Inorganic Chemistry Study Resources for Competitive Exams

Inorganic Chemistry

Acids, Bases and Salts Acids, Bases and Salts - Advanced Concepts Acids, Bases and Salts - Applications Acids, Bases and Salts - Case Studies Acids, Bases and Salts - Competitive Exam Level Acids, Bases and Salts - Higher Difficulty Problems Acids, Bases and Salts - Numerical Applications Acids, Bases and Salts - Problem Set Acids, Bases and Salts - Real World Applications General Principles of Metallurgy General Principles of Metallurgy - Advanced Concepts General Principles of Metallurgy - Applications General Principles of Metallurgy - Case Studies General Principles of Metallurgy - Competitive Exam Level General Principles of Metallurgy - Higher Difficulty Problems General Principles of Metallurgy - Numerical Applications General Principles of Metallurgy - Problem Set General Principles of Metallurgy - Real World Applications Hydrogen and its Compounds Hydrogen and its Compounds - Advanced Concepts Hydrogen and its Compounds - Applications Hydrogen and its Compounds - Case Studies Hydrogen and its Compounds - Competitive Exam Level Hydrogen and its Compounds - Higher Difficulty Problems Hydrogen and its Compounds - Numerical Applications Hydrogen and its Compounds - Problem Set Hydrogen and its Compounds - Real World Applications Periodic Table and Periodicity Periodic Table and Periodicity - Advanced Concepts Periodic Table and Periodicity - Applications Periodic Table and Periodicity - Case Studies Periodic Table and Periodicity - Competitive Exam Level Periodic Table and Periodicity - Higher Difficulty Problems Periodic Table and Periodicity - Numerical Applications Periodic Table and Periodicity - Problem Set Periodic Table and Periodicity - Real World Applications Transition Elements and Coordination Chemistry Basics Transition Elements and Coordination Chemistry Basics - Advanced Concepts Transition Elements and Coordination Chemistry Basics - Applications Transition Elements and Coordination Chemistry Basics - Case Studies Transition Elements and Coordination Chemistry Basics - Competitive Exam Level Transition Elements and Coordination Chemistry Basics - Higher Difficulty Problems Transition Elements and Coordination Chemistry Basics - Numerical Applications Transition Elements and Coordination Chemistry Basics - Problem Set Transition Elements and Coordination Chemistry Basics - Real World Applications

Q. How many grams of sodium chloride are needed to prepare 0.5 L of a 0.2 M solution?

A. 5.84 g
B. 11.68 g
C. 2.92 g
D. 0.58 g

Solution

Molar mass of NaCl = 58.44 g/mol. Moles needed = 0.2 M * 0.5 L = 0.1 moles. Mass = moles * molar mass = 0.1 * 58.44 g = 5.844 g.

Correct Answer: B — 11.68 g

Q. How many moles of potassium hydroxide are needed to neutralize 0.1 moles of hydrochloric acid?

A. 0.05
B. 0.1
C. 0.2
D. 0.3

Solution

The reaction between KOH and HCl is 1:1. Therefore, 0.1 moles of HCl will require 0.1 moles of KOH.

Correct Answer: B — 0.1

Q. If 25 mL of 0.5 M acetic acid is mixed with 25 mL of 0.5 M sodium acetate, what is the resulting pH of the buffer solution?

A. 4.76
B. 5.00
C. 5.76
D. 6.00

Solution

Using the Henderson-Hasselbalch equation: pH = pKa + log([A-]/[HA]). pKa of acetic acid is approximately 4.76. Since [A-] = [HA], pH = 4.76.

Correct Answer: A — 4.76

Q. If 50 mL of 0.1 M sulfuric acid is neutralized by sodium hydroxide, how many moles of NaOH are required?

A. 0.005
B. 0.01
C. 0.02
D. 0.03

Solution

H2SO4 dissociates to give 2 H+ ions. Moles of H2SO4 = 0.1 M * 0.050 L = 0.005 moles. Therefore, moles of NaOH required = 0.005 moles * 2 = 0.01 moles.

