1. What is the pH of a neutral solution at 25^circ C a) b) 0 c) 14 2. Which of the following salts has a pHgt 7 __ a) NaCl b) Na2CO3 c) NH_(3) d) H2O 3. Which solution would have the highest pH? a) 0.01 M NaOH b) 0.01 M HCl c) 0.001 MHCI d)pure water 4. A weak acid is one that: a) Dissociates completely in solution b) Partially dissociates in solution c) Does not dissociate at all d) Has a pH of less than 7 5. The conjugate base of HCl is: a) Cl- b) H3O+ c) H2Cl d) Cl2 6. In water, which compound acts as a Bransted-Lowry acid? a) NH3 b) H2O c) HCl d) CH4 7. Which of the following has the lowest pH? a) &T M NaCl b) 0.1 M H2SO4 c) 0.1 M NaOH d) 0.1 M CH3COOH 8. The dissociation constant for acetic acid (CH3COOH) is known as: a) KW b) Ka c) Kb d) Ksp 9. Which of the following is a buffer solution? a) HCl and NaCl b) NH3 and NH4Cl c) NaOH and HCl d) H2O 10. The pH/of a 0.001 M HCl solution is: a) 3/6) 1 c) 0.1 d) 2 11. When an acid donates a proton, it becomes a: a) Stronger acid b)Conjugate base c)Weak aci(d d)Neutral prolecule 12. What is the pH of a 0.1 M NaOH solution? a) 11 by 1 c) 12 d)13 12. The term "pKa''refers to: a) The negative logarithm of the acid dissociation constant b) The concentration of hydrogen ions c) The strength of the base

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1. What is the pH of a neutral solution at 25^circ C a) b) 0 c) 14 2. Which of the following salts has a pHgt 7 __ a) NaCl b) Na2CO3 c) NH_(3) d) H2O 3. Which solution would have the highest pH? a) 0.01 M NaOH b) 0.01 M HCl c) 0.001 MHCI d)pure water 4. A weak acid is one that: a) Dissociates completely in solution b) Partially dissociates in solution c) Does not dissociate at all d) Has a pH of less than 7 5. The conjugate base of HCl is: a) Cl- b) H3O+ c) H2Cl d) Cl2 6. In water, which compound acts as a Bransted-Lowry acid? a) NH3 b) H2O c) HCl d) CH4 7. Which of the following has the lowest pH? a) &T M NaCl b) 0.1 M H2SO4 c) 0.1 M NaOH d) 0.1 M CH3COOH 8. The dissociation constant for acetic acid (CH3COOH) is known as: a) KW b) Ka c) Kb d) Ksp 9. Which of the following is a buffer solution? a) HCl and NaCl b) NH3 and NH4Cl c) NaOH and HCl d) H2O 10. The pH/of a 0.001 M HCl solution is: a) 3/6) 1 c) 0.1 d) 2 11. When an acid donates a proton, it becomes a: a) Stronger acid b)Conjugate base c)Weak aci(d d)Neutral prolecule 12. What is the pH of a 0.1 M NaOH solution? a) 11 by 1 c) 12 d)13 12. The term "pKa''refers to: a) The negative logarithm of the acid dissociation constant b) The concentration of hydrogen ions c) The strength of the base

Answer 1

Let's go through each question one by one: 1. **What is the pH of a neutral solution at \(25^{\circ}C\)?** - The pH of a neutral solution at \(25^{\circ}C\) is 7. 2. **Which of the following salts has a \(pH > 7\)?** - b) \(Na_2CO_3\) (Sodium carbonate is basic in nature, leading to a pH greater than 7.) 3. **Which solution would have the highest pH?** - a) 0.01 M \(NaOH\) (Sodium hydroxide is a strong base, resulting in a high pH.) 4. **A weak acid is one that:** - b) Partially dissociates in solution 5. **The conjugate base of \(HCl\) is:** - a) \(Cl^-\) 6. **In water, which compound acts as a Bronsted-Lowry acid?** - c) \(HCl\) (Hydrochloric acid donates protons in water.) 7. **Which of the following has the lowest pH?** - b) 0.1 M \(H_2SO_4\) (Sulfuric acid is a strong acid, resulting in a low pH.) 8. **The dissociation constant for acetic acid \((CH_3COOH)\) is known as:** - b) \(K_a\) (Acid dissociation constant) 9. **Which of the following is a buffer solution?** - b) \(NH_3\) and \(NH_4Cl\) (This combination can resist changes in pH.) 10. **The pH of a 0.001 M HCl solution is:** - a) 3 (Since HCl is a strong acid, the pH is calculated as \(-\log(0.001) = 3\).) 11. **When an acid donates a proton, it becomes a:** - b) Conjugate base 12. **What is the pH of a 0.1 M NaOH solution?** - d) 13 (Since NaOH is a strong base, the pH is calculated as \(14 - \log(0.1) = 13\).) 13. **The term "pKa" refers to:** - a) The negative logarithm of the acid dissociation constant

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