Topic 3.1-3.21 Acids Flashcards

1
Q

What are acids in solution sources of?

A

Hydrogen ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What are alkalis in solution sources of?

A

Hydroxide ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Describe the pH scales

A

A neutral solution has a pH of 7 and that acidic solutions have lower pH values and alkaline solutions higher pH values

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

How do acids and alkalis react to phenolphthalein?

A

Alkalis turn pink
Acids are colourless

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

How do acids and alkalis react to methyl orange?

A

Alkalis turn yellow
Acids are red

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

How do acids and alkalis react to litmus?

A

Alkalis turn blue
Acids turn red

(Same for blue/red litmus paper.
Red litmus paper stays red in acid, turns blue in alkali.
Blue litmus paper turns red in acid, stays blue in alkali)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

How does the concentration of hydrogen and hydroxide ions effect the pH of an acidic/alkaline solution?

A

The higher the concentration of hydrogen ions in an acidic solution, the lower the pH.
The higher the concentration of hydroxide ions in an alkaline solution, the higher the pH.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

How does hydrogen ion concentration effect pH?

A

As hydrogen ion concentration in a solution increases by a factor of 10, the pH of the solution decreases by 1 unit.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

​ ​​​​​​Explain the terms dilute and concentrated

A

​ ​​​​​​​​​​​Concentrated​ ​=​ ​larger​ ​quantity​ ​of​ ​solute​ ​in​ ​a​ ​given​ ​volume​ ​of​ ​a​ ​solution
Dilute​ ​=​ ​smaller​ ​quantity​ ​of​ ​solute​ ​in​ ​a​ ​given​ ​volume​ ​of​ ​a​ ​solution

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Describe the core practical for ​​​​ ​​​​ ​​​​​​​​​​​​​​​​ ​​​​​​​​ ​​
investigating the change in pH on adding powdered calcium hydroxide or calcium oxide to a fixed volume of dilute hydrochloric acid

A

-Add​ ​dilute​ ​HCl​ ​to​ ​the​ ​beaker​ ​and​ ​measure​ ​pH
-Add​ ​weighed​ ​mass​ ​of​ ​calcium​ ​hydroxide​ ​and​ ​stir​ ​then​ ​record​ ​pH
-Keep​ ​adding​ ​weighed​ ​masses​ ​of​ ​calcium​ ​hydroxide​ ​until​ ​there​ ​is​ ​no​ ​more change​ ​to​ ​the​ ​pH
To analyse it:
-draw​ ​a​ ​line​ ​graph​ ​with​ ​mass​ ​added​ ​on​ ​the​ ​horizontal​ ​axis​ ​and​ ​with​ ​pH​ ​on the​ ​vertical​ ​axis
-draw​ ​a​ ​line​ ​of​ ​best​ ​fit​ ​(remember​ ​to​ ​ignore​ ​any​ ​anomalies)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Explain the terms weak and strong acids

A

Strong​ ​acid​ ​=​ ​fully​ ​dissociates​ ​in​ ​aqueous​ ​solution​ ​(dissociation​ ​is​ ​where​ ​an​ ​acid breaks​ ​down​ ​to​ ​release​ ​H​+​​ ​ions​ ​in​ ​solution)

Weak​ ​acid​ ​=​ ​partially​ ​dissociates​ ​in​ ​aqueous​ ​solution as it has fewer H+ ions than expected

Stronger​ ​an​ ​acid,​ ​greater​ ​the​ ​dissociation,​ ​the​ ​more​ ​H​+​​ ​ions​ ​released,​ ​the​ ​lower the​ ​pH​ ​(for​ ​a​ ​given​ ​conc.​ ​of​ ​aq.​ ​solutions)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What is a base?

A

A base is any substance that reacts with an acid to form a salt and water only

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What is an alkali?

A

A soluble base

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What results from the reaction of an aqueous solution of acid with a metal?

A

A salt + hydrogen gas (H2)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What results from the reaction of an aqueous solution of acid with a metal hydroxide?

A

A salt + water

(Metal​ ​hydroxides​ ​are​ ​bases/alkalis​ ​if​ ​insoluble/soluble)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What results from the reaction of an aqueous solution of acid with a metal oxide?

