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Chemistry 1 > Solution chemistry > Flashcards

Solution chemistry Flashcards

(58 cards)

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1
Q

What is molarity equivilent to?

A

Concentraition

1M = 1mol/dm3

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2
Q

What is Molality

A

Mols of solute / kg of solvent

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3
Q

How to solve for molality

A
  1. use the conc. as moles per dm3
  2. find m(solvent)per dm3 with Mr
  3. m(solute) = m(solution)-m(solvent)

Everything must be done by per dm3 or kg

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4
Q

Define ppm

A

m(solute)/m(solvent) x10^6

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5
Q

Defintion of pH and pOH

A

pH = -log10[H+]
pOH = -log10[OH-]

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6
Q

pKw equation

A

pKw = pH + pOH

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7
Q

What is water self-ionisation?

Does it tend to matter?

A

water dissociates into hydronium ion and hydroxide ion

dsm as it is very insignificant compared to acid and base dissociation

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8
Q

How to verify water self ionisation is negligible?

A

Use the [H+] or [OH-] value calculated and sub into Kw expression to find counter [OH-] or [H+] formed and compare magnitude

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9
Q

3 ways of defining an acid

A
  1. produce H+
  2. proton donor
  3. electron pair acceptor
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10
Q

3 ways of defining a base

A
  1. OH- produced when dissociates
  2. proton acceptor
  3. electron pair donor
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11
Q

How to find pKa / pKb of conjugate acid or base when given pKb or pKa

A

pKa + pKb = pKw
Kw=Ka x Kb

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12
Q

Ka expression

A
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13
Q

Kb expression

A
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14
Q

Factor affecting acid strength

(for hydrohalide acid)

+4 points of explanation

A

Electronegativity of halide

  1. More EN
  2. greater energy dissymetry
  3. easier to undergo homolytic splitting
  4. easier to dissociate
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15
Q

3 factors that affects strength of oxo acid

A
  1. electronegativity of centre atom
  2. EN of atoms bonded to centre
  3. No. of extra oxygen on OXO acid
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16
Q

How does the EN of atoms in oxoacid affect strength

A
  1. More EN
  2. pulls electron density from the oxygen bonded to H
  3. increase energy dissymetry (poor overlap)
  4. makes hetrolytic cleavage easier
  5. hence more likely to dissociate
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17
Q

3 Assumptions in
acid calculation

A
  1. Only monoprotic present - further dissociation is negligible
  2. Change in acid conc. is negligible
  3. Water self-ionisation is negligible
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18
Q

How to check whether [HA] eqm = [HA] initial

A

400 x Ka < [HA]

then TRUE

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19
Q

How to ensure further dissociation is insignificance

A

Ka of further dissociation is 3 SF smaler than Ka of 1st dissociation

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20
Q

What happens when [HA]eqm does not equal initial

A

[HA]eqm = [HA]initial - [H30+]

solve quadratic

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21
Q
A
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21
Q

How to solve for [HA] at eqm

after finding [H30+]

A

Material balance

[HA]eqm = [HA]i - [all conjugate acid formed]

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22
Q

How to solve for further dissociation products

A

Assume:
1. hydroxide/hydronium ion contribution is insignificant
2. change in 1st dissociation product is negligible

Ka2 = [A2-]
Kb2 = [BH2 2+]

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23
Q

What does speciation diagram tell

Study These Flashcards
A

relative proportion of the polyprotic acid and conjugate base species present at different pH

