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Chapter 1: Problem 85

How much mass of sodium acetate is required to make \(250 \mathrm{~mL}\) of \(0.575\) molar aqueous solution? (a) \(11.79 \mathrm{~g}\) (b) \(15.38 \mathrm{~g}\) (c) \(10.81 \mathrm{~g}\) (d) \(25.35 \mathrm{~g}-\mathrm{a}=\)

Short Answer

Expert verified
15.38 g of sodium acetate is required.

Step by step solution

01

Determine the Number of Moles Needed

Using the molarity formula Molarity = Moles of solute / Liters of solution, we can calculate the number of moles of sodium acetate needed for the solution. We have 0.575 moles/L and we want to make 250 mL (0.250 L) of the solution, so the moles of sodium acetate required is 0.575 moles/L x 0.250 L.
02

Calculate the Mass of Sodium Acetate Required

To find the mass, multiply the number of moles by the molar mass of sodium acetate (NaC2H3O2). The molar mass of sodium acetate is approximately 82.03 g/mol. Thus, the mass required is the number of moles from Step 1 multiplied by the molar mass of sodium acetate.
03

Check the Answer Choices

Calculate the product of the moles of sodium acetate and its molar mass to find the closest answer option.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Sodium Acetate
Sodium acetate, represented by the chemical formula NaC2H3O2, is a commonly used compound in laboratories and various industrial applications. It emerges from the reaction between sodium hydroxide and acetic acid, and it is often seen in the form of its three hydrate, NaC2H3O2·3H2O, showcasing its ability to form crystals with water molecules.

Sodium acetate has various real-world applications, including as a buffer solution in biochemistry labs to maintain a constant pH level, or in heating pads since it crystallizes in an exothermic process. Due to its versatile nature, understanding how to work with sodium acetate is an essential skill in chemistry.
Molar Mass
Molar mass is defined as the mass of one mole of a substance and is expressed in grams per mole (g/mol). It is calculated by summing the atomic masses of all the atoms in a molecule as defined on the periodic table.

For sodium acetate, NaC2H3O2, the molar mass is computed by adding the atomic masses of sodium (Na), carbon (C), hydrogen (H), and oxygen (O). With the molar mass known, it converts moles of a substance to grams—vital for real-world applications, such as creating a specific concentration of a solution, where weighing a precise mass of a substance is required.
Moles of Solute
Moles of solute refer to the quantity of a solute expressed in moles. A mole is a unit in chemistry representing Avogadro's number (approximately 6.022 x 10^23) of particles, atoms, ions, or molecules. The concept of moles is central for a chemist, allowing them to consider vast numbers of molecules in practical, weighable amounts.

When preparing a solution, knowing the moles of solute is essential because it determines the concentration of the solution, often expressed as molarity. The molarity is the number of moles per liter of solution, which demonstrates why understanding and calculating moles of solute is a foundational skill in chemistry.
Aqueous Solution Preparation
Preparing an aqueous solution involves dissolving a certain amount of solute in water to achieve a desired volume and concentration. Molarity, denoted as M, plays a crucial role since it represents the concentration of the solution, defined as moles of solute per liter of solution. To prepare an aqueous solution of a desired molarity, one must:
  • Calculate the moles of solute needed based on the desired molarity and the volume of solution.
  • Determine the mass of solute required by using the molar mass of the compound.
  • Measure the precise amount of solute and dissolve it in a volume of water to obtain the required concentration.
Accurate measurements and calculations are imperative to achieve the correct concentration, especially in scientific experiments, industrial applications, and medical formulations.

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Most popular questions from this chapter

\(1.4\) moles of phosphorus trichloride are present in a sample. How many atoms are there in the sample? (a) \(5.6\) (b) 34 (c) \(2.4 \times 10^{23}\) (d) \(3.372 \times 10^{24}\)

How many moles of oxygen gas can be produced during electrolytic decomposition of \(180 \mathrm{~g}\) of \(\begin{array}{ll}\text { Water? } & \text { (b) } 5 \text { moles }\end{array}\) (a) \(2.5\) moles (c) 10 moles (d) 7 moles

How many seconds are there in 3 days? (a) \(259200 \mathrm{~s}\) (b) \(172800 \mathrm{~s}\) (c) \(24800 \mathrm{~s}\) (d) \(72000 \mathrm{~s}\)

A mixture having 2 g of hydrogen and \(32 \mathrm{~g}\) of oxygen occupies how much volume at NTP? (a) \(44.8 \mathrm{~L}\) (b) \(22.4 \mathrm{~L}\) (c) \(11.2 \mathrm{~L}\) (d) \(67.2 \mathrm{~L}\)

The final molarity of a solution made by mixing \(50 \mathrm{~mL}\) of \(0.5 \mathrm{M} \mathrm{HCl}, 150 \mathrm{~mL}\) of \(0.25 \mathrm{M} \mathrm{HCl}\) and water to make the volume \(250 \mathrm{~mL}\) is (a) \(0.5 \mathrm{M}\) (b) \(1 \mathrm{M}\) (c) \(0.75 \mathrm{M}\) (d) \(0.25 \mathrm{M}\)
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