Textbook Question
Calculate the number of moles of solute present in each of the following aqueous solutions: (a) 600 mL of 0.250 M SrBr2,
Ch.13 - Properties of Solutions
Chapter 13, Problem 52a
Calculate the number of moles of solute present in each of the following solutions: (a) 255 mL of 1.50 M HNO3(aq),
Verified step by step guidance1
Convert the volume from milliliters to liters by dividing by 1000.
Use the formula for molarity: \( M = \frac{n}{V} \), where \( M \) is the molarity, \( n \) is the number of moles, and \( V \) is the volume in liters.
Rearrange the formula to solve for the number of moles: \( n = M \times V \).
Substitute the given values into the equation: \( n = 1.50 \, \text{M} \times 0.255 \, \text{L} \).
Calculate the number of moles by performing the multiplication.
Verified video answer for a similar problem:
This video solution was recommended by our tutors as helpful for the problem above.
Video duration:
51sWas this helpful?
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Molarity (M)
Molarity is a measure of concentration defined as the number of moles of solute per liter of solution. It is expressed in moles per liter (mol/L). Understanding molarity is essential for calculating the amount of solute in a given volume of solution, as it directly relates the volume of the solution to the number of moles present.
Recommended video:
Guided course
00:53
Molarity Concept
Volume Conversion
In chemistry, it is often necessary to convert between different units of volume. In this case, milliliters (mL) must be converted to liters (L) since molarity is defined in terms of liters. The conversion factor is 1 L = 1000 mL, which is crucial for accurately calculating the number of moles of solute in a solution.
Recommended video:
Guided course
02:38Common Conversion Factors
Calculating Moles from Molarity
To find the number of moles of solute in a solution, the formula used is: moles = molarity × volume (in liters). This relationship allows for the direct calculation of moles when both the molarity and the volume of the solution are known, making it a fundamental concept in solution chemistry.
Recommended video:
Guided course
03:12Molar Mass Calculation Example
Related Practice
Textbook Question
Calculate the number of moles of solute present in each of the following aqueous solutions: (b) 86.4 g of 0.180 m KCl,
Textbook Question
Calculate the number of moles of solute present in each of the following aqueous solutions: (c) 124.0 g of a solution that is 6.45% glucose (C6H12O6) by mass.
Textbook Question
Describe how you would prepare each of the following aqueous solutions, starting with solid KBr: (b) 125 g of 0.180 m KBr,
Textbook Question
Describe how you would prepare each of the following aqueous solutions, starting with solid KBr: (c) 1.85 L of a solution that is 12.0% KBr by mass (the density of the solution is 1.10 g/mL)