Acids, Bases and Salts

Which of the following is NOT a property of bases?

 
 
 
 

NH₃ cannot be classified as a base by which theory?

 

 
 
 
 

Consider the following reaction: H₂O + HCl → H₃O⁺ + Cl⁻. Which species is an electron pair acceptor in this reaction?

 

 
 
 
 

When an acid and a base react, the products formed are:

 
 
 
 

Milk of magnesia contains Mg(OH)₂. It neutralizes excess stomach acid. Which salt is formed in this reaction?

 

 
 
 
 

Choose Lewis acid:

 

 
 
 
 

Which of the following is NOT a characteristic of acids?

 
 
 
 

Which of the following is a strong acid?

 

 
 
 
 

In the following reaction, which species is donating an electron pair? NH₃ + BF₃ → [NH₃-BF₃]:

 

 

 

 
 
 
 

Which of the following cannot be classified as an Arrhenius acid?

 

 
 
 
 

Which of the following is true for a Lewis acid?

 
 
 
 

What is the conjugate acid of in the following reaction?

NH₃ + H₂O → NH₄+ + OH–

 
 
 

Which of the following is a salt formed when NaOH reacts with HCl?

 
 
 
 

An aqueous solution of NaOH is used as a drain cleaner. If the concentration of OH⁻ ions in this solution is 1.0 x 10⁻⁴ M, the concentration of H⁺ ions in it would be?

 
 
 
 

Which of the following statements about bases is correct?

 

 
 
 
 

Which of the following compounds is considered a weak acid?

 

 
 
 
 

Ammonia is a base because it:

 

 
 
 
 

A drain cleaner solution contains 1.0 x 10⁻⁸ M OH⁻. This solution is:

 

 
 
 
 

What is the pH of a neutral solution at 25°C?

 
 
 
 

Which of the following is a Lewis base?

 

 
 
 
 

Question 1 of 20

Related Questions:

  1. ACIDS, BASES AND SALTS
  2. Define acids with examples.
  3. Define bases, write their properties and examples aswell.
  4. Define salts, write its properties and examples also.
  5. Discuss the uses of acids, bases, and salts in detail.
  6. 1. Write the equation for the self-ionization of water?
  7. Define and give examples of Arrhenius acids?
  8. Why H⁺ ion acts as a Lewis acid?
  9. Why BF₃ acts as a Lewis acid?
  10. Define a conjugate acid-base pair.
  11. What is the role of indicators in acid-base titrations?
  12. What is meant by the neutralization reaction?
  13. What is the pH range of acids and bases?
  14. Explain why water is considered neutral.
  15. How does a strong acid differ from a weak acid?
  16. Define the term “ionization constant” (Ka) for acids.
  17. What is the difference between a monoprotic acid and a diprotic acid?
  18. Explain the pH scale, its importance, and the calculation of pH in detail.
  19. Describe the process of neutralization. Write the balanced chemical equation and discuss its applications.
  20. CHEMICAL EQUILIBRIUM