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Chem 101 🙃 > 🥰 > Flashcards

🥰 Flashcards

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1
Q

Normal neural binary acids

A

H - hydro

Then end in ic

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2
Q

Polyatomic anions

A

H- nothing

If ion ends in ate then ic acid
If ion ends in ite then us acid

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3
Q

Arrhenius acid and base

A

Acid : increases h+
Base : increases OH-

Equation

Acid : HNO3 -> H+ + NO3-
Base : NaOH -> Na+ + OH-

Acid + base —> water + salt
HCl + NaOH —-> H2O + NaCl

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4
Q

Bronsted Lowry acid and base

A

Acid : proton donor
Base: proton acceptor

Equation

Hcl+ H2O —> H3O + cl-

Reaction doesn’t need to happen in water
A reaction with water is called hydrolysis

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5
Q

How to write neutralization reaction containing an acid and base containing oh-

A

Forms water and a salt

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6
Q

Titrant

A

Reagent of known concentration

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7
Q

Titration

A

Titration
A chemical reaction used to determine the exact amount of a reagent

Titrant is carefully added to a known volume of analyte to find the equivalence point which can be used to find the concentration

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8
Q

Analyte

A

Reagent of unknown concentration

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9
Q

Equivalence point

A

Equivalence point is when all the analyte has been reacted with the Titrant

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10
Q

Purpose of indicator

A

Is to determine the equivalence point

Turns colors to know that the reaction is done

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11
Q

Strong acids

A 
HCl
Hbr
HI
HNO3
H2SO4
HCLO4
HCLO3
Are irreversible and completely dissociate
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12
Q

Strong bases

A 
LioH
NaOH
KOH
RbOH
CsOH
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13
Q

Strong and weak acid or base

A

Strong acid / base completely separates when places into a solution

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14
Q

Equilibrium constant for acid or base

A

Ka(acid) = (h30)(products)/reactants
Don’t include water !!!!!

Ka * Kb= 1x10^-14

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15
Q

Kw

A

Auto ionization of water
H20 + H2O -> H3O + OH

Kw= H3O x OH-= 1.0 x10^-14

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16
Q

Ph scale and calculations

A 
pH=-log (H3O)
H+= 10 ^-pH
pOH= -log(OH)
OH= 10^-pOH
pH + pOH= 14
H+ x OH- = 1x10-14

Increase of 1 ph = 10 x increase of h+

Ph and pOH = 7 is neutral
pH<7 acidic pOH>7
pH>7 basic pOH<7

17
Q

2 components of the buffer

A

Weak acid and conjugate base (in the form of a soluble salt)

Resistís dramatic changes in pH

18
Q

Intermolecular forces
London dispersion factor
Dipole dipole
Hydrogen binding

A

London - all molecules (vanderwalls) induced dipole (larger the stronger)

Dipole dipole - only polar molecules
Permanent dipoles

Hydrogen binding :H bound to O N or f atom and interact with one of the 3

London < dipole < hydro

19
Q

Melting and boiling point trends

A

The stronger the IMF the higher the melting / boiling point

If it a positive number it is endothermic

If it is negative it would be exothermic

20
Q

Fusion

A

Melting

Solid to liquid

21
Q

Solidification

A

Freezing

Liquid to solid

22
Q

Vaporization

A

Liquid to gas

23
Q

Condensation ☁️

A

Gas to liquid

24
Q

Sublimation

A

Solid to gas (dry ice)

25
Q

Deposition

A

Gas to solid

26
Q

Heat of fusion

A

Delta Hfus = amount of energy needed to change from a liquid to a solid

Appeintly there is a direct correlation between enthalpy of fusion and the streagth of the imfs

27
Q

Heat of vaporization

A

Delta H Vap amount of energy needed. For a liquid to become a gas

Increase with increase IMF for both

28
Q

Hearing and cooling curve

A

Draw out know

Trends as energy increases heat also increases if it is not in a transition state if at a transition state energy is being used to transition meaning heat will platou

29
Q

Exothermic vs endothermic

A

Right to left is endothermic

Left to right is exothermic

30
Q

Acids vs bases characteristics

A 
Acids 
Turn litmus red
Give off h2 gas with some metals 
React with carbonate and bicarb salts to give off co2
Have a sour taste

Bases
Turn litmus blue
Are slippery to the touch
Have a bitter flavor

31
Q

Conjugate acid base pare

A

Differ only by one proton
H20 acid OH conjugate base

Water is amphiprotic meaning it can be an acid or a base

32
Q

Delta h sub

A

Enthalpy of sublimation

Is the energy needed to take a solid to a gas and is equal to delta h fus + delta h vap

Chem 101 🙃 (6 decks)

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