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Chemistry 🌺 > Module 2: Acids & Redox > Flashcards

Module 2: Acids & Redox Flashcards

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1
Q

What is the formula of hydrochloric acid?

A

HCl

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2
Q

What is the formula of sulphuric acid?

A

H2SO4

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3
Q

What is the formula of nitric acid?

A

HNO3

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4
Q

What is the formula of ethanoic acid?

A

CH3COOH

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5
Q

What is the formula of phosphoric acid?

A

H2PO4

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6
Q

What is the formula of ammonia?

A

NH3

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7
Q

What is the formula of an ammonium ion?

A

NH4+

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8
Q

Define the term ‘hydrogen ion’

A

-Known as a proton as it has no electrons on its outer shell
-Commonly known as H+

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9
Q

Define the term ‘acid’

A

Releases hydrogen ions into aqueous solution

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10
Q

What is a strong acid?

A

A strong acid completely dissociates in aqueous solutions and the dissociation is irreversible

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11
Q

What is a weak acid?

A

A weak acid only partially dissociates in aqueous solutions and the dissociation is reversible

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12
Q

Define the term ‘base’

A

A compound that neutralises an acid by accepting a hydrogen ion to form a salt (proton acceptor)

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13
Q

State four examples of bases

A

Ammonia, metal hydroxides, metal carbonates, metal oxides

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14
Q

Define the term ‘alkali’

A

A type of soluble base which releases hydroxide ions in aqueous solution

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15
Q

Why is ammonia also classed as an alkali?

A

It takes a proton from water to form ammonium and hydroxide
NH3 + H2O —> NH4+ + OH-

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16
Q

Define the term ‘salt’

A

The product of a reaction in which the hydrogen ions from the acid are replaces by the metal or ammonium ions

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17
Q

What are the products of a reaction between an acid and an alkali?

A

Acid + alkali —> salt + water

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18
Q

What are the products of a reaction between an acid and a metal carbonate?

A

Acid + metal carbonate —> salt + water + carbon dioxide

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19
Q

What are the products of a reaction between an acid and a metal carbonate?

A

Acid + metal carbonate —> salt + water + carbon dioxide

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20
Q

What are the products of a reaction between a metal and an acid?

A

Acid + metal —> salt + hydrogen

21
Q

Explain why the reaction of an acid and a metal is not a full neutralisation reaction?

A

Water is not formed

22
Q

What are the products of a reaction between an acid and a metal oxide?

A

Acid + metal oxide —> salt + water

23
Q

What are the products of a reaction between an acid and ammonia?

A

Acid + ammonia —> ammonium salt

24
Q

Define the term ‘standard solution’

A

A solution with a known concentration

25
Q

What is a volumetric flask?

A

A type of laboratory flask calibrated to contain a precise volume at a particular temperature

26
Q

What is the equation to calculate new concentration?

A

New concentration= (original volume/ new volume) x original concentration

27
Q

Describe how to prepare a standard solution

A
  1. Weigh the solid by difference in a mass balance to 2 d.p.
  2. Transfer the solid to a beaker then add 100mls of distilled water and dissolve by stirring with a glass rod
  3. Transfer the solution to a 250cm3 volumetric flask using a funnel
  4. Rinse beaker, funnel and glass rod into the volumetric flask
  5. Fill the volumetric flask to the 250cm3 line with distilled water, making sure the solution has its meniscus on the line with a dropping pipette
  6. Put the lid on and invert several times
28
Q

Describe how to carry out an acid-base titration

A
  1. Transfer the standard solution to a clean, dry beaker and label it
  2. Transfer 25.0cm3 of standard solution to a 250cm3 conical flask using a pipette and pipette filler
  3. Add 5 drops of methyl orange
  4. Rinse then fill the burette with hydrochloric acid using a funnel
  5. Titrate the standard solution (sodium hydrogen carbonate) with the hydrochloric acid continuously swirling until you reach the end point (yellow to orange). This is your trial titration
  6. Repeat the titration until you have two concordant results
  7. All the results should be recorded in a table, with burette readings to the nearest 0.05cm3
  8. Use concordant results to calculate the mean titre
  9. Calculate the moles of NaOH in a 25cm3 sample with a concentration of 0.100moldm-3
  10. Using the neutralisation equation of the reaction, calculate the moles of HCl in the mean titre
  11. Calculate the concentration of HCl in moldm-3 and give yours answer to 3 significant figures
29
Q

State the equation to calculate percentage uncertainty

A

Percentage uncertainty= (uncertainty of equipment/ size of measurement) x 100

30
Q

Define the term ‘oxidation number’

A

A measure of the number of electrons that an atom uses to bond with an atom of another element

31
Q

What does the oxidation number of an element represent?

A

How many electrons an atom has donated or accepted to form an ion or a compound

32
Q

What is rule 1 of oxidation states?

A

The oxidation number of a neutral element is zero e.g. H2, F2, Na, O2

33
Q

What is rule 2 of oxidation states?

A

The oxidation number of a monoatomic (one-atom) ion is the same as the charge on the ion e.g. Na+ has an oxidation number of (+1)

34
Q

What is rule 3 of oxidation states?

A

The sum of all oxidation numbers in a neutral compound is zero e.g. Na2CO3= 0

35
Q

What is rule 4 of oxidation states?

A

The sum of all the oxidation numbers in a polyatomic (many-atom) ion is equal to the charge on the ion e.g. CO3^2- = (-2)

36
Q

What is rule 5 of oxidation states?

A

In compounds the elements of:
Group 1= +1
Group 2= +2
Group 3= +3
E.g. in NaCl, Na= (+1) and Cl= (-1)

37
Q

What is rule 6 of oxidation states?

A

-The oxidation state of hydrogen in a compound is usually +1
-If hydrogen is part of a binary metal hydride (hydrogen and metal) then the oxidation state of hydrogen is -1 e.g. in NaH Na= +1 and H= -1

38
Q

What is rule 7 of oxidation states?

A

Fluorine always has an oxidation number of -1 in compounds

39
Q

What is rule 8 of oxidation states?

A

-The oxidation number of oxygen is usually -2
-However if with a peroxide then oxygen has an oxidation number of -1
-If bonded with fluorine it has an oxidation number of -1 e.g. in H2O2, O= -1

40
Q

What is rule 9 of oxidation states?

A

In transition metals the oxidation number can vary e.g. in Fe2O3, Fe= +3 but in Fe= +2

41
Q

What is rule 10 of oxidation states?

A

-Chlorine, bromine and iodine usually have oxidation numbers of -1
-Except when in a compound with oxygen e.g. in HCl, Cl= -1 but in NaClO3, Cl= +5

42
Q

State the systematic name for FeCl2

A

Iron (II) chloride

43
Q

State the systematic name for CuSO4

A

Copper (II) sulfate

44
Q

State the systematic name for SnO2

A

Tin (IV) oxide

45
Q

State the systematic name for Cu2O

A

Copper (I) oxide

46
Q

Define the term ‘redox reaction’

A

A reaction involving both oxidation and reduction

47
Q

What is OILRIG?

A

Oxidation is loss (of electrons) Reduction is gain (of electrons)

48
Q

What is a disproportionation reaction?

A

When an element is both oxidised and reduced in a reaction

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