Term
A Solution is,
and made of |
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Definition
a homogenous mixture of 2 or more substance
made up of a solvent and a solute |
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Term
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Definition
what the solute is dissolved into
ex. water |
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Term
| Electrolyte solutions do/do not conduct electricity? |
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Definition
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Term
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Definition
| a substance that dissociates into ions when dissolved in water |
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Term
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Definition
| may also dissolve in water but will not dissociate into ions |
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Term
| Strong electrolyte dissociates ______ when dissolved in water |
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Definition
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Term
| Strong electrolytse include? |
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Definition
Strong Acids
Strong bases
and Soluble ionic salts |
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Term
| Weak Electrolytes dissociate ______ when dissolved in water |
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Definition
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Term
| Weak Electrolytes are include? |
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Definition
Weak acids ex. HF
Weak Bases ex. NH3 |
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Term
| Molecular compounds when they dissolve break into? |
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Definition
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Term
| Ionic Compounds when they dissolve break into? |
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Definition
Cations and
Anions
they have charges |
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Term
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Definition
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Term
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Definition
HCl-Hydrochloric
HBr- Hydrobromic
HI- Hydroiodic
HClO3- Chloric Acid
HClO4- Perchloric
HNO3- Nitric
H2SO4- Sulfuric |
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Term
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Definition
Group 1A metal hydroxides and
group 2A
ex. LiOH, NaOH, KOH,RbOH
Ca(OH)2, Sr(OH)2, Ba(OH02 |
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Term
Work
Which ions and molecules are present in aq solutions of
ZnCl2
HCl
HF |
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Definition
Zn 2+ and Cl-
H + and Cl-
H + and F- |
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Term
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Definition
| reactions that result in the formation of an insoluble product ( thats the precipitate) |
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Term
Metathesis is?
example formula |
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Definition
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Term
Work
Complete and balance the following reaction
Pb(NO3)2 (aq) + KI (aq) --> |
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Definition
| Pb(NO3)2 (aq) + 2 KI (aq) --> PbI2 (s) + 2 KNO3 (aq) |
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Term
Work
Write the balanced net ionic equation for the reaction below
and name the spectator ions.
FeSO4 (aq) + 2 LiOH (aq) --> |
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Definition
Fe2+ (aq) + 2 OH-(aq) -->Fe(OH)2 (s)
Spectator ions: SO42- and Li+ |
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Term
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Definition
Substances that increase the concentration of H+ (proton) when dissolved in water
Proton Donors |
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Term
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Definition
Substances that increase the concentration of OH− when dissolved in water
Proton acceptors |
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Term
| A Neutralization Reaction aka? and def? and what happens? |
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Definition
Acid-Base
A neutralization reaction between an acid and metal hydroxide produces a salt and water
the acid donates a proton (H+) to the base |
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Term
Work
Give the balanced (molecular) equation for the reaction between hydrobromic acid and aluminum hydroxide. |
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Definition
| 3HBr (aq) + Al(OH)3 (s) ï‚® 3H2O (l) + AlBr3 (aq) |
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Term
| Acid-Base reactions with Gas formation do what? |
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Definition
| give a molecular compound in gaseous form |
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Term
| Carbonates: CO32- or HCO3- give off what in gas formation? |
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Definition
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Term
| Sulfite: SO32- give off what in gas formation? |
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Definition
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Term
| Sulfide : S2- give off what in gas formation? |
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Definition
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Term
| Redox Reactions aka? Def? |
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Definition
Reductions-Oxidation
a reaction of electron transfer consisting of two half reactions: oxidation and reduction. |
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Term
L.E.O
oxidation or reduction? |
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Definition
Loss of Electrons
oxidation |
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Term
G.E.R
oxidation or reduction? |
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Definition
Gain of Electron
Reduction |
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Term
| Atoms in their elemental form have an oxidation number of? |
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Definition
0
this includes at diatomic molecules |
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Term
| The oxidation number of a monatomic ion ? |
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Definition
| is the same as its charge |
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Term
Hydrogen is +1 when?
and -1 when? |
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Definition
when bonded to a metal
bonded to a nonmetal |
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Term
| Oxygen usually has what oxidation number? and what is an exception to this rule? |
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Definition
usually -2
and except in the peroxides in which it has an oxidation number of −1. |
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Term
Fluoride oxidation number is?
and other halogens range from? |
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Definition
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Term
| The sum of the oxidation numbers in a neutral compound is |
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Definition
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Term
| The sum of the oxidation numbers in a polyatomic ion is |
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Definition
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Term
WORK
Determine the oxidation numbers in
MnCl2 |
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Definition
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Term
WORK
Determine the oxidation numbers in
(SO4)2- |
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Definition
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Term
WORK
Determine the oxidation numbers in
Fe2(SO4)3 |
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Definition
| Fe = +3 ; S = +6 ; O = -2 |
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Term
WORK
Determine the oxidation numbers in
P2O5 |
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Definition
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Term
WORK
Redox reaction or not ? Which element is oxidized and which
reduced in case of a redox reaction?
-The reaction between hydrobromic acid and sodium hydroxide |
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Definition
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Term
WORK
Redox reaction or not ? Which element is oxidized and which
reduced in case of a redox reaction?
-The reaction between hydrobromic acid and zinc under formation of hydrogen gas and and zinc bromide |
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Definition
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Term
WORK
Redox reaction or not ? Which element is oxidized and which
reduced in case of a redox reaction?
-The reaction between silver nitrate and copper under formation of silver and copper(II) nitrate |
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Definition
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Term
| Any Metal in the list of displacement can be oxidized by ? |
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Definition
| ions of the elements below it. |
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Term
| Molarity Concentration def |
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Definition
| the amount of solute dissolved in a given quantity of solvent or solution. |
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Term
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Definition
Moles of solute/
(over) Volume of solution in Liters |
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Term
WORK
2.00 M NaCl solution contains what M of each ion? |
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Definition
| 2.00 M Na+ and 2.00 M Cl- |
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Term
WORK
0.025 M Ca(NO3)2 solution contains what M of each element ? |
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Definition
| 0.025 M Ca2+ and 0.050 M NO3- |
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Term
WORK
Calculate the molarity of a solution made by dissolving 8.65 g of K2CO3 in enough water to form a 100. mL solution |
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Definition
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Term
WORK
How many grams of potassium carbonate are there in 35.0 mL of a 1.25 M K2CO3 solution |
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Definition
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Term
WORK
How many mL of a 1.25 M K2CO3 solution are needed to provide 0.110 mol of K2CO3 |
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Definition
| 88.0 mL 1.25 M K2CO3 solution |
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Term
WORK
How many mL of 1.25 M K2CO3 are needed to dilute this solution to 100. mL 0.45 M? |
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Definition
| 36.0 mL 1.25 M K2CO3 solution |
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Term
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Definition
Moles of solute before dilution = Moles of solute after dilution
Mconc x Vconc = Mdil x Vdil |
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Term
WORK
43.21 mL of 0.250 M H2SO4 is required in a titration to neutralize 25.00 mL NaOH solution
-Calculate the concentration of NaOH.
-Calculate the mass (g) of NaOH needed to prepare 100.0 mL NaOH solution. |
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Definition
-0.864 M NaOH solution
-3.45 g NaOH |
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