Chemistry 2D

Front 1

Suggest a pH value for anacid.

Back 1

Acids have a pH between 1and 6.

Front 2

What pH is a neutral solution?

Back 2

A neutral solution has a pH of7

Front 3

Which ion makes solutionsacidic?

Back 3

The hydrogen ion (H+) makessolutions acidic.

Front 4

Which ion makes solutionsalkaline?

Back 4

The hydroxide ion (OH-)makes solutions alkaline.

Front 5

What is the equation forneutralisation?

Back 5

The equation for neutralisationis

H+(aq) + OH-(aq) =H2O(aq)

Front 6

Which salts are producedfrom:

• hydrochloric acid

• sulfuric acid

• nitric acid

Back 6

hydrochloric acid = chloride• sulfuric acid = sulfate• nitric acid = nitrate

Front 7

How is ammonium nitrateproduced and what is it usedfor?

Back 7

Ammonium nitrate is producedby reacting ammonia solutionwith nitric acid. Ammoniumnitrate is used as a fertiliser

Front 8

What is meant by electrolysis?

Back 8

Passing an electric currentthrough an ionic substancewhich is melted or dissolved inwater, causing the substanceto break down into elements

Front 9

In electrolysis, what is meantby the electrolyte.

Back 9

In electrolysis, the electrolyteis the ionic compound which isbroken down to its elementsas electric current is passed.

Front 10

During electrolysis, which ionmoves to the negativeelectrode and why?

Back 10

During electrolysis, thepositive ion moves to thenegative electrode. This isbecause opposite chargesattract.

Front 11

Suggest a reason why weelectroplate a metal with adifferent metal.

Back 11

Electroplating can be used toprevent corrosion. It can alsobe carried out to make a metalmore attractive.

Front 12

During electrolysis, what takesplace at the negativeelectrode?

Back 12

At the negative electrode,positive ions gain electrons.Gaining electrons is calledreduction.

Front 13

During electrolysis, what takesplace at the positiveelectrode?

Back 13

At the positive electrode,negative ions lose electrons.Losing electrons is calledoxidation.

Front 14

When electrolysing an ioniccompound in solution, how dowe work out what is producedat the negative electrode?

Back 14

If the metal is more reactive thanhydrogen, then hydrogen isproduced at the negative electrode.If the metal is less reactive thanhydrogen, the metal is produced atthe negative electrode.

Front 15

Write the half equation for theoxidation of chloride at thepositive electrode.

Back 15

2Cl- Cl2 + 2eor2Cl- - 2e- Cl2

Front 16

What is the role of cryoliteduring electrolysis of moltenaluminium oxide?

Back 16

Cryolite lowers the meltingpoint which reduces theenergy needed, saving money.

Front 17

During the electrolysis of moltenaluminium oxide, what isproduced at the negativeelectrode and what is producedat the positive electrode?

Back 17

During electrolysis of aluminiumoxide, aluminium is produced atthe negative electrode andoxygen is produced at thepositive electrode.

Front 18

During electrolysis of moltenaluminium oxide, why does thepositive electrode need to bereplaced regularly?

Back 18

During electrolysis of molten aluminiumoxide, graphite electrodes are used.Oxygen is produced at the positiveelectrode. The oxygen reacts with thecarbon graphite, producing carbondioxide. The positive electrode thereforeneeds replacing regularly.

Front 19

During electrolysis of sodiumchloride solution, what isproduced at the negativeelectrode?

Back 19

During electrolysis of sodiumchloride solution, hydrogengas is produced at thenegative electrode

Front 20

During electrolysis of sodiumchloride solution, what isproduced at the positiveelectrode?

Back 20

During electrolysis of sodiumchloride solution, chlorine gasis produced at the positiveelectrode. This is used tomake bleach and plastic.

Front 21

During electrolysis of sodiumchloride, what solution remainsat the end?

Back 21

During electrolysis of sodiumchloride solution, sodiumhydroxide solution remains atthe end. This is used to makesoap.