Chemistry

Question	Answer
Solution	Homogenous mixiture in which the components are uniform, looks the same throughout Example: Salt Water
Solvent	the dissolving medium in a solution present in the largest amount. Typically in a larger quantity than the solute Example Water.
Solute	A substance dissolved in a solvent to form a solution Example : Sodium Chloride
Aqueous solution	Solution with water as the solvent
Ionic Substance	as an ionic substance dissolved in water the solute breaks apart into its ions. Example: sodium chloride will break apart into the sodium cation and the chloride anion
Solubility	polar substance dissolve in polar substances non polar substances dissolve in non polar substances. Water dissolves both ionic and polar substances. Example: oil and water don't mix because oil is non polar, and water is non polar
Saturated Solutions	A solution which contains as much solute as will dissolve at a given temperature Example: tea with one pack of sugar that dissolves throughly, but more packets than that will not
Unsaturated	a Solution that contains less solute than will dissolve at a given temperature Example: unsweetened tea
Supersaturated	A solution that contains more solute than will dissolve at a given temperature. This may occur if a solute is dissolved at a high temperature and solute beyond the saturation point remains solution. Example: tea with so much sweetener it is like diabetes in a bottle.
Solubility Curve	Is used to find the saturation point of a solute at a given temperature
Concentrated Solution	Describes a solution that has a relatively large amount of dissolved solute. Quantitative term
Dilute Solution	Describes a solution that has a relatively small amount of dissolved solute. Qualitative term. more dilute has more solvent present it would be a clearer color when talking about water.
Factors Affecting the Rate of Dissolution	Dissolution is the dissolving Process. Process is influenced by 1. Surface area: the greater the solvent-solute surface area interaction the faster the dissolution process 2. Stirring: provides continuous exposure of solvent 3. Temperature: Allow the solvent molecules to move faster. Most solids are generally more soluble at higher temperatures.
Mass Percent	an expression of the mass of solute present and the given mass of solution mass of solute/ mass of solution 100= grams of solute/ grams of solute + grams of solvent 100
Molarity (M)	Description of a solution in terms of concentration of the solution. Moles of soluter per volume of solution in liters. M=molarity= moles of solute/ liters of solution= mol/L
Formalin	aqueous solutions of formaldehyde
Standard Solution	concentrate is accurately known
Stock Solution	is a concentrated solution that is often diluted to obtain a desired concentration
Dilution	is the process of adding more solvent to a known solution to achieve a lesser concentration
Dilution Process	The Dilution process should occur in a volumetric flask. To determine the volume of the needed of the standard solution in comparison to the volume desired of the dilute solution use: M1V1=M2V2 the moles of solute remain the same before and after a dilution
Volumetric Flask	Image: volum.gif (image/gif)
Steps to making a Solution (Example problem using if you are given 12 M HCl how much is needed to make 125 mL of 6.0 M HCl)	1. use a volumetric pipette to measure 63 mL of 12 M HCl 2. Place the 12 M HCl (63 ml) into the volumetric flask. In this case the desired flask is 125 mL 3. Add water to the line 4. Shake it
Molality	A method of describing solute concentration is molality (m) m=molality= moles of solute/kilograms of solvent= mol/kg
Colligative Properties	A solution property that depends on the number of solute particles
Boiling Point Elevation	Boiling Point of a substance is the temperature at which the vapor pressure of a liquid equals the atmospheric pressure. Adding a nonvolatile solute to a liquid decreases. More kinetic energy is required to raise the vapor pressure of the liquid which in turn elevates the boiling point of the solution above and the pure solvents
Boiling Point Elevation Equation	DeltaTb= iKbm DeltaT= Change in the boiling temperature i= van't Hoff factor = # ions salt breaks into Kb= boiling point elevation constant m= molality concentration of the solution
Freezing Point Depression	The presence of a solute interrupts the order of the solvent as it freezes this causes more kinetic energy to be withdrawn from a solution in comparison to a pure solvent which depresses the freezing point of the solution
Freezing Point Depression	Depends on the concentration of the particles not the identity of the particles. Freezing point depression is calculated using: DeltaTf= iKfm DeltaTf= change in the freezing temperature i=Van't Hoff factor= # ions salt breaks into Kf= molal freezing point depression constant m= molal concentration of the solution
PH Formula	PH=-Log [H+]
Concentration (M)	[ ] All Measured using molarity
pOH	pOH=-log [OH-]
pH+pOH	14
[H+]	Inverse log of -pH (on calculator inverse log looks like 10^
Acids	Contain an H+ ion Ex: HCl, H302
Bases	Contain OH- Ex. NaOH NH4OH
Neutrals	Contain neither H+ or OH- or they contain both H+ and OH- in equal concentration Ex: H2O-> H+ OH-
Brønsted- Lowry	Acids- proton H+ donor ex. HBR can donate the H+ Base- proton H+ acceptor ex. NH3 + H20 -> NH4+ plus OH-
Conjugate acid- base pair under Brønsted Lowry	NH3 + H20 -> NH4+ plus OH- Base plus acid on one side of arrow -> conjugate acid plus conjugate base on the other side of the arrow
Amphoteric	a substance that can behave as both an acid or a base ex. if H20 donates an H+ then OH- remains; in this case H20 is acting as an acid. if H20 accepts an H+ then H30 + forms , in this case H20 is acting as a base

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	Created by annikasquires about 10 years ago