Sodium chloride molar mass

Sodium chloride has a relative molecular mass of 58.44. A 0.1000M solution is prepared by weighing out 2.922 g of the pure dry salt (see Section 10.74) and dissolving it in 500 mL of water in a graduated flask. Alternatively about 2.9 g of the pure salt is accurately weighed out, dissolved in 500 mL of water in a graduated flask and the molar concentration calculated from the weight of sodium chloride employed. 

Molar mass is important when we need to know the number of atoms in a sample. It would be impossible to count out 6 X ID23 atoms of an element, but it is very easy to measure out a mass equal to the molar mass of the element in grams. Each of the samples shown in Fig. E.2 was obtained in this way each sample contains the same number of atoms of the element (6.022 X 1023), but the masses vary because the masses of the atoms are different (Fig. E.4). The same rule applies to compounds. Flence, if we measure out 58.44 g of sodium chloride, we obtain a sample that contains 1.000 mol NaCl formula units (Fig. E.5). 

Fig. 1. Capsule permeability as measured by the inverse GPC method. Capsules were made from 1.25% A-carrageenan (Fluka) and 0.02% carboxymethylcellulose (Aqualon) in 0.9% sodium chloride (core polymers) and 2% polydimethylamine-co-epichlorohydrin modified, quater-nized (Scientific Polymer Products) and a quaternary amine (Agefloc B50, CPS) in PBS (receiving bath) using a 3 min reaction time. The capsules were subsequently washed with PBS, coated for 15 min with 0.1% LV alginate (Kelco) and again washed in PBS. Two molecular size dex-trans were used to probe the capsule permeability. 170 kD dextran is almost totally excluded while the lower molar mass polymers permeated the membrane to varying extents...

For sodium chloride (relative atomic masses Na = 23.0, Cl = 35.5), the molar mass = 58.5 g mob1 therefore ... 

BB 0.10 m. This problem gives you the value of your solute (sodium chloride) in grams and the value of your solvent (water) in liters. You must first convert the sodium chloride to moles. To do so, divide by the molar mass (which we discuss in Chapter 7) ... 

A simple calculation reveals the limits of the numbers of water molecules that may be associated with an ion in a standard solution. A l mol dm-3 aqueous solution of sodium chloride has a density of 1038 kg m-3 at 25 °C, so 1 dm3 of such a solution has a mass of 1038 g. One mole of the salt has a mass of 58.44 g, so the water in the litre of solution has a mass of 1038-58.44 = 979.56 g. This amount of water contains 979.56/18.015 = 54.4 moles of the liquid. The molar ratio of water molecules to ions in the 1 mol dm-3 aqueous solution of Na h(aq) and Cl (aq) ions is therefore 54.4/2 = 27.2, assuming that the water molecules are shared equally between the cations and anions. This represents the theoretical upper limit of hydration of any one ion in a standard solution of 1 mol dm-3 concentration. The limit may be exceeded in more dilute solutions, but that depends upon the operation of forces over a relatively long range. Certainly, in more concentrated solutions, the limits of hydration of ions become more restricted as fewer water molecules are available to share out between the cation and anion assembly. 

CHEMICAL NAME = sodium chloride CAS NUMBER = 7647-14-5 MOLECULAR FORMULA = NaCl MOLAR MASS = 58.4 g/mol COMPOSITION = Na(39.3°/o) Cl(69.7°/o)... 

To calculate the molality of a solution prepared by dissolving 10.5 g of sodium chloride in 250 g of water, we convert the mass of sodium chloride to moles of NaCl (by dividing the mass by the molar mass) and divide it by the mass of water in kilograms ... 

Many common substances are ionic, e.g., sodium chloride, NaCl. A crystal of NaCl contains sodium ions, Na +, and chloride ions, CT, arranged in a regular spatial array. Although there are no NaCl molecules, the formula indicates the relative number of atoms of each element present in the crystal, and we can speak of the molar mass of NaCl, 22.98977 + 35.4527 = 58.4425 g/mol, as the mass of sodium chloride which contains NA... 

If you were to add 50.0 g of sodium chloride, an electrolyte (NaCl, molar mass 58.44 g), to enough water to make 1.00 L of solution, what would be the osmotic pressure of the solution at 22°C ... 

Step 1 To find the amount (in mol) of sodium chloride, first determine its molar mass. Then divide the amount of sodium chloride (in g) by its molar mass (in g/mol). 

