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Sodium chloride dissolving in water

Water is a very poor conductor of electricity. Yet when sodium chloride dissolves in water, the solution conducts readily. The dissolved sodium chloride must be responsible. How does the dissolved salt permit charge to move through the liquid One possibility is that when salt dissolves in water, particles with electric charge are produced. The movement of these charged particles through the solution accounts for the current. Salt has the formula, NaCl—for every sodium atom there is one chlorine atom. Chemists have... [Pg.78]

With these symbols, we can write the equation for the reaction that occurs when sodium chloride dissolves in water... [Pg.78]

In Chapter 6 we saw that the chemistry of sodium can be understood in terms of the special stability of the inert gas electron population of neon. An electron can be pulled away from a sodium atom relatively easily to form a sodium ion, Na+. Chlorine, on the other hand, readily accepts an electron to form chloride ion, Cl-, achieving the inert gas population of argon. When sodium and chlorine react, the product, sodium chloride, is an ionic solid, made up of Na+ ions and Cl- ions packed in a regular lattice. Sodium chloride dissolves in water to give Na+(aq) and C (aq) ions. Sodium chloride is an electrolyte it forms a conducting solution in water. [Pg.169]

Sodium chloride dissolves in water Ion-dipole forces of attraction between water molecules and ions are sufficient to overcome the forces between oppositely charged ions in the solid lattice. [Pg.13]

In contrast to sugar, solid sodium chloride dissolves in water to give a liquid that conducts electricity. Figure 3-19 shows that a solution of NaCl is a good conductor. When an ionic compound dissolves in water, its component cations and anions are free to move about in the solution. Mixing leads to a uniform distribution of Na and Cl ions through the entire solution, with each ion surrounded by a sheath of water molecules as shown in Figure 3-20. [Pg.173]

A solution consists of a solute dissolved in a solvent- The solute is recoverable from the solution, e.g. sodium chloride dissolved in water is... [Pg.1]

This is a good time to bring in a concept that you probably have not encountered before activity. Activity is the effective concentration of a solute, and activity is always less than molality. You need to become increasingly concerned about the difference between molality and activity when the concentration rises above 0.1 molal, especially if you are dealing with ionic solutes. In the previous example, we assumed that sodium chloride dissolves in water to give completely separated ions that have no interactions with each other. Is this reasonable ... [Pg.207]

Sodium chloride dissolves in water, a very polar solvent. Although the interactions between the water molecules and the sodium and chloride ions are not as strong as the interactions between the ions themselves, they are potent enough to make the process only somewhat endothermic. Entropy then makes the overall process favorable. Sodium chloride does not dissolve in a nonpolar solvent such as pentane (CH3CH2CH2CH2CH3) because the interactions between the pentane molecules and the ions are too weak in comparison to the forces between the ions, making the overall process too endothermic for entropy to overcome. [Pg.49]

Ionization of an alkyl halide requires formation and separation of positive and negative charges, similar to what happens when sodium chloride dissolves in water. Therefore, SN1 reactions require highly polar solvents that strongly solvate ions. One measure of a solvent s ability to solvate ions is its dielectric constant (e), a measure of the solvent s polarity. Table 6-6 lists the dielectric constants of some common solvents and the relative ionization rates for fm-butyl chloride in these solvents. Note that ionization occurs much faster in highly polar solvents such as water and alcohols. Although most alkyl halides are not soluble in water, they often dissolve in highly polar mixtures of acetone and alcohols with water. [Pg.250]

When a molecule splits apart, such as when salt, sodium chloride, dissolves in water to form the separate ions of Na+ and CP. This is also called ionization. [Pg.243]

When sodium chloride dissolves in water, the H2O molecules orient their dipoles around the Na and Cl ions so that their oppositely charged ends are adjacent to each ion (Figure 15.1). Each sodium or chloride ion in solution is sur-ronnded by many water molecules, lessening the attractions between the ions. Silver chloride, AgCl, does not dissolve in water. Evidently, the ion-dipole attractions are not sufficient to overcome the ion-ion attractions of this solid lattice. The nonpolar solvent benzene, CgHg, cannot dissolve either of these ionic compounds. [Pg.419]

We can also use vapor pressure measurements to characterize solutions. For example, 1 mole of sodium chloride dissolved in water lowers the vapor pressure about twice as much as expected because the ions separate when it dissolves. Thus vapor pressure measurements can give valuable information about the nature of the solute after it dissolves. We will discuss this in more detail in Section 17.7. [Pg.842]

