Exam 2 Flashcards by Gabrielle Carter

Is the solute normally lesser or greater?

lesser

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Is the solvent normally lesser or greater?

greater

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Under what conditions does a solute dissolve?

solute-solvent attraction > solute-solute attraction

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hydrated ions

when positive and negative are separated and surrounded by water molecules

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solvation

process of solute and solvent molecules interacting

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hydration

when the solvent is water

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water is a ___ molecule

polar

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three characteristics of water

uneven electron distribution
bent molecular shape
dissolves most substances

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van der Waals forces

forces between neutral molecules

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London dispersion forces

temporary attractive force that results from the electrons of two adjacent atoms occupying positions where the atoms form temporary ‘induced’ dipoles.
-weakest van deer waal force

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dipole-dipole forces

between positive end of one polar molecule and the negative end of another polar molecule
-can be repulsive

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hydrogen bond forces

H (partially positive) and lone pair

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ion-dipole forces

attraction that results from the electrostatic attraction between an ion and a neutral molecule

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molecules with similar intermolecular forces are most likely ____ to one another

soluble

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immiscible

when liquids do not mix

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water and ethanol are ____.

miscible

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water and gasoline are ____.

immiscible

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gasoline and CCl4 are ____.

miscible

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is non polar covalent hydrophobic or hydrophilic?

hydrophobic

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are polar covalent and ionic compounds hydrophilic or hydrophobic?

hydrophilic

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Are hydrocarbons polar or non polar?

non polar

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polar and ionic substances dissolve best in ____.

polar solvents

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non polar substances dissolve best in _____.

non polar substances.

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electrolyte

contain ions when in an aq solution
-conduct electricity

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non electrolyte

does not form ions when in an aq solution.

strong acids and bases do what in water?

completely ionizes

HCl is a ___ and ___.

strong acid, strong electrolyte

acetic acid is a ___ and ____.

weak acid (ionizes slightly), weak electrolyte

ionic compounds are usually ____.

strong electrolytes

ionic compound

ions held together by ionic bonding.

Hbr is a ___.

strong acid

HI is a ___.

strong acid

HNO3 is a ___.

strong acid

H2SO4 is a ___.

strong acid

HClO3 is a ____.

strong acid

HClO4 is a ___.

strong acid

NaOH is a ___.

strong base

KOH is a ___.

strong base

Ca(OH)2 is a ____.

strong base

molecular (covalent) compounds, with the exception of acids and bases, are ___.

nonelectrolytes

dissociation

when ionic compounds dissolve in water and the anions and cations separate from each other.

When acids dissolve in water the molecule ionizes into __ and ____.

H+, anions

When something is highly soluble, the original compound can still be found in small amounts.

true

Does AgCl dissolve in water?

only slightly, leaves white powder.

unsaturated solution

when more solute can be added to the solvent and the solute will still dissolve

saturated solution

when more solute is added than will dissolve (solubility limit has been reached)

Solubility

maximum amount of solute that will dissolve in a specific amount of solvent at a given temp. (mol/L)

a compound is soluble than it ___.

dissolves in water.

>0.1M

soluble

<0.01M

insoluble

>0.01M but <0.1M

partially soluble

When two soluble solutions are mixed, they may form an insoluble compound and a ____.

precipitate

Nitrate (NO3-) and acetate (C2H3O2-) are ___.

soluble

Alkali metal (first row) and ammonium (NH4+) salts are ___.

soluble

Most Cl-,Br-, and I- salts are ___ except __,__, and ___.

soluble, Ag+,Pb2+,Hg2(2+)

most sulfates (SO42-) are ____ except __,___, and ___.

soluble, Ca2+,Sr2+, and Ba2+, Ag, Pb

Most hydroxides (OH-) are ___ except

insoluble, Na,K, Li, NH4+

What hydroxides are partially soluble?

Ba2+,Sr2+,Ca2+

S2- is ___, unless with ___.

insoluble, Li,Na,K,NH4+,Ca,Sr,Ba

CO32- is ___.

insoluble

CrO42- is ____.

insoluble

Cr2O72- is ____.

insoluble

PO43- is ____.

insoluble -except with alkali metal cations, NH4+

soluble when combined with anions

Li+,Na+,K+,NH4+

Carbonate (CO32-) and phosphate ions (PO43-) ions are usually ____ unless with ____.

insoluble, Li,Na, K, NH4+

The solubility of one substance in another varies with ___ and ___.

temp, pressure

For most ionic substances, solubility in water ____ as temp ____.

increases, increases

The solubility of gases ___ with temperature

decreases

Even insoluble solids will dissociate a little.

true.

Acetic acid is a __ and ___.

weak electrolyte, very soluble.

Concentration

amount of solute in a total volume of solution

Molarity

amount of solute (mol)/volume of soln (L)

dilution equation

M1V1=M2V2

moles =

mass / molar mass

combustion reaction

substance and oxygen reacting

A reaction between ions in aq solution can form:

another solid, a gas, or a liquid

precipitation reactions are

double displacement reactions

molecular equation

complete chem formula with states.

total ionic equation

all soluble ionic substances are represented by the ions they form in solution.

net ionic equation

same as total ionic (ions) but has spectator ions removed.

binary acids

acid hydrogens attached to a nonmetal atom. Ex: HCl

oxyacids

acid hydrogens attached to an oxygen atom (H2SO4)

acid produces ___.

H+ (A)

bases produces ___.

OH- (A)

Acid is a ___.

H+ donor (B-L)

Base is a ___.

H+ acceptor (B-L)

pH < 7.0

acid

The molarity of H3O in the solution determines the ___.

two arrows in an equation represents?

equilibrium -usually a weak electrolyte

HF is a

weak acid

HNO2 is a

weak acid

HClO is a

weak acid

CH3COOH is a

weak acid

bases can be __ or ___

ionic or covalent

LiOH is a

strong base

NaOH is a

strong base

KOH is a

strong base

RbOH is a

strong base

CsOH is a

strong base

Ca(OH)2 is a

strong base

Sr(OH)2 is a

strong base

Ba(OH)2 is a

strong base

NH3 is a

weak base

Fe(OH)2 is a

weak base

amines are ___ and they are ____.

molecules with C-N in them, weak bases

pH =

-log[H3O+]

[H3O+]=

10^-pH

pOH=

-log[OH-]

pH + pOH =

when an acid and base are combined

water is formed and a salt (ionic) (neutralization reaction)

acid/base titrations are based on

the neutralization reaction

the titrant or standard solution

solution being added from buret

end point (titration)

point in titration where there is a physical change of the solution

indicator

changes physically near the equivalence point

equivalence point (titration)

Exam 2 Flashcards

(115 cards)