Latihan soal asam dan basa (dalam bhs Inggris)

A. MULTIPLE CHOISE

1.       Given the equation: H⁺ + OH^-           H₂O. Which type of reaction does the equation represent?

1. esterification
2. decomposition
3. hydrolysis
4. neutralization
5. combution

2.       Which substance can be classified as an Arrhenius acid?

1. HCL
2. NaCl
3. LiOH
4. KOH
5. NH₃

3.       Which solution will change red litmus to blue?

1. HCl(aq)
2. NaCl(aq)
3. CH₃OH(aq)
4. NaOH(aq)

4.       What is the pH of a 0.00001 molar HCl solution?

1. 1
2. 9
3. 5
4. 4
5. 3

 

5.       What is the pH of a solution with a hydronium ion concentration of 0.01 mole per liter?

1. 1
2. 2
3. 7
4. 10
5. 14 

6.       There are alternate acid base theories that define an acid as any species that can

1. donate a neutron
2. donate a proton
3. donate an electron
4. accept a proton
5. accept an electron

7.       Which 0.1 M solution will turn phenolphthalein pink?

1. HBr(aq)
2. CO₂(aq)
3. LiOH(aq)
4. CH₃OH(aq)
5. NH₃ (aq)

8.       When HCl(aq) is exactly neutralized by NaOH(aq), the hydrogen ion concentration in the resulting mixture is

1. always less than the concentration of the hydroxide ions
2. always greater than the concentration of the hydroxide ions
3. always equal than the concentration of the hydroxide ions
4. always zero the concentration of the hydroxide ions
5. sometimes greater and sometimes less than the concentration of the hydroxide ions

9.       An acidic solution could have a pH of

1. 7
2. 10
3. 3
4. 14
5. 8

10.   A student wishes to prepare approximately 100 milliliters of an aqueous solution of 6M HCl using 12 M HCl. Which procedure is correct?

1. adding 50 mL of 12 M HCl to 50 mL of water while stirring the mixture steadily.
2. adding 50 mL of 12 M HCl to 50 mL of water and then stirring the mixture steadily.
3. adding 50 mL of water to 50 mL of 12 M HCl while stirring the mixture steadily.
4. adding 50 mL of water to 50 mL of 12 M HCl and then stirring the mixture steadily.

11.   As the hydrogen ion concentration of an aqueous solution increases, the hydroxide ion concentration of this solution will

1. decrease
2. increase
3. remain the same

12.   The following data were collected at the endpoint of a titration performed to find the molarity of an HCl solution.
Volume of acid (HCl) used = 14.4 mL
Volume of base (NaOH) used = 22.4 mL
Molarity of standard base (NaOH) = 0.20 M
What is the molarity of the acid solution?

1. 1.6 M
2. 0.64 M
3. 0.31M
4. 0.13M

13.   The acid dissociation constant, Ka for a weak monobasic acid is 4 x 10^-5 mol dm^‑3. What is the pH of a 0.1 mol dm^-3 solution of the acid? (Log 2 = 0.3)

a.    1.00

b.    2.20

c.    2.70

d.    4.40

e.    4.00

14.   The pH of a 0.01 mol dm^-3 solution of monobasic acid is 4. What is the pKa for the acid?

a.    2

b.    3

c.    4

d.    6

e.    8

15.   Which one of the following solutions has the lowest pH?

a.    500 cm³ of 2.0 M CH₃COOH

b.    10 cm³ of 0.4 M H₂SO₄

c.    1 dm³ of 0.4 M HCl

d.    200 cm³ of 0.5 M HCl

e.    1000 cm³ of 4.0 M CH₃COOH

B.  ESSAY

1.         For a 0.1 M solution of HCl calculate the equlibrium concentration of  H₃O⁺ !

2.         For a 0.1 M solution of KOH calculate the equlibrium concentration of H₃O⁺ !

3.         For a 0.1 M solution of acetic acid (K_a = 1.8*10^-5) calculate the equlibrium concentration of CH₃COO^- !

4.         For a 0.1 M solution of Ammonia (K_b = 1.78*10^-5) calculate the equlibrium concentration of

a.    NH₃

b.    NH₄¹⁺

c.    H₃O¹⁺

d.    OH^1-

5.         What are the characteristic of acid and base?

6.         Give the examples of strong acid (4) and weak acid (4)!

7.         Give the examples of strong base (4) and weak base (4)!

8.         Ka for a weak monobasic acis = 1.10^-5 M. In a 0.1 M solution of the acid, calculate

a.    The concentration oh H⁺ ion

b.    Tha pH

c.    The concentration of OH^- ion (Kw = 1.10^-14)

9.         A 0.1 M solution of a weak monobasic has a pH of 4.0. Calculate the value of Ka and pKa for the acid!

10.     The acid dissociation constant, Ka, for methanoic acid is 1.8 x 10^-4 M. In a 0.1 M solution of methanoic acid, calculate:

a.    The concentration of hydrogen ion

b.    pH

c.    the concentration of hydroxide ions

d.    the degree of ionisation of the acid (Kw = 1.10^-14)

Posted in: Latihan Soal Kelas XI