Oceans(O) Flashcards

1
Q

Define acid and base

A

Acid=substance which donates H+ in a chemical reaction
Base=substance which accepts H+ in a chemical reaction

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2
Q

What is the equation for the dissociation of an acid?

A

HA—–>H+ and A-

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3
Q

What is a conjugate base or acid?

A

A conjugate base means it is able to accept H+ after the reaction has occured

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4
Q

What is pH?

A

A measurement of hydrogen ions (H+) in a substance

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5
Q

Why is done this way

How is the pH of a strong acid calculated?

A

-log(H+)
The amount of moles pf H+ ions is equal to the amount of acid (HA) put into solution

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6
Q

Which equation(s) is used to the pH of a weak acid?

A

Ka=[H+] [A-]/[HA]

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7
Q

What assumptions are used to calculate the pH of a weak acid?

A
  • [H+]=[A-]
  • amount/moles of [HA] at eqm is equal to the amount/moles of [HA] put in
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8
Q

How does pH affect pKa

Why is pKa used and what is the equation?

A

pKA is used when the Ka values is very small
pKa=-log(Ka)
Weaker the acid the higher the pKa value

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9
Q

What equation is used to calculate the pH of a strong base?

A

[H+]= Kw(1x10(-14)) x [OH-]
-log(H+)

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10
Q

Define buffer

A

Solutions that can resist changes in pH, despite the addition of small quantities of acid or alkali

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11
Q

How do buffers work?

A

They remove the majority of any acid or alkali added to the solution

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12
Q

Two types

What are buffers usually made up of?

A
  • A weak acid and one of its salts
  • A weak base and one of its salts
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13
Q

What are the two assumptions that the action of buffers is based on?

A
  1. All the anions come from the salt
  2. Almost all the acid molecules put into the buffer remain unchanged
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14
Q

How do you calculate the pH of a base?

A

[H+]=Ka x acid/salt

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15
Q

Define lattice enthalpy

A

The enthalpy change when 1 mole of an ionic lattice is formed from its gaseous ions under standard conditions
It is always negative~because bonds are fomed

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16
Q

Define enthalpy of hydration

A

The enthalpy change for the formation of a solution of ions

17
Q

Define charge density

A

A measure of ionic radius and ion’s charge. This depends on two factors:ionic charge and ionic radii

18
Q

How do you convert solubility in g dm-3 into mol dm-3?

A

Divide by the molar mass

19
Q

What is Ksp and give its formula?

A

Solubility product
This is the sum of the products

20
Q

What is the difference between strong acids and weak acids?

A

Strong acids dissociate almost completely in water~nearly all hydrogen ions are released
Weak acids only partially dissociate in water~Eqm is set up which iswell over to the left

21
Q

What happens to equilibrium when you add more acid or base to an acid-base reaction?

A

Eqm moves to the right

22
Q

What equation is used to calculate the pH of a strong base?

A

Kw=[H+][OH-]

23
Q

How is pKa calculated?

24
Q

Define a buffer solution

A

A solution a change in pH when small quantities of acid or base are added

25
Q

How are acidic buffers made?

A

A weak acid and one of its salts

26
Q

Why are buffers important in human cells?

A

Enzymes work at optimum pH if there is a signifcant change in pH it may lead to bonds within the enzyme breaking. Preventing the enzymes from working

27
Q

What happens to the position of equilibrium when an acid is added to a buffer?

A

H+ concentration increases
Majority of H+ combines with an ion from the acid’s salt
Eqm shifts to the left=Reduces H+ concentration

28
Q

How is the pH of a buffer solution calculated?

A

Ka=[H+][Salt]/[Acid]
[H+]=Ka x [Salt]/[Acid]