A

A salt + water

(Metal​ ​oxides​ ​are​ ​normally​ ​bases​ ​(because​ ​insoluble))

17
Q

What results from the reaction of an aqueous solution of acid with a metal carbonate?

A

A salt + water + carbon dioxide

18
Q

Describe the chemical test for hydrogen

A

Use a burning split held at the open end of a test tube of the gas. If it contains hydrogen it creates a ‘squeaky pop’ sound

19
Q

Describe the chemical test for carbon dioxide (using limewater)

A

Bubble​ ​the​ ​gas​ ​through​ ​the​ ​limewater​ ​(calcium​ ​hydroxide​ ​solution)​ ​and​ ​it will​ ​turn cloudy/output a white precipitate if it contains carbon dioxide

20
Q

Describe a neutralisation reaction

A

​A reaction​ ​between​ ​an​ ​acid​ ​and​ ​a
base

21
Q

​ ​​ Explain an acid-alkali neutralisation

A

A reaction in which hydrogen ions (H+) from the acid react with hydroxide ions (OH–) from the alkali to form water

H​+(​aq)​​+​​OH​-(​aq)​​->​​H2​O​(l)

22
Q

Explain what you should do to prepare soluble salts from an acid and an insoluble reactant and why

A

-Add excess​ ​of​ ​the​ ​reactant
* this​ ​is​ ​to​ ​ensure​ ​your​ ​volume​ ​of​ ​acid​ ​reacts​ ​completely

-Remove excess​ ​reactant
* this​ ​is​ ​done​ ​by​ ​filtration​ ​of​ ​the​ ​insoluble​ ​reactant​ ​and​ ​is​ ​done​ ​so​ ​that​ ​you are​ ​left​ ​with​ ​just​ ​a​ ​salt​ ​and​ ​water

-The​ ​remaining​ ​solution​ ​is​ ​only​ ​salt​ ​and​ ​water
* this​ ​is​ ​because​ ​all​ ​of​ ​your​ ​acid​ ​has​ ​fully​ ​reacted​ ​and​ ​you​ ​have​ ​filtered​ ​off your​ ​other​ ​reactant,​ ​so​ ​that​ ​the​ ​only​ ​products​ ​of​ ​your​ ​reaction​ ​are​ ​a​ ​salt and​ ​water
* if​ ​you​ ​have​ ​used​ ​a​ ​carbonate​ ​you​ ​would​ ​still​ ​only​ ​have​ ​a​ ​salt​ ​and​ ​water remaining​ ​as​ ​carbon​ ​dioxide​ ​gas​ ​would​ ​have​ ​been​ ​given​ ​off​ ​into​ ​the atmosphere

23
Q

What should you do if soluble salts are prepared from an acid and an soluble reactant and why?

A

-Titration​ ​must​ ​be​ ​used:
* both​ ​reactants​ ​are​ ​liquids/soluble,​ ​so​ ​if​ ​you​ ​have​ ​an​ ​excess​ ​of​ ​one​ ​you would​ ​not​ ​be​ ​able​ ​to​ ​easily​ ​remove​ ​it​ ​from​ ​your​ ​mixture​ ​of​ ​products,​ ​this means​ ​you​ ​need​ ​to​ ​measure​ ​the​ ​exact​ ​amount​ ​of​ ​volumes​ ​that​ ​react, which​ ​is​ ​easily​ ​done​ ​using​ ​a​ ​titration.

-You​ ​can​ ​then​ ​mix​ ​the​ ​exact​ ​proportions​ ​of​ ​the​ ​two​ ​reactants

-The​ ​exact​ ​amount​ ​of​ ​acid​ ​has​ ​thus​ ​been​ ​added​ ​to​ ​the​ ​soluble​ ​reactant,​ ​meaning that​ ​the​ ​leftover​ ​solution​ ​is​ ​only​ ​salt​ ​and​ ​water,​ ​no​ ​acid​ ​or​ ​alkali,​ ​because​ ​they have​ ​been​ ​completely​ ​neutralised