Fig. 2 shows MALDI-MS spectra of the same three samples.The spectra usually show the mole peaks plus the molar mass of Na (23 Da) and K (39 Da). Unless they have been specifically added, the sodium and potassium ions come fi-om contaminants in the specimen and/or the matrix. Alternatively, another suitable salt may be added. The addition of lithium chloride suppresses sodium (and potassium) ions, so that the spectra can be more easily interpreted. Thus, the numbers in Fig. 2a refer to mole peaks M plus a (= M + 23 Da) and in Fig. 2b and 2c to M plus Li (= M + 7 Da). As can be seen, the resolution in the higher molecular mass range is more pronounced than in SFC. Components with more than 100 monomer units can be separated in the diol sample. 

Some substances exist as a collection of ions rather than as separate mol- ecules. An example is ordinary table salt, sodium chloride (NaCl), which is composed of an array of Na+ and Cl- ions. There are no NaCl molecules present. However, in this text, for convenience, we will apply the term molar mass to both ionic and molecular substances. Thus we will refer to 58.44 (22.99 + 35.45) as the molar mass for NaCl. In some texts the term formula weight is used for ionic compounds instead of the terms molar mass or molecular weight. ... 

Suppose 150 mL of a 10.00% by mass solution of sodium chloride (density = 1.0726 g cm ) is acidified with sulfuric acid and then treated with an excess of Mn02(s). Under these conditions, all the chlorine is liberated as Cl2(g). The chlorine is collected without loss and reacts with excess H2(g) to form HCl(g). The HCl(g) is dissolved in enough water to make 250 mL of solution. Compute the molarity of this solution. 

A. Solution A, because sodium fluoride has a lower molar mass than potassium chloride. 

If the sucrose solution in the aforementioned membrane sac were replaced with a sodium chloride solution of the same molarity, the solution in the manometer would reach equilibrium at a point almost twice as high as that observed with sucrose because sodium chloride dissociates into two ions per molecule. If ion activity is unrestricted, the sodium chloride solution would have twice as many osmoticaUy active particles (osmoles) for the same molecular concentration as the sucrose solution. In reality, the number of active particles is less than this (0.93 for NaCl), as explained later in this chapter. The total number of individual (solute) particles present in a solution per given mass of solvent, regardless of their molecular nature (i.e., nonelectrolyte, ion, or coUoid), determines the total osmotic pressure of the solution. In blood plasma, for example, nonelectrolytes such as glucose and urea and even proteins contribute to the osmotic pressure of this body fluid. 

Standard acid or base solutions can also be prepared with ion-exchange resins. Here, a solution containing a known mass of a pure compound, such as sodium chloride, is washed through the resin column and diluted to a known volume. The salt liberates an equivalent eunount of acid or base from the resin, permitting calculation of the molarity of the reagent in a straightforward way. 

To calculate the molar mass for sodium chloride, we must realize that 1 mol of NaCl contains 1 mol of Na ions and 1 mol of Cl ions. 

Therefore, the molar mass (in grams) for sodium chloride represents the sum of the mass of 1 mol of sodium ions and the mass of 1 mol of chloride ions. 

The molar mass of a compound demonstrates the law of conservation of mass the total mass of the reactants that reacted equals the mass of the compound formed. Figure 10.10 shows equivalent masses of one mole of potassium chromate, sodium chloride, and sucrose. 

The molar mass of NaCl is 58.44 g. It represents the mass of 1 mole of sodium chloride. 

Carboxylic, hydroxyl, adipoyl chloride, and sodium adipate end-groups of the high molar mass poly(butylene adipate) (PBA), S5mthesized by polycondensation of an equimolar mixture of adipoyl chloride and 1,4-butanediol, were characterized by MALDI-TOF. Narrow dispersed fractions with low molar masses (<6000 Da) were collected by SEC fractionation, prior to MALDI analysis. ° ... 

This process is cheaper than the transesterification and leads to higher molar masses. But it is difficult to remove the sodium chloride also formed from the product, by, for example, extrusion volatilization. The Schotten-Baumann reaction is carried out either in organic solvents (aromatics, chlorohydro-carbons) with addition of acceptors (pyridine, /-amines) or in aqueous alkali under addition of water-insoluble organic compounds otherwise high molar masses are not obtained. 

Rubidium iodide crystallizes with the same structure as sodium chloride, (a) How many iodide ions are there per unit cell (b) How many rubidium ions are there per unit cell (c) Use the ionic radii and molar masses of Rb (1.66 A, 85.47 g/mol) and 1 (2.06 A, 126.90 g/mol) to estimate the density of rubidium iodide in g/cm. ... 

The term a is the linear coefficient for the effect of concentration on the osmotic pressure in mass frac units. Osmotic pressures are given for aqueous sodium chloride solutions in Perry and Green, 6th edition (1984, p. 16-23). At 25°C and 0.001 mole frac the osmotic pressure is 0.05 atm. Thus, in molar units a = 0.05 atm/0.001 mole frac = 50 atm/mole frac. 

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