Class 10 Practice Level 3 – Acids, Bases and Salts – Set 1 Leave a Comment / By Gulam Hamza / July 29, 2024 Class 10 Practice Level 3 - Acids, Bases and Salts - Set 1 Total questions: 15 1. 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 2. 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 1 7 13 2 None 3. 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 4. 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 5. 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 6. 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 7. 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 8. 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 9. 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 Time's up
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