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Chemistry > acid base equilibria > Flashcards

acid base equilibria Flashcards

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1
Q

Properties of acid solutions

A 
produces H+ ions in water
taste sour
corrode metals
electrolytes
react with bases to form a salt and water
pH less than 7
turns blue litmus paper red
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2
Q

Properties of base solutions

A 
produce OH+ ions in water
taste bitter, chalky
feel soapy, slippery
electrolytes
react with acids to form salts and water
pH greater than 7
turns red litmus paper blue
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3
Q

Acid-base reactions

A

acids can be either strong or weak

a strong acid is a strong electrolyte

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4
Q

common strong acids

A

hydrochloric acid
nitric acid
sulfuric acid

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5
Q

common weak acids

A

methanoic acid
ethanoic acid
nitrous acid

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6
Q

acids react with metals

A

metal + acid –> salt + hydrogen

react with certain metals to produce hydrogen gas

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7
Q

acids react with carbonates

A

acid + carbonate –> salt + water + carbon dioxide

react with carbonates and bicarbonates to produce carbon dioxide gas

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8
Q

common bases

A 
sodium hydroxide
potassium hydroxide
barium hydroxide
magnesium hydroxide
lithium hydroxide
calcium hydroxide
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9
Q

Definition of acids

A

substances that when dissolved in water increase the concentration of H+ ions

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10
Q

Definition of bases

A

substances that when dissolved in water increase the concentration of OH- ions.
problem: some bases don’t have hydroxide ions

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11
Q

What is a Bronsted-Lowry acid?

A

proton donor

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12
Q

What is a Bronsted-Lowry base?

A

proton acceptor

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13
Q

H+ ion in water

A

a proton is just a hydrogen atom that has lost its electron
the interaction of a proton with water leads to the formation of the hydronium ion (H3O+)
chemists use H+ and H3O+ interchangeably to represent the same thing; namely the hydrated proton which is responsible for an aqueous acids properties

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14
Q

Non-aqueous reactions

A

HCl acts as the acid in this reaction and ammonia acts as a the base
an acid and a base always work together to transfer a proton

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15
Q

Kastle meyer test

A

phenolphthalein and hydrogen peroxide
haemoglobin acts as peroxidase - accelerates oxidation with peroxide
presumptive: potatoes and horseradish also give positive test

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16
Q

dissociation

A

strong acids completely dissociate in water. their conjugate bases have a very small tendency to accept protons in aqueous solution
weak acids only partially dissociate in aqueous solutions. they exist as a mixture of acid molecules and their constituent ions

17
Q

pH scale

A

molar conc of H+ ions in aqueous solution is very small. we usually express [H+] in terms of pH
the pH scale is a way of expressing the strength of acids and bases
acidic and basic are two extremes that describe chemicals. similarly hot and cold are two extremes that describe temperature
mixing acids and bases can cancel out the extreme effects

18
Q

pH

A

in neutral water the conc of H+ and OH- must be equal. their value is 10-7 moldm-3 at 25 degrees so that
Kw=10-7 x 10-7
= 10-14 mol2dm-6

19
Q

How is pH defined for practical purposes?

A

pH= -log10[H+]

20
Q

pH to concentration

A

10-pH

21
Q

the other p scale

A

since acids and bases are the opposite of each other; we express the conc of OH- as pOH
pOH doesnt really exist but it is convinient for changing the bases to pH
pOH = -log[OH-]
pH + pOH = 14 at 25 degrees

22
Q

pOH calculation

A 
the OH- ion conc of a blood sample is 2.35 x 10-7 M
what is pH of blood?
pOH= -log[2.35 x 10-7] = -(-6.63) = 6.63
pH = 14-pOH = 14 - 6.63
=7.37
23
Q

strong acids

A

strength of an acid dependent on the extent of ionisation
a strong acid is 100% dissociated in water
HCL + H20 –> H30+ + CL-

24
Q

what is a strong base

A

a base that is completely dissociated in water

25
Q

weak acid and base

A

weak acids and bases are less than 100% ionised in water
acetic acid is a well known weak acid
ammonnia is a well known weak base

Chemistry (2 decks)

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