24
Q

Describe the core practical for investigating the preparation of pure, dry hydrated copper sulfate crystals starting from copper oxide including the use of a water bath

A

-Add​ ​an​ ​excess​ ​of​ ​copper​ ​oxide​ ​(insoluble)​ ​to​ ​your​ ​acid​ ​(sulfuric​ ​acid — H​2S​O​4 — as​ ​you​​ are​​ making​​ copper​​ SULFATE)
-use​ ​a​ ​filter​ ​and​ ​filter​ ​paper​ ​to​ ​filter​ ​off​ ​any​ ​copper​ ​oxide​ ​that​ ​hasn’t reacted​ ​(your​ ​solution​ ​should​ ​be​ ​blue​ ​as​ ​copper​ ​sulfate​ ​solution​ ​has​ ​been formed)
-evaporate​ ​off​ ​the​ ​water​ ​by​ ​placing​ ​your​ ​final​ ​solution​ ​in​ ​a​ ​water​ ​bath

25
Q

Describe how to carry out an acid-alkali titration, using burette, pipette and a suitable indicator, to prepare a pure, dry salt

A
  1. Wash​ ​burette​ ​using​ ​the​ ​acid​ ​and​ ​then​ ​water
  2. Fill​​ burette​ ​to​​ 100cm3​​​ w​ith​​ acid​​ with​​ the​​ meniscus’​ ​base​​ on​​ the​​ 100cm3​​​​ line
  3. Use 25cm3​ pipette to add 25cm3​ of alkali into a conical flask, drawing alkali into​ ​the​ ​pipette​ ​using​ ​a​ ​pipette​ ​filler
  4. Add a few drops of a suitable indicator to the conical flask (eg: phenolphthalein​ ​which​ ​is​ ​pink​ ​when​ ​alkaline​ ​and​ ​colourless​ ​when​ ​acidic)
  5. Add acid from burette to alkali until end-point is reached (as shown by the indicator).
  6. The titre (volume of alkali needed to exactly neutralise the acid) is the difference​ ​between​ ​the​ ​first​ ​(100cm3)​ ​and​ ​second​ ​readings​ ​on​ ​the​ burette
  7. Repeat​ ​the​ experiment​ ​to​ ​gain​ ​more​ ​precise​ ​results
  8. To prepare a pure, dry salt you warm the salt solution to evaporate the water
  9. Crystals​ ​form
26
Q

Describe the affect of traces of water in the pipette

A

The traces of water in the pipette reduce the titration result as it lowers the concentration of the barium hydroxide solution

27
Q

Describe the affect of traces of water in the conical flask

A

The water has no effect on the titration result as any water present does not affect the amount of barium hydroxide present

28
Q

Which common substances are always soluble in water?

A

All common sodium, potassium and ammonium salts and all nitrates are soluble

29
Q

What is the general solubility rule for chlorides?

A

Common chlorides are soluble except those of silver and lead

30
Q

What is the general solubility rule for sulfates?

A

Common sulfates are soluble except those of lead, barium and calcium

31
Q

What is the general solubility rule for carbonates and hydroxides?

A

Common carbonates and hydroxides are insoluble except those of sodium, potassium and ammonium

32
Q

When solutions are mixed together what will cause a precipitate to be formed?

A

If a salt in the reaction is insoluble it will form as precipitate.

Soluble salts remain in solution

33
Q

Describe the method used to prepare a pure, dry sample of an insoluble salt

A
  1. mix​ ​the​ ​two​ ​solutions​ ​needed​ ​to​ ​form​ ​the​ ​salt
  2. filter​ ​the​ ​mixture​ ​using​ ​filter​ ​paper,​ ​which​ ​the​ ​insoluble​ ​salt​ ​will​ ​be​ ​left​ ​on
  3. wash​ ​the​ ​salt​ ​using​ ​distilled​ ​water
  4. leave​ ​the​ ​salt​ ​to​ ​dry​ ​on​ ​filter​ ​paper​ ​(water​ ​will​ ​evaporate,​ ​speed​ ​this​ ​process​ ​up by​ ​drying​ ​it​ ​in​ ​an​ ​oven)