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Chapter 1: Problem 99

You are given a mixture of sand, salt (sodium chloride), and naphthalene, a white solid that is not soluble in water. Write a detailed description of a procedure that would completely separate each component from this mixture.

Short Answer

Expert verified
Dissolve salt in water, filter to remove sand, evaporate to get salt, and sublime to separate naphthalene.

Step by step solution

01

Dissolution of Salt in Water

Begin by adding the mixture to a beaker containing warm water. Stir the mixture well to ensure that the salt (sodium chloride) dissolves completely in the water. The sand and naphthalene will not dissolve because sand is insoluble, and naphthalene is not soluble in water.
02

Filtration to Separate Sand

Pour the mixture through a filter paper that is placed in a funnel. The sand particles will be retained on the filter paper, while the salt solution (salt dissolved in water) and naphthalene will pass through. Collect the sand and allow it to dry.
03

Evaporation of Water

Heat the salt solution to evaporate the water. This process will leave behind the dissolved salt. Continue heating until all the water has evaporated, ensuring that only salt remains.
04

Sublimation of Naphthalene

Place the remaining mixture (naphthalene and salt, after water removal) in a sublimation apparatus. Heat the mixture gently 鈥� naphthalene, which sublimes at a relatively low temperature, will transform directly from solid to gas. Cool the vapor to condense it back into a solid, collecting the pure naphthalene.
05

Collect and Verify Each Component

After sublimation, ensure that you have collected all three components separately: dry sand from the filtration, dry salt from the evaporation, and solid naphthalene from sublimation.

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Key Concepts

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

Dissolution
Dissolution is the process of a solid, liquid, or gas becoming incorporated into a liquid to form a solution. In the context of our mixture, we are primarily focused on dissolving the salt, which is soluble in water. By adding warm water to the mixture containing sand, salt, and naphthalene, only the salt dissolves because it is the only component that is water-soluble. Stirring helps facilitate this process by increasing the interaction between the water molecules and salt, speeding up the dissolution. As a result, sand and naphthalene remain in their solid forms while salt forms a homogeneous saline solution.
Filtration
Filtration is a mechanical or physical process used to separate solid particles from a liquid. After dissolving the salt in water, the next task is to separate the insoluble sand. This is accomplished with the help of filter paper placed inside a funnel. When our mixture is poured onto the filter paper, only the liquid part, the salt solution, passes through, while the sand is left behind on the filter. This separation works because filter paper has tiny pores that allow liquid to pass but trap larger solid particles. As a result, we achieve the successful separation of sand from the salt solution and naphthalene.
Evaporation
Evaporation is the process of turning a liquid into vapor and is used to separate a dissolved solid from a solution. Once you have your filtered salt solution, heating it causes the water to evaporate, leaving the salt behind. During heating, the liquid phase (water) transitions into a gaseous form, gradually leaving behind the solid salt. Continue to apply heat until all the water has evaporated. What remains is dry salt, free from the liquid, effectively separating it from the initial solution.
Sublimation
Sublimation is a process where a solid changes directly into a gas without passing through the liquid phase. This property is unique to certain substances, such as naphthalene. After removing the water and leaving the salt behind from the previous step, you are left with naphthalene mixed with salt. Using sublimation, naphthalene is gently heated in a sublimation apparatus to transform it into vapor, skipping the liquid phase entirely. The vapor is allowed to cool and change back into a solid, free from salt. This enables the recovery of pure naphthalene, completing the separation of all mixture components.

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Most popular questions from this chapter

The element zinc reacts with the element sulfur to form a white solid compound, zinc sulfide. When a sample of zinc that weighs \(65.4 \mathrm{~g}\) reacts with sulfur, it is found that the zinc sulfide produced weighs exactly \(97.5 \mathrm{~g}\). (a) Calculate the mass of sulfur in the zinc sulfide. (b) Calculate the mass of zinc sulfide that could be produced from \(20.0 \mathrm{~g}\) zinc.

Write a chemical formula for each substance, and draw a picture of how the nanoscale particles are arranged at room temperature. (a) Water, a liquid whose molecules contain two hydrogen atoms and one oxygen atom each (b) Nitrogen, a gas that consists of diatomic molecules

When volumes of liquids are mixed, the resulting volume is not always equal to the sum of the volume of each liquid. For example, when \(50.0 \mathrm{~mL}\) of ethanol \((\mathrm{d}=\) \(0.789 \mathrm{~g} / \mathrm{mL}\) ) is mixed with \(50.0 \mathrm{~mL}\) of water \((0.998 \mathrm{~g} / \mathrm{mL})\) at \(25^{\circ} \mathrm{C}\), the resulting volume is only \(95.6 \mathrm{~mL}\). Calculate the density of the solution.

When \(12.6 \mathrm{~g}\) calcium carbonate (the principal component of chalk) is treated with \(63.0 \mathrm{~mL}\) hydrochloric acid (muriatic acid sold in hardware stores; density \(=1.096 \mathrm{~g} / \mathrm{mL}\) ), the calcium carbonate reacts with the acid, goes into solution, and carbon dioxide gas bubbles out of the solution. After all of the carbon dioxide has escaped, the solution weighs \(76.1 \mathrm{~g} .\) Calculate the volume (in liters) of carbon dioxide gas that was produced. (The density of the carbon dioxide gas is \(1.798 \mathrm{~g} / \mathrm{L}\).)

These temperatures are measured at various locations during the same day in the winter in North America: \(-10^{\circ} \mathrm{C}\) at Montreal, \(28^{\circ} \mathrm{F}\) at Chicago, \(20^{\circ} \mathrm{C}\) at Charlotte, and \(40^{\circ} \mathrm{F}\) at Philadelphia. Which city is the warmest? Which city is the coldest?
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