Answered

Looking for trustworthy answers? Westonci.ca is the ultimate Q&A platform where experts share their knowledge on various topics. Get the answers you need quickly and accurately from a dedicated community of experts on our Q&A platform. Join our Q&A platform to connect with experts dedicated to providing accurate answers to your questions in various fields.

Shown above is information about the dissolution of AgCl(s) in water at 298K. In a chemistry lab a student wants to determine the value of s, the molar solubility of AgCl, by measuring [Ag+] in a saturated solution prepared by mixing excess AgCl and distilled water. How would the results of the experiment be altered if the student mixed excess AgCl with tap water (in which [Cl−]=0.010M) instead of distilled water and the student did not account for the Cl− in the tap water?

Sagot :

Answer:

Value for K would be too small. Less AgCl would dissolve due to the common ion effect due to the presence of Cl- in the water.

Explanation:

Think of this through the lenses of a shifting problem. Cl- ions are a product in this situation and increasing its concentration would shift the reaction back to the solid AgCl. In this specific case, due to Cl- ions, AgCl would dissolve less to maintain equilibrium and as a result, the concentrations of Ag+ and Cl- ions would be lower than normal making a smaller K value.

In the solution of AgCl in tap water, the dissociation constant K has been decreased.

The dissolution of silver chloride in water results in the formation of silver ions and chloride ions.

The dissociation constant has been the amount of compound that has been dissociated into the constituent ions at equilibrium.

Dissociation constant for AgCl

The dissociation constant has been dependent on the number of ions in the solution that has been present.

The common ion effect has been defined as the change in the dissociation constant for the compound with the presence of common ions in the solution.

The dissociation of AgCl in tap water has been resulted with presence of Cl ions in the solution. There has been early reach to the equilibrium in tap water.

Thus, with the solution of AgCl in tap water, the dissociation constant K has been decreased.

Learn more about dissociation constant, here:

https://brainly.com/question/7145687

Thanks for using our service. We aim to provide the most accurate answers for all your queries. Visit us again for more insights. We appreciate your time. Please revisit us for more reliable answers to any questions you may have. We're here to help at Westonci.ca. Keep visiting for the best answers to your questions.