Correct Answer: B — 0.01

Q. In redox reactions, what happens to the oxidation state of a transition metal when it acts as a reducing agent?

A. It increases
B. It decreases
C. It remains the same
D. It becomes zero

Solution

When a transition metal acts as a reducing agent, it donates electrons, resulting in a decrease in its oxidation state.

Correct Answer: B — It decreases

Q. In redox reactions, what happens to the oxidation state of a transition metal when it acts as an oxidizing agent?

A. It decreases
B. It increases
C. It remains the same
D. It becomes zero

Solution

When a transition metal acts as an oxidizing agent, its oxidation state increases as it gains electrons.

Correct Answer: B — It increases

Q. In redox reactions, which of the following statements is true?

A. Oxidation is the gain of electrons.
B. Reduction is the loss of electrons.
C. Oxidizing agents are reduced.
D. Reducing agents are oxidized.

Solution

Oxidizing agents are reduced as they gain electrons during redox reactions.

Correct Answer: C — Oxidizing agents are reduced.

Q. In the context of metallurgy, what does the term 'gangue' refer to?

A. The desired metal
B. The waste material
C. The reducing agent
D. The flux used

Solution

Gangue refers to the waste material that is separated from the desired metal during the extraction process.

Correct Answer: B — The waste material

Q. In the context of metallurgy, what does the term 'reduction' refer to?

A. Loss of electrons
B. Gain of electrons
C. Increase in oxidation state
D. Decrease in temperature

Solution

Reduction refers to the gain of electrons, which is essential in the extraction of metals.

Correct Answer: B — Gain of electrons

Q. In the context of metallurgy, what is the primary purpose of roasting a sulfide ore?

A. To reduce the ore
B. To oxidize the ore
C. To concentrate the ore
D. To purify the ore

Solution

Roasting a sulfide ore involves heating it in the presence of oxygen to convert it into an oxide, which is a necessary step for further extraction of the metal.

Correct Answer: B — To oxidize the ore

Q. In the context of redox reactions, what happens to a transition metal when it acts as a reducing agent?

A. It gains electrons.
B. It loses electrons.
C. It remains unchanged.
D. It forms a complex.

Solution

When a transition metal acts as a reducing agent, it loses electrons and is oxidized.

Correct Answer: B — It loses electrons.

Q. In the context of redox reactions, which transition metal is commonly used as a reducing agent?

A. Manganese
B. Iron
C. Copper
D. Silver

Solution

Iron is commonly used as a reducing agent in various redox reactions.

Correct Answer: B — Iron

Q. In the extraction of iron, what is the role of limestone?

A. To act as a reducing agent
B. To remove sulfur
C. To form slag
D. To increase temperature

Solution

Limestone is added to form slag, which helps remove impurities during the extraction of iron.

Correct Answer: C — To form slag

Q. In the extraction of metals, what is the role of a flux?

A. To increase the temperature of the reaction
B. To remove impurities
C. To provide energy for the reaction
D. To act as a catalyst

Solution

A flux is used to remove impurities from the metal during the extraction process.

Correct Answer: B — To remove impurities

Q. In which application is hydrogen used as a reducing agent?

A. Electrolysis
B. Metal extraction
C. Acid-base neutralization
D. Combustion

Solution

Hydrogen acts as a reducing agent in the extraction of metals from their ores, such as in the reduction of metal oxides.

Correct Answer: B — Metal extraction

Q. In which of the following compounds does hydrogen act as a Lewis acid?

A. H2O
B. HCl
C. BF3
D. H2

Solution

In HCl, hydrogen can act as a Lewis acid by accepting an electron pair.

Correct Answer: B — HCl

Q. In which of the following coordination compounds does hydrogen act as a ligand?

A. [Fe(H2O)6]2+
B. [Cu(NH3)4]2+
C. [CoCl4]2-
D. [Ag(CN)2]-

Solution

In the complex [Fe(H2O)6]2+, water (H2O) acts as a ligand, coordinating with the iron ion.

