Ch-8 Chemical Equilibrium Leave a Comment / By abdulslambsn@gmail.com / October 6, 2025 Welcome To Your Quiz "Ch-8 Chemical Equilibrium" Click on "Start Quiz" To Continue... 1. The value of pH and pOH of pure water at 25°C is approximately: 14 7 1 x 10-14 1 x 10 14 None 2. Conjugate acid of a very strong base is relatively: Very strong acid Weak acid Very weak acid strong acid None 3. Molarity of pure water is: 1 18 55.5 6 None 4. By adding NH4CI to NH4OH solution, the ionization of NH4OH: Increases Decreases Remain same Increases 100 times None 5. When Kc value is small, the equilibrium position is: Towards left Towards right Remains unchanged None of these None 6. A basic buffer solution can be prepared by mixing: A strong acid and salt with weak base Weak base and its salt with strong acid Strong base and its salt with weak acid Weak acid and its salt with strong base None 7. The term pH was introduced by: Henderson Sorenson Goldstein Thomson None 8. The solubility of KCIO3 in water is suppressed by adding: NaCIO3 NaCl KMNO4 KCI None 9. The ionic product of water will increase if: H+ ions are added OH ion are added Temperature is increased H+ and OH ions are added in equal amount. None 10. Which of the following factor affects on equilibrium constant? Change in temperature Change in concentration Change in Pressure Change in volume None 11. Which one of the following salt dissolves in water to form a solution with pH greater than 7? NaCl CuSO4 Na2CO3 NH4CI None 12. pH of milk is 6.5, its pOH will be: 14 7.5 7 None of these None 13. Formation of NH3 is an exothermic reaction. Low temperature favors forward reaction. However, in Haber's process temperature used is: 200°C 300°C 400°C 500°C None 14. When KCI is added to a saturated solution of KCIO3, the equilibrium is shifted to the: Forward direction Backward direction Not affected All of these None 15. pH of rain water is: 5,5 6.0 6.2 6.4 None 16. Strength of an acid can be determined by: pKa pH Ka All of these None 17. Solubility of Ca(OH)2 is exothermic, its solubility will increase: At high temperature At low temperature Temperature independent None None 18. Buffer action can be explained by: Common ion effect Law of mass action Le-Chatlier's principle All of these None 19. pH of a buffer solution having 0.01M CH3COONa and 0.1M CH3COOH (pKa = 4.74) is: 4.74 3.74 5.74 0 None 20. The pH of soft drink is: >7 <7 7 0 None 21. The pH of human blood is: 7.0 7.35 7.85 6.65 None 22. Almost forward reaction is complete when: Kc is very large Kc is very small Moderate Kc value None of these None 23. Equilibrium constant for gaseous equilibrium is represented by: Ka Kc Kx Kp None 24. The suppression or ionization of weak acid or a weak base by adding one of its own ions is: Buffer action Common ion effect Buffer capacity Ionization effect None 25. Law of mass action was derived by Guldberg and wage in: 1909 1906 1846 1864 None 1 out of 5 Thanks For Taking This Quiz - Please See Your Answers/Results Below After Entering Your Name & Email... Name Email Time's up
