Module 2: Acids And Redox Flashcards

Question

Acids and bases What does metal hydroxide and acid

Answer 1

Salt and water

Answer 2

Salt and water

Answer 3

H+ (aq) + OH- (aq) —> H2O(l)

Answer 4

Salt and water and carbon dioxide gas

Answer 5

When hydrogen ions in the acid area replaced by metal ions or ammonium ions from the alkali

Answer 6

Base fully dissociates in water and lots of OH-ions are released

Answer 7

Bases which partially ionise in water to release OH- ions

Answer 8

Doesn’t directly produce OH- ions

Answer 9

Reaction between ammonia and water produces hydroxide ions

Answer 10

Ammonium salt

Answer 11

Finding concentration of acid or alkali solutions

Answer 12

2. Use a pipette and pipette filler to transfer 25.0 cm3 of known solution to a conical flask. 3. Add a few drops of indicator to the flask. 4. Using the funnel, rinse then fill the burette with the unknown solution and record initial 5. Titrate theknown solution with the unknown solution , with constant swirling, until the end point is reached . This is your rough titration. 6. Repeat your titration accurately until you have three concordant results. You may wish to keep the solution from your first accurate titration in order to achieve consistency by colour matching. 7. Ensure that you have recorded all of your results, with burette readings to the nearest 0.05 cm3. 8. Find titre by doing final-initial

Answer 13

Bottom of meniscus

Answer 14

Methyl orange Phenolphthalein

Answer 15

Turns yellow to red when adding acid to alkali

Answer 16

Turns pink to colourless when adding acid to alkali

Answer 17

Colour change is too gradual

Answer 18

Standard solutions

Answer 19

Unknown solution

Answer 20

A solution that has a precisely known concentration

Answer 21

-Using a precise balance, carefully weigh out the required mass of solid onto a weighing boat. -Transfer this solid to a beaker. Use some distilled water to wash any bits of solid from the weighing boat into the beaker. -Add water to the beaker to completely dissolve the solid -Use a glass rod to stir the solution to help the solid dissolve. -Once the solid has dissolved, transier the solution into a volumetric flask. You'll need to use a volumetric flask that's the same size as the volume of solution you want to make up. -Rinse the beaker and glass rod with water, transferring this water into the volumetric flask. -Use water to fill the volumetric flask up to the graduation line. Use a pipette to add the final few drops to make sure you don't add too much water and overshoot the graduation line. -Put the lid on the flask and turn the flask over a few times to thoroughly mix the solution.

Answer 22

Concentrations

Answer 23

1. Balance equation 2. And in table write molratio, con, vol, mol for each of what you know *using the right units 3. Work moles of both using con=mol/vol then mol ratio 4. Using con=mol/vol to find concentration

Answer 24

Acids that donate more than one proton

Answer 25

Acid that donates two protons

Answer 26

Sulphuric acid H2SO4

Answer 27

Donates three protons eg phosphoric acid H3PO4

Answer 28

Need double or triple number of moles to neutralise acid

Answer 29

Times by Mr

Answer 30

Done to analys a chase or acid that does not treat easily or quickly with a base or acid

Answer 31

Base or acid is treated with and excess of acid or base hen left over is then titration which can be used to work back to find about original acid or base

Answer 32

Molecules only partially ions in the solution but there is still lots of acid particle in the volume of solutions

Answer 33

Molecules fully ionise in solution but only few acid particles in the volume of solution

Answer 34

Measure of number of hydrogen ions in solution

Answer 35

Directly PH § [H+] Down1. ^x10

Answer 36

Ions which don’t charge and aren’t used in a reaction

Answer 37

Redox hydrogen ions in acid gain electrons so are reduced Metal lose electrons so are oxidised

Answer 38

2H+ + O2- —> H2O

Answer 39

H+ + OH- —> H2O

Answer 40

2H+ + CO3 2- —> H2O + CO2

Answer 41

Loss of electrons Gain of oxygen Loss of hydrogen

Answer 42

Gain of electrons Loss of oxygen Gain of hydrogen

Answer 43

Mg —> Mg 2+ + 2 e-

Answer 44

1/2 O2 + 2e- —> O2-

Answer 45

Lose or gain electrons

Answer 46

How many electron an atom has donated or accepted to form an ion or to form part of a compound

Answer 47

All uncombined element and elements bonded to identical elements have an oxidation number of 0 which means they haven’t accepted or donated any electrons

Answer 48

Oxidation number is the same as its charge Eg Na+ has an oxidation number of +1 and Mg2+ has an oxidation number of +2

Answer 49

Sum of oxidation numbers is the same as the overall charge of the ion so each of the atoms within the ion will have oxidation’s number which add up to the overall charge

Answer 50

Overall oxidation number is 0and each elements have own oxidation number which add up to 0

Answer 51

Nearly always 0 except in peroxides (O2 2-) where its -1 and molecular oxygen (O2) where its 0

Answer 52

Always +1 except in metal hydrides (MH x ) where its -1 and in molecular hydrogen (H2( where its 0

Answer 53

If an element can have multiply oxidation number os isn’t in its normal oxidation state eg (l) = +1, (ll) = +2 and (lll) = +3

Answer 54

Provides the electrons for another substance to be reduced and itself is oxidised

Answer 55

Accepts electrons from another substance fort hate to be oxidised and itself is reduced

Answer 56

Have positive values in compounds Value is normally that of group number Values can go no higher than the group number

Answer 57

Mostly negative based on usual ion Can have values up to groups number Often included in name

Answer 58

Reduction and oxidation happen simultaneously

Answer 59

Increase by 1 for each electron

Answer 60

Decrease by 1

Answer 61

Element has lost electron and been oxidised

Answer 62

Element had gained electrons and been reduced

Answer 63

1. Work out formula before and after 2. Work out oxidation state of element for before and after 3. Add electrons to one side so oxidation’s states balance 4. If overall charge on both sides aren’t equal add H+ ions (protons) to one side to balance 5. If still don’t balance, add water molecules to one side

Answer 64

1. Write out two half equations 2. Multiply equation s so the the number of electrons balance in both equations 3. Add two equations together and cancel out electrons 4. Cancel our anything else which appears on both sides

Answer 65

When a species is simultaneously oxidised and reduced

Answer 66

CL2 + H2O -> HCl + HClO Chlorine

Answer 67

2NaOH + Cl2 -> NaCl + NaClO + H2O Chlorine