Year 10 Term 3 - Revision Test

Acids/Bases/Indicators/Salts [print-friendly version]

Multiple choice questions

1. Some hydrochloric acid is added to a little white powder in a test-tube. The mixture bubbles up in the test-tube. The white powder may have been -

   A. sodium chloride	C. silver nitrate
   B. calcium carbonate	D. sodium hydroxide

   
   
   
2. The gas given off in the last question would

   A. relight a glowing splint	C. turn lime-water milky
   B. turn wet red litmus blue	D. 'pop' when ignited.

   
   
   
3. A base reacts with an acid to give

   A. salt and water only	C. salt, water and carbon dioxide only
   B. salt and hydrogen	D. none of the above

   
   
   
4. A dilute acid reacts with an active metal to give

   A. salt and water only	C. salt, water and carbon dioxide only
   B. salt and hydrogen	D. none of the above

   
   
   
5. An acid reacts with a carbonate or a hydrogencarbonate (bi-carbonate) to give

   A. salt and water only	C. salt, water and carbon dioxide only
   B. salt and hydrogen	D. none of the above

   
   
   
6. A concentrated acid

   A. contains a small amount of acid and a large amount of water.	B. contains a small amount of water and a large amount of acid.
   C. should always be diluted by adding it carefully to water.	D. should never be added directly to water.
   E. both B and C	F. both B and D

   
   
   
7. Which of the following reactions is likely to proceed spontaneously, liberating hydrogen?

   A. silver and dilute hydrochloric acid	C. magnesium and dilute sulfuric acid
   B. zinc and concentrated nitric acid	D. gold and dilute hydrochloric acid.

   
   
   
8. Lactic acid would have a pH of

   A. 7	C. > 7
   B. < 7	D. insufficient information

   
   
   
9. Liquid laundry detergent has a pH of 9. It is

   A. an acid	C. neutral
   B. a base	D. a solution with a large concentration of H+ ions.

   
   
   
10. A soluble base is a/an

    A. acid	C. indicator
    B alkali	D. salt

    
    
    
11. The reaction between an acid and a base is called -

    A. combustion	C. neutralisation
    B. precipitation	D. fermentation

    
    
    
12. Which of the following tests indicates the presence of hydrogen?

    A. Relights a glowing splint	C. Turns lime-water milky
    B. Turns wet red litmus blue	D. 'Pops' when ignited.

    
    
    

Short answer questions

1. Define an acid.
   
   
2. Give some common laboratory examples and some examples of acids in the home.
   
   
3. Define a base. Give some examples of strong and weak bases.
   
   
4. Compare and contrast acids and bases.
   
   
5. Define an indicator. Give some common examples.
   
   
6. Define a salt.
   
   
7. What is an alkali?
   
   
8. Explain the difference between a concentrated and a dilute acid.
   
   
9. What is the difference between a weak and strong acid?
   
   
10. How should you safely dilute a concentrated acid?
    
    
11. How should you treat an acid spill - on your skin? on a laboratory bench?
    
    
12. What should you do if someone were to get acid in his/her eyes or have a serious spill of more concentrated acid over their skin?
    
    
13. What is meant by neutralisation?
    
    
14. Complete the following word equations - (a) acid + strong base gives…. (b) acid + carbonate (or hydrogen carbonate) gives ….. (c). dilute acid + active metal gives ………
    
    
15. Which metals are too reactive to add to acids?
    
    
16. Which metals usually do not react with dilute acids? What are these metals called?
    
    
17. Which acid sometimes releases a brown toxic gas (nitrogen dioxide) rather than hydrogen when added to metals?
    
    
18. Why are antacid tablets used to treat indigestion?
    
    
19. What is the test for (a) carbon dioxide gas? (b) hydrogen gas?
    
    
20. Identify the following as acids, strong bases or salts.

    HCl	CaO	AgNO3
    NaOH	H2SO4	CaCl2
    Ca(OH)2	KNO3	BaSO4
    Na2O	Mg(NO3)2	CuSO4

    
    
    
21. What are bases often used for?
    
    
22. What is the pH scale?
    
    
23. What is the pH range for (a) acids? (b) bases? (c) neutral solutions?
    
    
24. How would you expect the pH to vary for a strong and weak acid of the same concentration?
    
    
25. Complete the following as balanced chemical equations. (Note: check if a reaction actually takes place)

(a) HCl + NaOH

(b) H2SO4 + CaO

(c) HNO3 + Ca(OH)2

(d) H2SO4 + Zn

(e)HCl + Cu

(f) HCl + Mg

(g) HCl + CuCO3

(h) H2SO4 + Na2CO3

(i) HNO3 + KHCO3

(j) H2SO4 + NaHCO3




26. Determine the unknown (x) in the following incomplete reactions.

(a) Pb(NO3)2 + 2 NaCl —> x + 2 NaNO3

(b) Zn + x —> ZnSO4 + H2

(c)Cu + x —> Cu(NO3)2 + 2 NO2 + 2 H2O

(d) x + H2SO4 —> K2SO4 + 2CO2 + 2 H2O




27. Determine whether the following solutions are acidic, basic or neutral.

(a) pH = 3.5;	(e) pH = 7.2
(b) pH = 10	(f) Solution remains clear when phenolphthalein is added.
(c) pH = 7.0;	(g) Solution is blue in litmus and pink in phenolphthalein.
(d) pH = 6.4;




28. Draw and label a set of apparatus to accurately find the neutralization point of a reaction between an acid and a base.
    
    
29. What is the laboratory technique being used here? Why is this technique used in chemistry?

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