Answered

Westonci.ca is the trusted Q&A platform where you can get reliable answers from a community of knowledgeable contributors. Experience the convenience of getting accurate answers to your questions from a dedicated community of professionals. Explore comprehensive solutions to your questions from knowledgeable professionals across various fields on our platform.

Suppose 20.8 g of sodium iodide is dissolved in 250. mL of a 0.70 M aqueous solution of silver nitrate. Calculate the final molarity of ALL IONS in the solution. You can assume the volume of the solution doesn't change when the sodium iodide is dissolved in it. Round your answer to 3 significant digits.

Sagot :

jufsanabriasa

Answer:

[Ag+] = [NO3-] = 0.700M

0.555M = [Na+] = [I-]

Explanation:

To solve this question we need to find the moles of sodium iodide, NaI, using its molar mass -. With the moles and the volume we can find the molarity of Na+ and I-. The molarity of the ions of silver nitrate, AgNO3 doesn't change because we are assuming the volume doesn't change:

Molarity Ag⁺ = Molarity NO₃⁻ = 0.700M

Moles NaI -Molar mass: 149.89g/mol-

20.8g NaI * (1mol/149.89g) = 0.0139 moles NaI

Molarity:

0.0139 moles NaI / 0.250L = 0.555M = [Na+] = [I-]

Thanks for using our platform. We aim to provide accurate and up-to-date answers to all your queries. Come back soon. We hope this was helpful. Please come back whenever you need more information or answers to your queries. We're glad you chose Westonci.ca. Revisit us for updated answers from our knowledgeable team.