The method for making sodium hydroxide is called the chlor-alkali process. The name comes from the fact that both chlorine and an alkali metal (sodium) are produced at the same time. In this case, an electric current is passed through a solution of sodium chloride dissolved in water ... [Pg.549]

Also notice that the entropy increases when 1 mol of sodium chloride dissolves in water to form 1 mol of aqueous sodium ions and 1 mol of aqueous chlorine ions. [Pg.377]

Sodium chloride and liquid water are pure substances each with a degree of orderliness. When sodium chloride dissolves in water, the entropy of the system increases because Na+ and Cl ions and water molecules mix together to create a large number of random arrangements. [Pg.516]

When sodium chloride dissolves in water, it produces sodium and chloride ions. H 0... [Pg.31]

What s going on in such a situation Your model of water and its interactions explains why salt and many other ionic compormds dissolve in water and why the solutions conduct electricity. Remember that ionic solids are composed of a three-dimensional network of positive and negative ions, which form strong ionic bonds. Look at Figure 13.15 to see how a crystal of sodium chloride dissolves in water. [Pg.451]

Sodium Chloride Dissolving in Water This shows the mixture immediately after sodium chloride has been added to water. Certain water molecules are highlighted to draw attention to their role in the process. [Pg.135]

The rules given in Table 4.2 (p. 113) allow us to predict the solubility of a particular ionic compound in water. When sodium chloride dissolves in water, the ions are stabilized in solution by hydration, which involves ion-dipole interaction. In general, we predict that ionic compounds should be much more soluble in polar solvents, such as water, liquid ammonia, and liquid hydrogen fluoride, than in nonpolar solvents, such as benzene and carbon tetrachloride. Since the molecules of nonpolar solvents lack a dipole moment, they cannot effectively solvate the Na and Cl ions. Solvation is the process in which an ion or a molecule is surrounded by solvent molecules arranged in a specific manner. The process is called hydration when the solvent is water.) The predominant intermolecular interaction between ions and nonpolar compounds is ion-induced dipole interaction, which is much weaker than ion-dipole interaction. Consequently, ionic compounds usually have extremely low solubility in nonpolar solvents. [Pg.470]

EXAMPLE 8 Calculate the mass of sodium produced from electrolysis of 10.0 g of sodium chloride dissolved in water by passage of 1.00 A for 40.0 minutes. [Pg.136]

Recall that solutions of electrolytes are formed from solutes that are soluble ionic compounds. These compounds dissociate in solution to produce ions that behave as charge carriers. Solutions of electrolytes are good conductors of electricity. For example, sodium chloride dissolving in water ... [Pg.178]

This behavior arises from the different natures of the components in these two solids. Common salt, NaCl, is an ionic solid that contains Na and Cl ions. When solid sodium chloride dissolves in water, sodium ions and chloride ions are distributed throughout the resulting solution. These ions are free to move through the solution to conduct an electric current. Table sugar (sucrose), on the other hand, is composed of neutral molecules that are dispersed throughout the water when the solid dissolves. No ions are present, and the resulting solution does not conduct electricity. These examples illustrate two important types of crystalline solids ionic solids, represented by sodium chloride and molecular solids, represented by sucrose. [Pg.504]

We saw in Chapter 8 that when sodium chloride dissolves in water, the resulting solution conducts an electric current. This convinces us that the solution contains ions that can move (this is how the electric current is conducted). The dissolving of solid sodium chloride in water is shown below. [Pg.521]

Figure 14.10 Sodium chloride dissolves in water as the water molecules surround the sodium and chloride ions. Note how the polar water molecules orient themselves differently around the positive and negative ions. [Pg.490]

Problem 7.6. Will sodium chloride dissolve in water ... [Pg.132]


See other pages where Sodium chloride dissolving in water is mentioned: [Pg.78]    [Pg.79]    [Pg.191]    [Pg.50]    [Pg.70]    [Pg.160]    [Pg.182]    [Pg.11]    [Pg.71]    [Pg.55]    [Pg.110]    [Pg.111]    [Pg.35]    [Pg.414]    [Pg.459]    [Pg.476]    [Pg.65]    [Pg.60]   
See also in sourсe #XX -- [ Pg.9 , Pg.12 , Pg.124 , Pg.126 , Pg.480 , Pg.481 , Pg.484 ]

See also in sourсe #XX -- [ Pg.533 ]




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