At low pH - no dissociation
At high pH - full dissociation

24
crucial properties of a salt
electrically neutral product
25
What do cation and anion do when dissociates in solution
Treating as lewis acid and base Cation - acts as acid (accept e pair) Anion - acts as base (donates e pair)
26
How to find Ka or Kb of a conjugate species
Kw = Ka x Kb
27
1. when does acidic salt form 2. what happens in solution
1. strong acid and weak base 2. **Anion** formed from the base **becomes a strong acid** 3. Eqm shifts in sol. to reform base **Treat as an acid hydrolysis**
28
1. when does base salt form 2. what happens in solution
1. Weak acid and strong base 2. **cation** formed from acid **becomes strong base** 3. Eqm shifts in sol. to reform acid **Treat as an base hydrolysis**
29
Rules for cation that influences salt's pH | 6 examples
Strong acid's conjugate base - no effect * HClO4 * HNO3 * HCl * H3O+ Strong base - has effect * OH- * NH2-
30
What does hydrated metal ion acts as in solution? What metal ions work?
1. form complex ion 2. energy dyssymetry - weakens OH bonds for dissociation Only high charge density can cause shift in e density Be - with small ionic radi so high Q density Group 3 - 3+ charge
31
Define Ksp
Deg. at which a substance dissolve in a particular conditon and solvent
32
Method of solving solubility of a subtance in solvent
solubility = conc. of substance 1. form Ksp expression with stoichiometry 2. convert all the conc. to one species **by their stiochiometry - they are not the same**
33
What is the common ion effect and what is the effect on solubility
* When salt MX is added to a solution containing salt MY * Both contain metal ion M * causes dissociation eqm to shift to LHS to oppose inc. * limiting solubility of salt MX
34
How to solve for solubility (common ion effect present)
1. form Ksp expression 2. do ICE balance 3. solve for change in conc. using Ksp expression
35
What is the consecutive ion hydrolysis | + example anion that works
* When the anion undergoes hydrolysis * reduce conc. of anion * allow further dissociation of the salt * inc. solubility E.g. anion : anion formed from diprotic acid dissociation SO32- , PO4 2- , CO32-
36
What is Q or IP
ionic product The Ksp at the exact moment of the experiment
37
What is Ksp
The **Maximum** dissociation product in the **saturated** solution
38
What happens when: * Q < / = / > IP
39
How to find Q | ionic product
Find the individual concentration of the ion present in the solution then sub into the Ksp expression to find the Q
40
What is selective p.p. + What is it for?
* delibrately forming insoluble salt * to seperate 2 salts with different Ksp
41
what happens when pKa = pH
conjugate acid and base are in equal concentration
42
Equivalence point
Theortical volume at which n(base) =n(acid)
43
How to calculate points on titration curve
* Find the moles of acid/base added * Subtract it to the moles of acid/base in cylinder * find the temperary conc. of each species (note change as an unknown x) * ICE balance - how eqm shifts
44
What is the role of buffer
resist pH
45
composition of a acid buffer
weak acid + conjugate base in salt form
46
composition of base buffer
weak base conjugate acid in salt form
47
Factors to consider when designing a buffer
1. must have a conjugate pair 2. must have a weak acid/base 3. ratio of the conjugate pair 4. target pH we want
48
HH equation | for calculating buffers
49
Steps to designing the buffer solution
1. Decide the conjugate pair [pKa as close to pH desired] 2. Decide the ratio of the pair in solution [use HH eq to adjust to exact conc.]
50
Why does hydrated metal ion form complex ion
**Lewis acid and base interaction** * metal = lewis acid (e deficient) * water = lewis base (donate lone pair)
51
What's the compex ion eqm? and its effect
1. complex ion is a more stable the metal ion itself 2. allow further dissolution of the salt
52
Why would we introduce ligands to inc. dissolution
1. Inc. dissolution 2. avoid p.p. forming
53
Define Kf
54
new overall constant | after complex ion eqm
Kc = Ksp x Kf
55
What is ligand exchange? Why does it happen?
1. when a stronger lewis base is present 2. e.g. NH3 3. sub out water ligand in the complex
56
Factors affecting Kf | for central ion
More stable: 1. smaller cation size 2. larger charge
57
Chelate effect
* Greater denticity of ligands in complex * more stable the complex * greater Kf

Chemistry 1 (5 decks)

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