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Chemistry Module 2 > Chapter 4 Acids and redox > Flashcards

Chapter 4 Acids and redox Flashcards

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1
Q

What are acids

A
  • When dissolved in water an acid releases hydrogen ions a protonss H+ into the solution
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2
Q

what is a strong acid

A
  • releases all it’s hydrogen atoms into solution as H+ ion and completley dissociates in an aqueous solution
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3
Q

What is a weak acid

A
  • only releases a mall propertion of it avilable hydrogen atoms into solution as H+ ions
  • partially dissociates in an aqueous solution
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4
Q

What are the four common acids

A
  • hydrochloric acid - HCl
  • sulfuric acid - H2SO4
  • nitric aci - HNO3
  • ethanoic acid - CH3COOH
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5
Q

What are the four common bases

A
  • metal oxides
  • metal hydroxides
  • metal caarbonates
  • ammonia
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6
Q

What is a base

A
  • neutralie an acid to form a salt
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7
Q

What is an alkali

A
  • a base that dissolved in water releasing hydroxide ions OH- into the solution
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8
Q

What are 3 example of alkalis

A
  • NaOH
  • KOH
  • NH3
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9
Q

What is a neutralisation reaction

A
  • H+ ions (aq) ions from the acid react with a base to form a salt and neutral water
  • H+ ions are replaced by metal of ammonium ions from the base
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10
Q

What are the type of salts formed from the 4 common acids

A
  • hydrochloric acid - chloride
  • sulfuric acid - sulfate
  • nitric acid - nitrate
  • ethanoic acid - ethanoate
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11
Q

Describe the neutralisation reaction between acid and metal oxide and hydroxides

A
  • form salt and water
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12
Q

Describe the ionic equation for a neutralisation reaction

A
  • H+(aq)+OH-(aq) -> H2O(l)
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13
Q

What is formed when an alkali reacts with an acid

A
  • salt and water
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14
Q

Describe the neutralisation reaction between acids and carbonates

A
  • form salt water and carbon dioxide
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15
Q

What is a titration

A
  • ued to accuratley meaure the volume of a solution that reacts exactly with another volume
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16
Q

What are titrations used for

A
  • finding the concentration of a solution
  • identification of an ynknown chemical
  • finding the purity of a substance - important in medicines ,food and cosmetics
17
Q

What is a concordant result

A
  • results are within 0.1cm3 of each other
18
Q

Decribe how you would prepare a standard solution

A
  • solid weighed accuratley
  • solid is dissolved in a beaker using less distilled water than will bed needed to fill the volumetric flask to the mark
  • this solution is transferred to a volumetric flask the last traces of solution is rinsed into a flask with distilled water
  • flask carefully filled to the graduation line by adding distilled water a drop at a time yntil meniscus lines up exactly with the mark
  • add stop and invert volumetric flask several times to mix up the solution - if not done titration will not be consistent
19
Q

Describe the acid base titration procedure

A
  • add a meaured volume of one solution to a conical flask using a pipette
  • add the other solution to a burette and record intial burette reading nearest 0.05 cm3
  • add a few drop o indication in concial flak
  • run solution in burette into the solution in the conical flak swirling throughout until indicator change to enf point
  • record the final burette reading
  • trial titration carried out firt
  • then titration is repeated until two accurate titres are concordant
20
Q

Decribe the error of the pipette having an air bubble

A

the air could be releaed during titration leading to an error

21
Q

What is an oxidation number

A
  • baed on the set of rules that apply to atoms
  • as the numner of electrons involved in bonding to a different element
22
Q

What are the oxidation rules for elements

A
  • zero for elements
  • each atom in a compound ha an oxidation number
23
Q

What are special case of oxidation numbers

A
  • H in metal hydrides - -1-NaH,CaH2
  • O in peroxides - -1-H2O2
  • O bonded to F - +2-F2O
24
Q

What are redox reactions

A

involves both reduction and oxidation

25
Q

What is reduction

A
  • gain of electrons
  • decrease in oxidation number
26
Q

What is oxidation

A
  • loss of electrons
  • increase in oxidation number

Chemistry Module 2 (5 decks)

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