Use the periodic table in the tools bar to answer these questions. How many moles of AgNO3 are present in 1.50 L of a 0.050 M solution?

The problem provides the volume and molarity of an AgNO3 solution.
We use the formula: Moles = Molarity × Volume .
Substituting the given values, we have: Moles of AgNO3 = 0.050 L mol ​ × 1.50 L .
The number of moles of AgNO3 is 0.075 mol ​ .

Explanation

Problem Analysis We are given a solution of AgNO3 with a volume of 1.50 L and a molarity of 0.050 M. We need to find the number of moles of AgNO3 present in this solution.

Formula Molarity (M) is defined as the number of moles of solute per liter of solution. In this case, the solute is AgNO3, and the solution is the 1.50 L mixture. We can use the formula: Moles = Molarity × Volume

Substitution Now, we plug in the given values: Moles of AgNO3 = 0.050 L mol ​ × 1.50 L

Calculation Calculating the product: Moles of AgNO3 = 0.075 mol

Final Answer Therefore, there are 0.075 moles of AgNO3 present in 1.50 L of a 0.050 M solution.


Examples
In chemistry, calculating the number of moles of a substance in a solution is crucial for performing stoichiometric calculations in reactions. For instance, if you need to react AgNO3 with another compound, knowing the exact number of moles allows you to determine the required amount of the other reactant to ensure a complete reaction. This is essential in fields like pharmaceutical research, environmental monitoring, and materials science, where precise chemical reactions are necessary for accurate results and the development of new products.

Answered by GinnyAnswer | 2025-07-03

There are 0.075 moles of AgNO3 in 1.50 L of a 0.050 M solution. This is calculated using the formula for moles, which is moles = molarity × volume. The calculation involves substituting the given values into the formula and performing the multiplication.
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Answered by Anonymous | 2025-07-04