College

Thank you for visiting Determine the molarity of a solution formed by dissolving 97 7 g LiBr in enough water to yield 750 0 ml of solution A 1. This page is designed to guide you through key points and clear explanations related to the topic at hand. We aim to make your learning experience smooth, insightful, and informative. Dive in and discover the answers you're looking for!

Determine the molarity of a solution formed by dissolving 97.7 g LiBr in enough water to yield 750.0 ml of solution.

A) 1.50 M
B) 1.18 M
C) 0.130 M
D) 0.768 M
E) 2.30 M

Provide the complete ionic equation for the reaction that occurs when aqueous solutions of K₂S and Fe(NO₃)₂ are mixed.

Answer :

Final answer:

To calculate the molarity of a solution, you find the number of moles of solute and divide by the volume of the solution in liters. For 97.7 g of LiBr dissolved in 750.0 ml, the molarity is calculated to be 1.50 M. Therefore, the correct answer is option A.

Explanation:

To determine the molarity of a solution formed by dissolving 97.7 g LiBr in 750.0 ml of solution, we first need to calculate the molar mass of LiBr. Lithium bromide (LiBr) has a molar mass of about 86.85 g/mol (6.94 g/mol for Li and 79.90 g/mol for Br).

We then use the formula: molarity (M) = moles of solute / liters of solution. First, find the number of moles of LiBr:

  1. Number of moles = mass (g) / molar mass (g/mol)
  2. Number of moles = 97.7 g / 86.85 g/mol
  3. Number of moles = 1.125 moles (approximately)

Now convert milliliters to liters:

  1. Liters of solution = 750.0 ml / 1000 ml/L
  2. Liters of solution = 0.750 L

Finally, calculate the molarity:

  1. Molarity (M) = 1.125 moles / 0.750 L
  2. Molarity (M) = 1.50 M

Thus, the molarity of the LiBr solution is 1.50 M, which corresponds to option A.

Thank you for reading the article Determine the molarity of a solution formed by dissolving 97 7 g LiBr in enough water to yield 750 0 ml of solution A 1. We hope the information provided is useful and helps you understand this topic better. Feel free to explore more helpful content on our website!

Rewritten by : Jeany

Other Questions