Correct Answer: A — [Fe(H2O)6]2+

Q. In which of the following processes is hydrogen used to reduce metal ores?

A. Electrolysis
B. Hydrometallurgy
C. Pyrometallurgy
D. Hydrogen reduction

Solution

Hydrogen reduction is a process where hydrogen gas is used to reduce metal ores to their metallic form.

Correct Answer: D — Hydrogen reduction

Q. In which of the following reactions does hydrogen act as a reducing agent?

A. H2 + Cl2 → 2HCl
B. H2 + O2 → 2H2O
C. H2 + CuO → Cu + H2O
D. H2 + N2 → NH3

Solution

In the reaction H2 + CuO → Cu + H2O, hydrogen reduces copper(II) oxide to copper.

Correct Answer: C — H2 + CuO → Cu + H2O

Q. In which oxidation state does manganese exhibit the highest oxidation state?

A. +2
B. +4
C. +6
D. +7

Solution

Manganese exhibits the highest oxidation state of +7 in permanganate ion (MnO4-).

Correct Answer: D — +7

Q. What is the bond angle in the H2O molecule?

A. 90 degrees
B. 104.5 degrees
C. 120 degrees
D. 180 degrees

Solution

The bond angle in H2O is approximately 104.5 degrees due to the bent shape of the molecule caused by the two lone pairs on the oxygen atom.

Correct Answer: B — 104.5 degrees

Q. What is the concentration of hydroxide ions in a solution with a pH of 11?

A. 1 x 10^-3 M
B. 1 x 10^-4 M
C. 1 x 10^-5 M
D. 1 x 10^-6 M

Solution

pOH = 14 - pH = 14 - 11 = 3. [OH-] = 10^-pOH = 10^-3 M.

Correct Answer: A — 1 x 10^-3 M

Q. What is the conjugate base of H2SO4?

A. HSO4-
B. SO4^2-
C. H3O+
D. H2O

Solution

The conjugate base of H2SO4 is HSO4-, formed when H2SO4 donates a proton (H+).

Correct Answer: A — HSO4-

Q. What is the coordination number of hydrogen in the complex ion [H2O]2+?

A. 1
B. 2
C. 3
D. 4

Solution

In the complex ion [H2O]2+, the coordination number of hydrogen is 2.

Correct Answer: B — 2

Q. What is the coordination number of the central metal ion in a complex with the formula [Co(NH3)6]Cl3?

A. 2
B. 4
C. 6
D. 8

Solution

The coordination number is determined by the number of ligands attached to the central metal ion. In this case, there are six NH3 ligands, giving a coordination number of 6.

Correct Answer: C — 6

Q. What is the coordination number of the central metal ion in the complex [Cu(NH3)4]SO4?

A. 2
B. 4
C. 6
D. 8

Solution

The coordination number of copper in [Cu(NH3)4]SO4 is 4, as it is surrounded by four ammonia ligands.

Correct Answer: B — 4

Q. What is the coordination number of the central metal ion in the complex [Fe(CN)6]3-?

A. 2
B. 4
C. 6
D. 8

Solution

The coordination number is 6 because there are six cyanide ligands coordinated to the iron ion.

Correct Answer: C — 6

Q. What is the coordination number of the complex ion [Co(NH3)6]Cl3?

A. 2
B. 4
C. 6
D. 8

Solution

The coordination number is 6 because there are six ammonia ligands coordinated to the cobalt ion.

Correct Answer: C — 6

Q. What is the coordination number of the complex ion [Cu(NH3)4]2+?

A. 2
B. 4
C. 6
D. 8

Solution

The coordination number of [Cu(NH3)4]2+ is 4, as it has four ammonia ligands.

Correct Answer: B — 4

Q. What is the coordination number of the complex ion [Ni(CN)4]2-?

A. 2
B. 4
C. 6
D. 8

Solution

The coordination number of [Ni(CN)4]2- is 4, as it has four cyanide ligands coordinated to the nickel ion.

Correct Answer: B — 4

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