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WorksheetsTitrations
Total questions: 10
Worksheet time: 8mins
Name
Class
Date
1.
acid + alkali ₋>
a)
salt + hydrogen
b)
salt + water
c)
salt + carbon dioxide + water
d)
salt
2.
HCl + NaOH →
a)
NaH + ClOH
b)
NaCl + H2
c)
NaCl + H2O
d)
NaCl + Cl2
3.
What is the endpoint of a titration
a)
Where the amount of acid and alkali are balanced according to the equation
b)
Where the colour changes
c)
At the end
4.
Why should you repeat your titration until you have results that are concordant (within 0.1cm3 of each other)
a)
To make sure your answer is accurate
b)
To make sure your answer is precise
5.
I am titrating 1M HCl with 1M NaOH. I have 25cm3 of HCl. How much NaOH will I need?
a)
2.5cm3
b)
5cm3
c)
25cm3
d)
50cm3
6.
what is the reading on this burette?
a)
4.4cm3
b)
3.5cm3
c)
3.6cm3
d)
4.5cm3
7.
I have 25cm3 of 1M HCl which neutralises 20cm3 of NaOH. What is the concentration of the NaOH?
a)
0.8 M
b)
1 M
c)
1.25 M
8.
I have 50cm3 of 0.1M HCl. How many moles of NaOH will I need to neutralise it?
a)
5
b)
0.5
c)
0.05
d)
0.005
9.
What's the white tile for in the titration?
a)
To clearly see the colour change
b)
To protect the workbench from acid spills
10.
Why do we use water to wash the solution from the burette into the flask
a)
To ensure accuracy (all solution reacts)
b)
To dilute the reagents
c)
To help the reaction go faster
d)
To see the colour of the indicator better
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