Study of Compounds – Nitric Acid Quiz - ICSE Class 10 Chemistry

Free practice quiz: Study of Compounds – Nitric Acid (ICSE Class 10 Chemistry). 57 multiple-choice questions with answers and explanations. Play online, no sign-up needed.

This ICSE Class 10 Chemistry practice quiz has 57 multiple-choice questions on Study of Compounds – Nitric Acid, and 57 of them come with an explanation. Try the 5 sample questions below (tap an option to check yourself), then play the full quiz online. No sign-up needed.

Sample questions

1. Nitric acid reacts with copper metal to produce copper(II) nitrate, nitrogen monoxide, and water. What is the balanced chemical equation for this reaction?

   1. Cu + 4HNO₃ → Cu(NO₃)₂ + 2NO₂ + 2H₂O
   2. 3Cu + 8HNO₃ → 3Cu(NO₃)₂ + 2NO + 4H₂O
   3. Cu + 2HNO₃ → Cu(NO₃)₂ + H₂
   4. Cu + HNO₃ → CuO + NO₂ + H₂O
   Show answer

   Answer: B. 3Cu + 8HNO₃ → 3Cu(NO₃)₂ + 2NO + 4H₂O

   This question tests the ability to balance redox reactions involving nitric acid. Copper is oxidized, and nitrogen in nitrate is reduced. The common products with dilute nitric acid are copper(II) nitrate, nitrogen monoxide (NO), and water. Balancing the half-equations for oxidation and reduction and combining them yields the correct balanced equation.

2. The brown ring formed in the nitrate test is a complex of iron with nitric oxide. The formula of this complex is typically represented as:

   1. [Fe(NO)(H₂O)₅]²⁺
   2. [Fe(NO₂)(H₂O)₅]²⁺
   3. [Fe(NO)₂(H₂O)₄]⁺
   4. [Fe(NO)₃(H₂O)₃]³⁺
   Show answer

   Answer: A. [Fe(NO)(H₂O)₅]²⁺

   In the brown ring test, nitrate ions are reduced to nitric oxide (NO) by ferrous sulphate. This NO then forms a coordination complex with excess Fe²⁺ ions present in the solution. The complex formed is nitrosyl ferrous ion or nitrosoiron(II) ion, with the formula [Fe(NO)(H₂O)₅]²⁺, which is brown in color and responsible for the characteristic ring.

3. The chemical formula of nitric acid is HNO₃. What is the oxidation state of nitrogen in this compound?

   1. +1
   2. +3
   3. +5
   4. +7
   Show answer

   Answer: C. +5

   To determine the oxidation state of nitrogen in HNO₃, we assign standard oxidation states to hydrogen (+1) and oxygen (-2). Let the oxidation state of nitrogen be 'x'. The sum of oxidation states in a neutral molecule is zero: (+1) + x + 3(-2) = 0. Solving for x: 1 + x - 6 = 0, which gives x = +5. Thus, the oxidation state of nitrogen in nitric acid is +5.

4. Which gas is produced when a very active metal like Magnesium reacts with extremely dilute nitric acid?

   1. Nitrous oxide (N₂O)
   2. Nitric oxide (NO)
   3. Nitrogen gas (N₂)
   4. Ammonia (NH₃)
   Show answer

   Answer: D. Ammonia (NH₃)

   When highly reactive metals like magnesium react with extremely dilute nitric acid, the reduction of nitric acid can proceed to the lowest possible oxidation state of nitrogen, which is -3 in ammonia (NH₃). The reaction is complex and often involves the formation of ammonium nitrate, which then reacts further or dissociates. A simplified representation might be: 8Mg + 10HNO₃(extremely dilute) → 8Mg(NO₃)₂ + NH₄NO₃ + 3H₂O, or even 8Mg + 10HNO₃ → 8Mg(NO₃)₂ + NH₃ + H₂O + N₂O (this is a simplified representation and often the product distribution is complex). However, the formation of ammonia or ammonium ions is indicative of the extreme reduction of nitric acid. Considering the options, and the extreme conditions, ammonia is the most likely answer representing the lowest reduction product. Let me verify this. Yes, with extremely dilute nitric acid and active metals, ammonium salts or ammonia can be formed. This is a higher complexity question testing nuanced reaction products.

5. The reaction of nitrogen dioxide with water forms nitric acid and nitric oxide. If 3 moles of NO₂ react, how many moles of HNO₃ are formed according to the equation 3NO₂ + H₂O → 2HNO₃ + NO?

   1. 1 mole
   2. 2 moles
   3. 3 moles
   4. 1.5 moles
   Show answer

   Answer: B. 2 moles

   The balanced chemical equation is 3NO₂(g) + H₂O(l) → 2HNO₃(aq) + NO(g). The stoichiometry of the reaction shows that 3 moles of nitrogen dioxide (NO₂) produce 2 moles of nitric acid (HNO₃). Therefore, if 3 moles of NO₂ react, 2 moles of HNO₃ are formed.

More questions in this quiz

Answers and explanations are in the full quiz.

