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Chemical Equilibrium Test UHS MDCAT Preparation

UHS MCAT & MDCAT Entry Tests Chemistry Preparations

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Chemical Equilibrium Test UHS MDCAT Preparation

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Chemistry Chemical Equilibrium Test 1

Total No. of MCQs: 25
Time Limit: No

1 / 25

An excess of aqueous silver nitrate is added to aqueous barium chloride and precipitate is removed by filtration. What are the main ions in the filtrate?

2 / 25

Which of the solution among the following has highest pH?

3 / 25

The rate at which a substance reacts is directly proportional to its active mass and the rate of reaction is directly proportional to the product of the active masses of reacting substances in knows as?

4 / 25

Le-Chatelier’s principle is applied on the reversible reactions in order to:

5 / 25

When rate of forward reaction is equal to rate of backward reaction, then the equilibrium established is called:

6 / 25

Who introduced the term pH?

7 / 25

The ionic product of solution is greater than solubility product. The solution is:

8 / 25

The solubility product of AgCI is 2 x 10¯¹⁰ mol² dm¯⁶. The maximum concentration of Ag⁺ in the solution is:

9 / 25

The value of Kp is greater than Kc for a gaseous reaction when

10 / 25

The value of Kp is greater than Kc for a gaseous reaction when

11 / 25

The pH of buffer solution is 4.74. On adding 0.1 ml (0.00001M) HC1 solution, the pH of solution will be:

12 / 25

Chemical equilibrium involving reactants and products is more than one phase is known:

13 / 25

For which system does the equilibrium constant Kc has units of (concentration)¯¹?

14 / 25

The strongest base among the following is

15 / 25

What is the unit of equilibrium constant kc for the following reaction? H₂ + I₂ Ĝ ≈ 2HI

16 / 25

Who studied the effect of temperature on equilibrium?

17 / 25

Which statement about the following equilibrium is correct? 2SO₂(g) + O₂(g) ≈2SO₃(g) ∆H≈ - 188.3 kJmol¯¹

18 / 25

All of the following are the postulates of Arrhenius theory of ionization except:

19 / 25

Which is not true about buffer is a solution?

20 / 25

0.1 M HCI has pH = 1.0, it is about 100 times stronger than acetic acid. Then pH of acetic acid will be:

21 / 25

If the difference of pKa values of the two acids is 2, then:

22 / 25

The pH of 10¯³ mol dm ¯³ of an aqueous solution of H₂OS₄ is

23 / 25

Neutralization of a strong acid with a strong base is:

24 / 25

Hydrogen gas and iodine vapours combine to form HI at 425°C. The same composition of mixture is present if we start with decomposition of HI. It suggests.

25 / 25

Law of mass action states that rate of chemical reaction is directly proportional to the product of active masses of the reactants. The term active mass means

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