 2.52 grams of Na2SO4 are dissolved in enough water to make one liter of solution, what is the concentration of the sodium ions in this solution? |
|
Definition
| 2.52g × 1 mol/ 142g = 0.019mol × 2= 0.0316M |
|
|
Term
| Using the solubility rules, predict whether or not a double-replacement reaction will occur between these ionic compounds. If so, choose the precipitate. |
|
Definition
|
|
Term
| Fill in the blanks: A colligative property is a property that changes based on the _______ of solute in a solvent, bent not the _________ of the solute. |
|
Definition
|
|
Term
| A 1.5 M aqueous solution of ammonium sulfate, (NH4)2SO4, has a boiling point of 102.2 degrees C and a melting point of -8.4 degrees C. Predict the boiling point and melting point of a 3.0 M solution of ammonium sulfate. |
|
Definition
| BP = 104.4 degrees C; MP = -16.8 degrees C |
|
|
Term
Fill in the blanks:
OH- is the _______________ ion.
H3O+ is the _________________ ion. |
|
Definition
|
|
Term
| How many times more acidic is a solution with pH 1 versus a solution with pH6? |
|
Definition
|
|
Term
| What is [H3O+] for a solution with pH6? |
|
Definition
|
|
Term
| 50.0 mL of a hydrochloric acid solution is titrated to its phenolphthalein endpoint with 37.5 mL of a 1.250 M KOH solution. What is the original concentration of the hydrochloric acid solution? |
|
Definition
0.0375L × 1.250 mol/ 1L = 0.046875 mol
0.046875 mol / 0.0500 L = 0.938 M |
|
|
Term
| The amount of dissolved oxygen in a sample of river water is 3.66 × 10^-4 M. What is this in units of milligrams per liter? |
|
Definition
|
|
Term
|
Definition
| The interaction between a solute and a solvent where solute particles become completely surrounded by solvent molecules. |
|
|
Term
|
Definition
| Able to contain more dissolved solute. |
|
|
Term
|
Definition
| The solute can be dissolved by the solvent to a form a solution. |
|
|
Term
|
Definition
| a homogeneous mixture where a solute is dissolved in a solvent. |
|
|
Term
|
Definition
| Containing more of a solute than is stable. |
|
|
Term
|
Definition
| a substance being dissolved. |
|
|
Term
|
Definition
| The substance in which the solute is dissolved. |
|
|
Term
|
Definition
| Containing as much dissolved solute as possible. |
|
|
Term
|
Definition
| Liquids which are insoluble in each other, and separate into phase or layers. |
|
|
Term
|
Definition
| The maximum amount of solute that can be dissolved in a given solvent at a given temperature |
|
|
Term
|
Definition
| When a solution has a greater concentration of hydroxide ions than hydronium. |
|
|
Term
|
Definition
| A method of determining the exact concentration of a solution through a known chemical reaction. |
|
|
Term
|
Definition
| based on observation or experience rather than the theory |
|
|
Term
|
Definition
|
|
Term
|
Definition
| When a solution has an equal concentration of hydronium and hydroxide ions. |
|
|
Term
|
Definition
| The separation of already - existing ions from an ions compound. |
|
|
Term
|
Definition
| The speration of a neutral, covalent molecule into ions through a reaction with a solvent. |
|
|
Term
|
Definition
| Wen a solution has a greater concentration of hydronium ions than hydroxide ions. |
|
|
Term
|
Definition
| Ions that exist in the same form on both the reactants and products of chemical equation. |
|
|
Term
|
Definition
|
|
Term
|
Definition
| An analysis method where the element under investigation is precipitated as a compound and then weighed |
|
|
