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Ch.4 - Reactions in Aqueous Solution
All textbooksMcMurry 8th EditionCh.4 - Reactions in Aqueous SolutionProblem 46a
Chapter 4, Problem 46a

How many moles of solute are present in each of the following solutions? (a) 35.0 mL of 1.200 M HNO3

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Determine the formula for calculating moles from molarity and volume: \( \text{moles} = \text{molarity} \times \text{volume in liters} \).
Convert the volume from milliliters to liters: \( 35.0 \text{ mL} = 0.0350 \text{ L} \).
Substitute the given values into the formula: \( \text{moles} = 1.200 \text{ M} \times 0.0350 \text{ L} \).
Perform the multiplication to find the number of moles.
Ensure the units are consistent and the calculation is correct.

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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 crucial 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.
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Molarity Concept

Volume Conversion

In chemistry, it is often necessary to convert volumes from milliliters (mL) to liters (L) when working with molarity. Since 1 L equals 1000 mL, converting mL to L involves dividing the volume in mL by 1000. This conversion is essential for accurately applying the molarity formula to determine the number of moles of solute.
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Common 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 straightforward calculation of moles when both the molarity and the volume of the solution are known. It is a fundamental concept in stoichiometry and solution chemistry.
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Molar Mass Calculation Example
Related Practice
Textbook Question

Assume that the electrical conductivity of a solution depends on the total concentration of dissolved ions and that you measure the conductivity of three different solutions while carrying out titration procedures: (a) Begin with 1.00 L of 0.100 M KCl, and titrate by adding 0.100 M AgNO3. (b) Begin with 1.00 L of 0.100 M HF, and titrate by adding 0.100 M KOH. (c) Begin with 1.00 L of 0.100 M BaCl2, and titrate by adding 0.100 M Na2SO4. Which of the following graphs corresponds to which titration?

Textbook Question

Based on the positions in the periodic table, which of the following reactions would you expect to occur? (a) Red+ + Green → Red + Green+ (b) Blue + Green+ → Blue+ + Green (c) Red + Blue+ → Red+ + Blue

Textbook Question

The following two redox reactions occur between aqueous cations and solid metals. Will a solution of green cations react with solid blue metal? Explain.

(a)

(b)

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