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Chem Test 2; Ch 4
Chapter 4
55
Chemistry
Undergraduate 1
10/04/2012

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Term
A Solution is,
and made of
Definition
a homogenous mixture of 2 or more substance
made up of a solvent and a solute
Term
The solvent is?
Definition
what the solute is dissolved into
ex. water
Term
Electrolyte solutions do/do not conduct electricity?
Definition
Do
Term
Electrolyte is?
Definition
a substance that dissociates into ions when dissolved in water
Term
Nonelectrolyte is?
Definition
may also dissolve in water but will not dissociate into ions
Term
Strong electrolyte dissociates ______ when dissolved in water
Definition
Completely
Term
Strong electrolytse include?
Definition
Strong Acids
Strong bases
and Soluble ionic salts
Term
Weak Electrolytes dissociate ______ when dissolved in water
Definition
Partially
Term
Weak Electrolytes are include?
Definition
Weak acids ex. HF
Weak Bases ex. NH3
Term
Molecular compounds when they dissolve break into?
Definition
Molecules
Term
Ionic Compounds when they dissolve break into?
Definition
Cations and
Anions
they have charges
Term
2 types of electrolytes
Definition
Strong and Weak
Term
Name the strong Acids

*7*
Definition
HCl-Hydrochloric
HBr- Hydrobromic
HI- Hydroiodic
HClO3- Chloric Acid
HClO4- Perchloric
HNO3- Nitric
H2SO4- Sulfuric
Term
The Strong bases are?
Definition
Group 1A metal hydroxides and
group 2A
ex. LiOH, NaOH, KOH,RbOH
Ca(OH)2, Sr(OH)2, Ba(OH02
Term
Work
Which ions and molecules are present in aq solutions of
ZnCl2
HCl
HF
Definition
Zn 2+ and Cl-
H + and Cl-
H + and F-
Term
Precipitation reactions
Definition
reactions that result in the formation of an insoluble product ( thats the precipitate)
Term
Metathesis is?
example formula
Definition
AX + BY → AY + BX
Term
Work
Complete and balance the following reaction

Pb(NO3)2 (aq) + KI (aq) -->
Definition
Pb(NO3)2 (aq) + 2 KI (aq) --> PbI2 (s) + 2 KNO3 (aq)
Term
Work
Write the balanced net ionic equation for the reaction below
and name the spectator ions.

FeSO4 (aq) + 2 LiOH (aq) -->
Definition
Fe2+ (aq) + 2 OH-(aq) -->Fe(OH)2 (s)
Spectator ions: SO42- and Li+
Term
Acids are?
Definition
Substances that increase the concentration of H+ (proton) when dissolved in water
Proton Donors
Term
Bases are?
Definition
Substances that increase the concentration of OH− when dissolved in water
Proton acceptors
Term
A Neutralization Reaction aka? and def? and what happens?
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
Term
Work
Give the balanced (molecular) equation for the reaction between hydrobromic acid and aluminum hydroxide.
Definition
3HBr (aq) + Al(OH)3 (s)  3H2O (l) + AlBr3 (aq)
Term
Acid-Base reactions with Gas formation do what?
Definition
give a molecular compound in gaseous form
Term
Carbonates: CO32- or HCO3- give off what in gas formation?
Definition
CO2
Term
Sulfite: SO32- give off what in gas formation?
Definition
SO2
Term
Sulfide : S2- give off what in gas formation?
Definition
H2S
Term
Redox Reactions aka? Def?
Definition
Reductions-Oxidation
a reaction of electron transfer consisting of two half reactions: oxidation and reduction.
Term
L.E.O
oxidation or reduction?
Definition
Loss of Electrons
oxidation
Term
G.E.R
oxidation or reduction?
Definition
Gain of Electron
Reduction
Term
Atoms in their elemental form have an oxidation number of?
Definition
0
this includes at diatomic molecules
Term
The oxidation number of a monatomic ion ?
Definition
is the same as its charge
Term
Hydrogen is +1 when?
and -1 when?
Definition
when bonded to a metal
bonded to a nonmetal
Term
Oxygen usually has what oxidation number? and what is an exception to this rule?
Definition
usually -2
and except in the peroxides in which it has an oxidation number of −1.
Term
Fluoride oxidation number is?
and other halogens range from?
Definition
-1
-1 to +7
Term
The sum of the oxidation numbers in a neutral compound is
Definition
0
Term
The sum of the oxidation numbers in a polyatomic ion is
Definition
the charge on the ion
Term
WORK
Determine the oxidation numbers in
MnCl2
Definition
Mn = +2 ; Cl = -1
Term
WORK
Determine the oxidation numbers in
(SO4)2-
Definition
S = +6 ; O = -2
Term
WORK
Determine the oxidation numbers in
Fe2(SO4)3
Definition
Fe = +3 ; S = +6 ; O = -2
Term
WORK
Determine the oxidation numbers in
P2O5
Definition
P = +5 ; O = -2
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
Definition
Acid-base reaction
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
Definition
Redox reation
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
Definition
REdox Reaction
Term
Any Metal in the list of displacement can be oxidized by ?
Definition
ions of the elements below it.
Term
Molarity Concentration def
Definition
the amount of solute dissolved in a given quantity of solvent or solution.
Term
Molarity (M) =
formula?
Definition
Moles of solute/
(over) Volume of solution in Liters
Term
WORK
2.00 M NaCl solution contains what M of each ion?
Definition
2.00 M Na+ and 2.00 M Cl-
Term
WORK
0.025 M Ca(NO3)2 solution contains what M of each element ?
Definition
0.025 M Ca2+ and 0.050 M NO3-
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
Definition
0.626 M K2CO3 solution
Term
WORK
How many grams of potassium carbonate are there in 35.0 mL of a 1.25 M K2CO3 solution
Definition
6.05 g K2CO3
Term
WORK
How many mL of a 1.25 M K2CO3 solution are needed to provide 0.110 mol of K2CO3
Definition
88.0 mL 1.25 M K2CO3 solution
Term
WORK
How many mL of 1.25 M K2CO3 are needed to dilute this solution to 100. mL 0.45 M?
Definition
36.0 mL 1.25 M K2CO3 solution
Term
Dilution formula?
Definition
Moles of solute before dilution = Moles of solute after dilution

Mconc x Vconc = Mdil x Vdil
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.
Definition
-0.864 M NaOH solution
-3.45 g NaOH
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