chapter 8 Flashcards by Sadie Fernandez

define solution

a homogeneous mixture of two or more substances

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define solvent and solute

solvent- substance present in the largest quantity (only 1)
solute- substance(s) present in lesser quantity

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define aqueous solution

where water is the solvent

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define concentration

amount of solute dissolved in a given amount of solvent or solution

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define net ionic equation

shows only the atoms/molecules involved in the rxn

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define full ionic equation

shows whats happening in solution

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define molecular (chemical) equation

a shorthand. not separated out

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define solubility

how much of a particular solute can dissolve in a given volume of solution.

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define saturated

maximum amount of solute dissolved (per volume) at a given temperature/pressure

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define unsaturated

sub-maximum amount of a solute dissolved(per volume)at a given temperature/pressure

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define supersaturated

over maximum but stays soluble until precipitation is seeded

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describe molarity( part of concentration)

moles solute/liters of solution (mol/L). “molar solution” ex: 125g NaCl in 2.5L of solution. g NaCl divided by molar mass. get answer divide by liters and get answer. this says for every 1L there is x mols

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ex of M concentration: “how many moles of NaOH are in 10.0 mL of a 5.0M NaOH solution?”

(10mL)(1L/1000mL)(5.0 mol/1L)=0.050 moles

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ex of M concentration: “how many liters do you need to make a 0.2 M NaOH solution with 2.2 g NaOH?”

(2.2 g NaOH)(1 mol/40.00 g NaOH)(1L/0.2 mol)=0.275 L

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formula for molarity and dilutions

mol/L
(M1)(V1) —–> (M2)(V2)
stock. working
concentration concentration

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how to tell if its a molarity dilution problem?

first M given is more than what you want out of it
will say “by diluting’

set up formula: “make 50 mL of a 0.05 M working solution from a 2.0 M stock solution of___”

(2.0M)(V1)/(0.05M)(0.05L)

define electrolyte and example:

ions in a solution, formed from solutes that dissociate into ions. (carry an electric current).
H2O
ex: NaCl(s) —–> Na+(aq) + Cl-(aq
1 mol. 2 mol
ONLY IONIC COMPOUND BREAK DOWN

define nonelectrolyte and example:

no ions in solution, dissolves but doesnt dissociate. (stays covalently bonded molecule)
H2O
glucose(s) ——–> glucose (aq)
1 mol. 1 mol

define strong electrolyte

dissociates virtually 100%
ex” NaCl thing

define weak electrolyte

only partially dissociates
ex: CH3COOH(aq) <====> H+(aq) + CH3COO-
EQUILIBRIUM

define acid and ex

donates H+ to solution(in water)
ex: HCl(aq) —> H+(aq) + Cl-(aq)

define base and ex

accepts H+ from solution(inH2O)
ex: NH3(aq) +H2O –> NH4+ + OH-(aq)
water acts as acid

whats acids and bases theory called

brønsted-lowry theory

describe hydronium ion when acid and bases

H+ in solution are combined with H2O to form H3O+ ex: from acid- H+(aq) + H2O(l) ---> H3O+ (aq)

describe hydrochloric acid base process

H2O(l) + HCl(aq) ---> Cl-(aq) + H3O+(aq) WATER ACTS AS BASE

define amphoteric

can behave as acid and base (WATER) (H2CO3)

define monoprotic acids and diprotic acids and how

mono- loses 1H+ di- loses 2 H+ poly exists. DI AND POLY GO THRPUGH RXN MULTIPLE TIMES TILL H IS OUT

what is the heart of all acid/base chemistry

H+(aq) + OH-(aq) ---> H2O(l)

how to solve neutralization rxn: "you spill 20.0 mL of 3.5 M HCl in lab. what volume of 5M NaOH is required to neutralize the acid?"

set up ionic equation and get net(H+ + OH- ---> H2O(l) ). use spill given(20mL) convert to L multiple by (3.5 mol HCl/1L) then do molar ratio from net (1 molH+/ 1mol HCl) and get 0.07 mol H+ take that answer as given then do molar ratio pf net (1 mol OH-/ 1 mop H+) then do another molar ratio ( 1 mol NaOH/ 1 mol OH-) and then do (1L/ 5 mol NaOH) and get 0.014 L 5M NaOH or 14 mL

define oxidation

lose of electrons gain O lose H

define reduction

gain of electrons lose O gain H

ex of redox reaction (reduction and oxidation happen simultaneously)

ANY ELEMENT YOU FIND IN NATURE = zero neutral Mg°(s) + Cl°2(g)--->Mg²+(aq) + 2Cl-(aq) Mg lost 2e-(ox) Cl gain 2e-(re) break into 1/2 rxns. Mg: Mg°(s)---> Mg²+(aq) + 2e- Cl: Cl°2(g) + 2e- ---> 2Cl-(aq)

do 1/2 redox rxns where you have to multiple so e- are same : Al°(s)+ O°2(g) --> Al2O3(s)

ox1/2:(Al°--->Al3+ +3e-) x 4 red1/2:(O°2+ 4e- --> 2O2-) x3 4Al°(s)--->4Al3+(aq) + 12e- 3O°2 + 12e- --> 6O(2-)(aq) 4Al°(s) + 3O°2 --> 4Al(3+) +6O(2-) 2Al2O0