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Chapter 12: Problem 98

Define molarity.

Short Answer

Expert verified
Molarity is a measure of the concentration of a solute in a solution, expressed in moles of solute per liter of solution (mol/L), and denoted by the letter M. The formula for calculating molarity is \(M = \frac{n}{V}\), where \(M\) is the molarity, \(n\) is the number of moles of solute, and \(V\) is the volume of the solution in liters. It is a crucial concept in chemistry for comparing concentrations of different solutions and performing calculations involving chemical reactions.

Step by step solution

01

Definition of Molarity

Molarity is a measure of the concentration of a solute in a solution, expressed as the number of moles of solute per liter of solution (mol/L). It is often denoted by the letter M. This allows us to easily compare the concentrations of different solutions and perform calculations involving chemical reactions.
02

Formula for Calculating Molarity

The formula for calculating molarity (M) is given by the following equation: \[M = \frac{n}{V}\] where: - \(M\) is the molarity (mol/L) - \(n\) is the number of moles of solute (mol) - \(V\) is the volume of the solution (L)
03

Understanding Molarity

To better understand molarity, let's consider an example. Suppose we have 1 mole of sodium chloride (NaCl) dissolved in 1 liter of water. The molarity of this sodium chloride solution would be: \[M = \frac{1 \, \text{mol of NaCl}}{1 \, \text{L of solution}}\] Therefore, the molarity of this solution is 1 mol/L, or simply 1 M.
04

Using Molarity in Calculations

Molarity can be used in various calculations involving chemical reactions. For example, in a titration experiment, the molarity and volume of one reactant can be used to determine the molarity of another reactant: \[M_1V_1 = M_2V_2\] where: - \(M_1\) and \(M_2\) are the molarities of the two reactants - \(V_1\) and \(V_2\) are the volumes of the respective reactants In summary, molarity is a crucial concept in chemistry that helps us define the concentration of a solution and enables us to perform calculations involving chemical reactions.

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Most popular questions from this chapter

Give precise instructions to your laboratory assistant as to how to prepare \(1.00 \mathrm{~L}\) of a \(1.00 \mathrm{M}\) aqueous solution of sucrose, \(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\). Remember that she will be measuring out the sucrose in grams. She has available a 1-L volumetric flask.

Draw pictures illustrating the solute-solvent interactions and the solvent- solvent interactions for methanol, \(\mathrm{CH}_{3} \mathrm{OH}\), in water. Is this a case of like dissolves like? Explain.

Your boss says, "Prepare \(0.5000 \mathrm{~kg}\) of a \(1.00 \%\) solution of hexane \(\left(\mathrm{C}_{6} \mathrm{H}_{14}\right.\), a liquid) in dichloromethane \(\left(\mathrm{CH}_{2} \mathrm{Cl}_{2}\right.\), also a liquid). \({ }^{\prime}\) (a) What is wrong with his request? (b) How would you prepare this solution if he meant a \(1.00 \%\) by mass solution?

A \(50.00\) -mL sample of hydrochloric acid of unknown concentration was neutralized by \(47.35 \mathrm{~mL}\) of \(0.01020 \mathrm{M}\) sodium hydroxide solution. Calculate the concentration of the original HCl solution.

Suppose \(200.0 \mathrm{~mL}\) of a \(2.50 \mathrm{M}\) solution of sodium hydroxide is combined with \(100.0 \mathrm{~mL}\) of a \(1.50 \mathrm{M}\) solution of iron(III) nitrate. (a) Write a net ionic equation for the formation of the expected precipitate. (b) What is the theoretical yield of precipitate in grams? (c) Suppose only \(10.95 \mathrm{~g}\) of precipitate is isolated. What is the percent yield for the reaction? (d) What is the molar concentration of the excess reactant in the combined solution?
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