Class 10 Practice Level 3 - Acids, Bases and Salts - Set 1

Total questions: 15

In a titration experiment , 25.0 mL of 0.1 M HCL is completely neutralized by 30.0 mL of NaOH solution . What is the concentration of the NaOH solution ?

Topic: Titration

0.083 M

0.125 M

0.167 M

0.200 M

None

Calculate the pH of a solution formed by mixing 50 mL of 0.1 M HCl with 50 mL of 0.1 M NaOH .

Topic: pH calculation

None

Which of the following mixtures will form a butter solution?

Topic: Buffer Solutions

$ \displaystyle HCl \text{ and}\text{ }NaOH$

$ \displaystyle HCl\text{ and}\text{ }NaCl$

$ \displaystyle C{{H}_{3}}COOH\text{ and}\text{ }C{{H}_{3}}COONa$

$ \displaystyle {{H}_{2}}S{{O}_{4}}\text{ and }N{{a}_{2}}S{{O}_{4}}$

None

What is the solubility product constant (Ksp) expression for calcium fluoride ,$ \displaystyle Ca{{F}_{2}}$ ?

Topic: Solubility Product

$ \displaystyle {{K}_{{sp}}}=\left[ {c{{a}^{{2+}}}} \right]\left[ {{{F}^{-}}} \right]$

$\displaystyle {{K}_{{sp}}}=\left[ {c{{a}^{{2+}}}} \right]{{\left[ {{{F}^{-}}} \right]}^{2}}$

$ \displaystyle {{K}_{{sp}}}={{\left[ {c{{a}^{{2+}}}} \right]}^{2}}\left[ {{{F}^{-}}} \right]$

$\displaystyle {{K}_{{sp}}}={{\left[ {c{{a}^{{2+}}}} \right]}^{2}}{{\left[ {{{F}^{-}}} \right]}^{2}}$

None

Calculate the pH of a 0.01M solution of acetic acid $ \displaystyle \left( {Ka=1.8\times {{{10}}^{{-5}}}} \right)$ .

Topic: pH of Weak Acid

3.4

4.2

5.0

6.1

None

Which of the following salts, when dissolved in water, will produce an acidic solution?

Topic: Electrolytic Dissociation

$ \displaystyle NaCl$

$ \displaystyle N{{a}_{2}}C{{O}_{3}}$

$ \displaystyle N{{H}_{4}}Cl$

$ \displaystyle KN{{O}_{3}}$

None

Using the Henderson-Hasselbalch equation ,calculate the pH of a buffer solution containing 0.1 M acetic acid and 0.1 M sodium acetate (pKa of acetic acid is 4.76).

Topic: Henderson-Hasselbalch equation

3.76

4.76

6.76

5.76

None

Which of the following illustrates the common ion effect?

Topic: Common ion Effect

Adding NaOH to $ \displaystyle N{{H}_{3}}$ Solution decreases its solubility

Adding HCl to NACl Solution decreases its solubility

Adding NACl to a saturated AgCl Solution decreases its solubility

Adding $ \displaystyle N{{H}_{4}}Cl$ to $ \displaystyle N{{H}_{3}}$ Solution increases its solubility

None

In an acid-base titration, which indicator would be suitable for titrating a weak acid with a strong base?

Topic: Acid - Base titration

Methyl orange

Bromothymol blue

Phenolphthalein

Litmus

None

10.

Which of the following salts will produce a neutral solution when dissolved in water ?

Topic: pH of Salts

$ \displaystyle {{K}_{2}}S{{O}_{4}}$

$ \displaystyle NaHS{{O}_{4}}$

$ \displaystyle N{{H}_{4}}N{{O}_{3}}$

$ \displaystyle N{{a}_{2}}C{{O}_{3}}$

None

11.

Which salt will hydrolyze to form an acidic solution ?

Topic: Hydrolysis Of Salts

$ \displaystyle N{{a}_{2}}HS{{O}_{4}}$

$ \displaystyle KCl $

$ \displaystyle NaHC{{O}_{3}}$

$\displaystyle N{{H}_{4}}N{{O}_{3}}$

None

12.

Calculate the pH of 0.01 M $ \displaystyle N{{H}_{3}}$ solution (kb for $ \displaystyle N{{H}_{3}}$ is $ \displaystyle {1.8\times {{{10}}^{{-5}}}}$)

Topic: pH of Weak Base

9.26

10.74

11.13

8.75

None

13.

Which of the following pairs can act as a buffer solution?

Topic: Buffer

$ \displaystyle N{{H}_{4}}OH\text{ and }N{{H}_{4}}Cl$

$ \displaystyle NaOH\text{ and }KCl $

$ \displaystyle {{H}_{2}}S{{O}_{4}}\text{ and }{{K}_{2}}S{{O}_{4}}$

$ \displaystyle HCl\text{ and }NaCl $

None

14.

What is the effect of adding a common ion solubility of a sparingly soluble salt?

Topic: Solubility Product

Solubility increases

Solubility decreases

No effect no Solubility

Solubility first increases then decreases

None

15.

Which of the following is a Lewis acid?

Topic: Lewis Acid And Bases

$ \displaystyle N{{H}_{3}}$

$ \displaystyle {O{{H}^{-}}}$

$ \displaystyle B{{F}_{3}}$

$ \displaystyle {{H}_{2}}O$

None

1 out of 15

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Class 10 Practice Level 3 - Acids, Bases and Salts - Set 1

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