Practise acids-bases-salts questions by applying proton definitions, choosing salt reagents and sequencing crystal preparation.
This question is about Group 2 elements and their compounds.
Which of these compounds is an insoluble solid?
calcium nitrate
calcium sulfate
magnesium nitrate
magnesium sulfate
This question is about salts.
Soluble salts can be prepared by the reaction between a metal oxide and an acid.
The equation for this type of reaction is
State, in terms of protons, what happens in this reaction.
A student is given of dilute sulfuric acid and a bottle of solid copper(II) carbonate.
Describe the method that the student should use to prepare a saturated solution of copper(II) sulfate.
In your answer, refer to the pieces of apparatus that the student should use.
Sodium hydroxide dissolves in water, forming a strongly alkaline solution.
Ammonia dissolves in water, forming a slightly less alkaline solution.
When ammonia solution reacts with sulfuric acid, a neutralisation reaction occurs and ammonium sulfate forms.
How does the sulfuric acid act in this reaction?
as a neutron donor
as a neutron acceptor
as a proton donor
as a proton acceptor
This question is about salts.
Soluble salts can be prepared by the reaction between a metal oxide and an acid.
The equation for this type of reaction is
State, in terms of protons, what happens in this reaction.
A student uses this apparatus to investigate the rate of reaction between marble chips and dilute hydrochloric acid.
The equation for the reaction is
During the reaction the mass of the contents of the flask decreases.
State why the mass of the contents of the flask decreases.
This question is about magnesium metal and its compounds.
A student uses this method to make a solution of magnesium chloride.
Step 1. measure of dilute hydrochloric acid into a beaker
Step 2 add magnesium powder a little at a time
Step 3 keep adding magnesium powder until it is in excess
Step 4 remove the excess magnesium powder by filtration
This is the equation for the reaction.
Give a reason why the student adds an excess of magnesium in step 3.
Sodium sulfate can be prepared by the reaction between sodium hydroxide solution and sodium hydrogensulfate ( ) solution.
This is the equation for the reaction.
Sodium hydrogensulfate solution is acidic.
A student adds of sodium hydroxide solution to a conical flask and adds two drops of indicator.
The student does a titration.
The student repeats the titration without the indicator and forms a solution of sodium sulfate.
Describe how the student can obtain pure, dry crystals of hydrated sodium sulfate from the solution.
A scientist reacts lead(II) nitrate solution with sodium bromide solution.
This is the equation for the reaction.
Describe how the scientist could obtain a pure dry sample of lead(II) bromide from the reaction mixture.
A salt can be made by reacting an acid with an insoluble base.
A student has a sample of copper(II) oxide.
Stage 1 pour of dilute sulfuric acid into a beaker
Stage 2 warm the acid using a Bunsen burner
Stage 3 add a small amount of copper(II) oxide to the warm acid and stir the mixture
Stage 4 add further amounts of copper(II) oxide until copper(II) oxide is in excess
Stage 5 filter the mixture
Stage 6 obtain crystals from the filtrate
State why the acid is warmed in stage 2.
State how the student would know that the copper(II) oxide is in excess in stage 4.
State why the mixture is filtered in stage 5.
State the colour of the filtrate obtained in stage 5.
Describe how the student could obtain a pure, dry sample of hydrated copper(II) sulfate crystals from the filtrate in stage 6.
This question is about soluble salts and insoluble salts.
When solutions of lead nitrate and sodium sulfate are mixed, one product is solid lead sulfate.
This is the equation for the reaction.
Describe how a pure, dry sample of solid lead sulfate can be obtained from the mixture.