1. Concentrated nitric acid, when heated with sulphur, produces sulphur dioxide, nitrogen dioxide, and water. Which of the following is NOT a product in this reaction?
2. The brown ring test for the detection of nitrate ions involves the reaction of nitrate ions with ferrous sulphate in the presence of concentrated sulphuric acid. The brown ring is formed due to the formation of which complex ion?
3. When nitric acid is heated strongly, it decomposes to produce nitrogen dioxide, oxygen, and water. What are the oxidation states of nitrogen in the reactant nitric acid and the product nitrogen dioxide?
4. Which of the following methods is NOT used for the laboratory preparation of nitric acid?
5. The action of nitric acid on metals depends on its concentration. Which of the following statements accurately reflects this?
6. When a metal like silver reacts with dilute nitric acid, what are the primary products formed?
7. The reaction of concentrated nitric acid with copper produces copper(II) nitrate, nitrogen dioxide, and water. Which of the following is the balanced chemical equation for this reaction?
8. Why is nitric acid stored in glass-stoppered bottles and not in metal containers?
9. What is the role of platinum-rhodium gauze in the Ostwald process for nitric acid production?
10. Consider the reaction of nitric acid with carbon: C + 4HNO₃ → CO₂ + 4NO₂ + 2H₂O. In this reaction, nitric acid acts as:
11. Which of the following is a property of pure nitric acid?
12. Nitric acid is considered a 'hygroscopic' substance. What does this term imply about its behavior?
13. In the Ostwald process, the reaction of nitrogen dioxide with water produces nitric acid and another nitrogen oxide. What is this other nitrogen oxide?
14. What is the primary product of the reaction between zinc and dilute nitric acid?
15. Concentrated nitric acid is a powerful dehydrating agent. Which of the following substances would NOT be dehydrated by concentrated nitric acid?
16. The reaction of nitric acid with lead to form lead(II) nitrate, lead(II) oxide, and nitrogen monoxide is an example of:
17. When nitric acid is heated strongly, it decomposes. The balanced equation for this decomposition is:
18. The Ostwald process uses a catalytic amount of platinum-rhodium gauze. What is the purpose of the rhodium in the alloy?
19. Nitric acid is classified as a strong acid. This means that in aqueous solution:
20. What is the color of nitrogen dioxide (NO₂) gas formed during the decomposition or reactions of nitric acid?
21. Nitric acid reacts with sodium hydroxide. What type of reaction is this?
22. Which of the following products is INCORRECTLY associated with the reaction of nitric acid with a specific substance?
23. The process of 'fuming' in concentrated nitric acid is due to the presence of dissolved:
24. In the Ostwald process, after the formation of NO, it is oxidized to NO₂. What is the balanced equation for this second step?
25. Which of the following metals reacts with dilute nitric acid to produce hydrogen gas?
26. What is the oxidation state of nitrogen in dinitrogen pentoxide (N₂O₅), a product formed by the dehydration of nitric acid?
27. Nitric acid is used in the manufacture of fertilizers. Which of the following is a common nitrogenous fertilizer produced using nitric acid?
28. Which of the following is a safety precaution when handling concentrated nitric acid?
29. The decomposition of nitric acid can be represented by the equation: 4HNO₃ → 4NO₂ + O₂ + 2H₂O. What is the role of nitric acid in this reaction?
30. Which of the following is a characteristic reaction of concentrated nitric acid with metals like gold and platinum?
31. The laboratory preparation of nitric acid involves heating a nitrate salt with concentrated sulfuric acid. What is the role of concentrated sulfuric acid in this reaction?
32. The brown ring test for nitrates is performed by adding ferrous sulphate solution and then slowly pouring concentrated sulphuric acid along the sides of the test tube. Why is it important to pour the concentrated sulphuric acid slowly and along the sides?
33. What is the balanced chemical equation for the reaction of phosphorus with concentrated nitric acid, producing phosphoric acid and nitrogen dioxide?
34. Nitric acid can be dehydrated by phosphorus pentoxide (P₂O₅). The product of this reaction is:
35. In the Ostwald process, the reaction between nitrogen monoxide and oxygen is:
36. Which of the following is NOT a characteristic property of nitric acid?
37. The reaction of bromine with nitric acid to form bromic acid and nitrogen dioxide is an example of:
38. What is the primary use of nitric acid in the explosives industry?
39. When iron reacts with very dilute nitric acid, it forms ferrous nitrate and ammonium nitrate. What are the oxidation states of nitrogen in the reactant and the products?
40. What is the primary function of concentrated sulfuric acid when used with nitric acid in the nitration of aromatic compounds like benzene?
41. Which of the following statements about the properties of nitric acid is FALSE?
42. Which of the following is a typical product when nitric acid reacts with sulphur dioxide?
43. The reaction of nitric acid with hydrogen gas (H₂) is:
44. What is the nature of the solution formed when nitric acid dissolves in water?
45. In the brown ring test, why is it important that the ferrous sulphate solution is freshly prepared?
46. Which of the following statements about the industrial production of nitric acid via the Ostwald process is INCORRECT?
47. When concentrated nitric acid reacts with charcoal (carbon), what are the main products?
48. Nitric acid is a powerful nitrating agent. What is the function of sulfuric acid when mixed with nitric acid for nitration?
49. Which of the following is a characteristic reaction of concentrated nitric acid with iodine?
50. The thermal decomposition of ammonium nitrate is commonly used to produce which gas for balloons and Whipple shields?
51. Nitric acid is stored in glass bottles because:
52. Which of the following metals does NOT react with dilute nitric acid?

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