Sign Up

Sign Up to our social questions and Answers Engine to ask questions, answer people’s questions, and connect with other people.

Have an account?

Sign In

Login to our social questions & Answers Engine to ask questions answer people’s questions & connect with other people.

Don't have account,

Forgot Password

Lost your password? Please enter your email address. You will receive a link and will create a new password via email.

Have an account?

You must login to ask a question.

Need An Account,

You must login to add post.

Need An Account,

Please briefly explain why you feel this question should be reported.

Please briefly explain why you feel this answer should be reported.

Please briefly explain why you feel this user should be reported.

Search
Ask A Question
Home/ Chemistry/Chemistry MCQ with Answer Explanation : Chemical and Ionic Equilibrium.

love-insta : Question and Answer Sharing Platform. Latest Articles

On: October 13, 2024 Posted in Chemistry, Education, Exam Comments: 0 Views: 140

Chemistry MCQ with Answer Explanation : Chemical and Ionic Equilibrium.

31. If KcKc​ for a reaction is very small (much less than 1), what can be inferred about the equilibrium position?

a) The reaction favors the products.
b) The reaction favors the reactants.
c) The reaction reaches equilibrium very quickly.
d) The reaction does not proceed at all.

Answer: b) The reaction favors the reactants.

Explanation:
A small KcKc​ value means that the concentration of reactants at equilibrium is much higher than the concentration of products, so the reaction favors the reactants.

32. What will be the effect of adding NaCl to a solution of AgNO33​?

a) No effect
b) Decrease in the concentration of Ag++ ions
c) Increase in the concentration of Ag++ ions
d) Decrease in the concentration of Cl−− ions

Answer: b) Decrease in the concentration of Ag++ ions

Explanation:
Adding NaCl provides Cl−− ions, which react with Ag++ ions to form a precipitate of AgCl, decreasing the concentration of free Ag++ ions in solution.

33. Which of the following statements is true about a buffer solution?

a) It resists changes in pH when small amounts of acid or base are added.
b) It can be made only with a strong acid and its salt.
c) It becomes more effective as the pH is lowered.
d) Its pH changes drastically upon dilution.

Answer: a) It resists changes in pH when small amounts of acid or base are added.

Explanation:
A buffer solution maintains a nearly constant pH by neutralizing small amounts of added acid or base.

34. For the reaction 2SO2(g)+O2(g)⇌2SO3(g)2SO2​(g)+O2​(g)⇌2SO3​(g), which of the following will decrease the amount of SO33​?

a) Decreasing the pressure
b) Increasing the concentration of SO22​
c) Increasing the pressure
d) Adding a catalyst

Answer: a) Decreasing the pressure

Explanation:
Since the forward reaction results in fewer moles of gas (from 3 moles to 2 moles), decreasing the pressure will shift the equilibrium to the left, reducing the amount of SO33​.

35. What is the effect of adding NH44​Cl to a solution of NH33​?

a) The ionization of NH33​ decreases.
b) The ionization of NH33​ increases.
c) The pH of the solution increases.
d) The concentration of OH−− increases.

Answer: a) The ionization of NH33​ decreases.

Explanation:
NH44​Cl provides NH4+4+​ ions, which shift the equilibrium of the dissociation of NH33​ (a weak base) to the left, reducing its ionization (common ion effect).

36. Which of the following is a characteristic of a system in equilibrium?

a) The forward reaction has stopped.
b) The reverse reaction has stopped.
c) The concentrations of reactants and products remain constant over time.
d) The equilibrium constant changes with concentration.

Answer: c) The concentrations of reactants and products remain constant over time.

Explanation:
In equilibrium, the rates of the forward and reverse reactions are equal, so the concentrations of reactants and products do not change over time.

37. Which of the following statements is correct about the solubility product (KspKsp​)?

a) It depends on the concentration of the solid phase.
b) It increases with the addition of a common ion.
c) It decreases with the increase in temperature for most salts.
d) It is constant at a given temperature.

Answer: d) It is constant at a given temperature.

Explanation:
The solubility product (KspKsp​) is a constant for a given solute at a specific temperature. It depends only on temperature and not on the concentration of the solid phase or the addition of common ions.

38. In an acidic solution, which of the following species will increase in concentration when more acid is added?

a) OH−−
b) H++
c) Water molecules
d) Conjugate base

Answer: b) H++

Explanation:
Adding more acid increases the concentration of H++ ions (protons) in the solution, making it more acidic.

39. The equilibrium constant for a reaction is 50 at 500 K. If the temperature is raised to 600 K, what will likely happen to the equilibrium constant if the reaction is exothermic?

a) It will increase.
b) It will decrease.
c) It will remain the same.
d) It will first increase, then decrease.

Answer: b) It will decrease.

Explanation:
For an exothermic reaction, increasing the temperature shifts the equilibrium to the left, decreasing the value of the equilibrium constant.

40. The addition of a catalyst to a system at equilibrium will:

a) Shift the equilibrium to the right.
b) Shift the equilibrium to the left.
c) Decrease the equilibrium constant.
d) Increase the rate at which equilibrium is achieved.

Answer: d) Increase the rate at which equilibrium is achieved.

Explanation:
A catalyst increases the rate of both the forward and reverse reactions equally, allowing the system to reach equilibrium faster without changing the position of equilibrium or the equilibrium constant.

Previous article
Next article

Leave a comment