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Chem Unit 3

this will contain all important information on unit 3

QuestionAnswer
What will NACl(s) dissolve into? 1 clear solution
Why do crystals pull apart? When crystals interact with water, the water molecules pull apart the crystal.
Is water polar or non-polar? Polar - has a negative and positive charge
What tends to dissolve compounds? Polar solvents
When you add crystals to water, what happens? They become more electrically conductive as more salt is added.
What is an electrolyte? Conducts electricity and can be a strong or weak.
What defines a strong electrolyte? Any ionic compound that is soluble or ionizes completely.
What is ionization? The process by which ions are formed by gain or loss of an electron from an atom or molecule
Are acids strong electroylytes? Yes
What defines weak electrolytes? partially conduct electricity acidic acid
What particles dissolve in water but don't conduct electricity (ionize)? Why? sucrose and glucose These ions don't break apart into single atoms
What defines a non-electrolyte? doesn't conduct electricity
What is a solution? Example. The combination of a solute and solvent NaCl (solute) + H2O (solvent) = NaCl + H2O
What is an aqueous solution? solvent is water
What is solubility affected by? Show example. temperature Temp rise --> dissolution rises --> solubility rises
What defines a concentration? How many moles of the substance are present per unit volume
What defines molarity? the number of moles of solute per liter of solution M = moles/liters
What do you do when you have grams of a solute instead of moles when finding molarity? just convert grams to moles
What is dilution? adding solvent to a solution
What happens if moles of solute stayed the same? It will become less concentrated as volume rises. M1V1 = M2V2
In the equation M1V1 = M2V2, what is important about the quantities? They are inversely related? doubling V = 1/2 concentration
What would the molarity of a solution made from 86.5 g Ca(OH)2 in 200.0 mL of water? 5.85 M
To what volume would you need to dilute 5.85 M to make it 1.95 M? 0.600 L
What is concentration of a solution? measurement of the number of particles of a solute number of particle sin concentrated solutions are greater than the number of particles in a diluted solution
What are the formulas for concentration of solution? Formula 1 M = moles/liter or V Formula 2 M = mass (g)/volume
What is an example of an aqueous solution? sugar in water sugar = solute and water = solvent
Is sugar(sucrose) covalent? Yes because all the atoms are nonmetal?
What happens in an aqueous solution? Water breaks apart sugar molecules, but doesn't break apart the covalent bond
What is solvation? When a solute particle is surrounded by molecules of a solvent
What is solvated? Solute surrounded by solvent molecules
What is hydrated? solute surrounded by water molecules
What are hydration shells? clusters of water molecules surrounding solute (solute cages)
What are ionic solutes? Example. ionic compounds made of ions (nm and m) crystal
What is dissociation? Example. Water breaking up ionic compound into ions in a solution table salt NaCl
Covalent vs Ionic Covalent solutes stay molecular ionic solutes dissociate into ions
What happens when water dissolves ionic compounds? They form different hydration shells
Why are partial charges attracted to ions? partially negative is attracted to positive ions and vice vers
What is precipitation? It is a double replacement reaction
What is important to know about percipitation? nitrates and chlorides are always soluble with the exception of silver, mercury, and lead lithium, sodium, potassium are always soluble
What is an Arrhenius acid? Any species that increases the concentration of hydrogen (H+) ion in aqueous solutions
What is an Arrhenius base? Any species that increases the concentration of H+ ion in aqueous solutions
What is molecule is made when H+ ions react with water? H3O+ (hydronium) ions
What is the molarity of hydronium ions? 1.0 *10 ^-7 M at 25 degrees C
What is acid-base or neutralization reaction? acid and a base react to form water and salt
Give an example of an Arrhenius Acid. HCL (aq) --> H+ (aq) + Cl- (aq) Arrhenius acid as hydrochloric acid dissociates into H+ ions
Give an example of forming hydronium ion. H+ (aq) + H2O (l) --> H3O+ (aq) Forms immediately when an acid dissociates in water.
What is the most common base? NaOH(aq)
What is neutralization? A double replacement reaction
What equations can you use to find [H+] and pH? ph = -log[H+] [H+] = 10 ^-ph
What equations can you use to find [OH-] and pOH? pOH = -log[OH-] [OH-] = 10 ^-pOH
What is important to know about concentrations of [H+]? for every factor of 10 increase in concentration of [H+], pH will decrease by 1 unit, and vice cersa
Determine the pH, [OH-], pOH of 0.039 M HCl. pH = 1.41 pOH = 12.59 [OH-] = 0.000034 M
What scale does the pH scale use? logarithmic scale
What is the neutral solution of pH? 7
What is the acidic solution of pH? pH < 7
What is the basic solution of pH? pH > 7
What is a Bronsted-Lowry acid? any species that is capable of donating a proton
What is a Bronsted-Lowry base? any species that is capable of accepting a proton, which requires a long pair of electrons to bond to the H+
What is a conjugate base? Bronsted-Lowry acid formed after a base accepts a proton
What is a conjugate acid? Bronsted-Lowry based formed after a base accepts a proton
What is an acid base reaction? any reaction where a proton is transferred from acid to base
What is a strong acid? a species that dissociates completely into its constituent ions in aqueous solutions.
What is a weak acid? doesn't completely dissociate into its constituent ions
What are the 6 strong acids? HCl, HI, HNO3, H2SO4, HBr, HClO4
What is an example of a weak acid? acetic acid (CH3COOH)
What is a strong base? base that ionizes completely in aqueous solutions
Example of a strong base. sodium hydroxide (NaOH)
Example of a weak base. ammonia (NH3)
Created by: pandabear66*
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