Sodium chloride calculating mass

If 10.0 g of sodium and 20.0 g of chlorine are mixed, they react to form 25.4 g of sodium chloride. Calculate the mass of chlorine that does not react. 

The total volume of seawater is 1.5 X 10 L. Assume that seawater contains 3.1 percent sodium chloride by mass and that its density is 1.03 g/mL. Calculate the total mass of sodium chloride in kilograms and in tons. (1 ton = 2000 lb 1 lb = 453.6 g)... 

Using Parts by Mass (or Parts by Volume) in Calculations We can use the parts by mass (or parts by volume) concentration of a solution as a conversion factor between mass (or volume) of the solute and mass (or volume) of the solution. For example, for a solution containing 3.5% sodium chloride by mass, we write the following conversion factor ... 

PRACTICE EXAMPLE B A particular sample of seawater has a density of 1.027 g/cm at 10 °C and is 2.67% sodium chloride by mass. Given that sodium chloride is 39.34% sodium by mass and that the mass of a single sodium atom is 3.817 X 10"36 Lg, calculate the maximum mass of sodium and the maximum number of sodium atoms that can be extracted from a 1.5 L sample of this seawater. 

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. 

A solution is prepared by dissolving 10.0 g of table salt (sodium chloride), and 15.0 g of cane sugar (sucrose) in 500.0 g of water. Calculate the mass percent of the table salt in the solution. 

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. 

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 ... 

The objective of the mass transport lab is to explore the effect of controlled hydrodynamics on the rate at which a mass transport controlled electrochemical reaction occurs on a steel electrode in aqueous sodium chloride solution. The experimental results will be compared to those predicted from the Levich equation. The system chosen for this experiment is the cathodic reduction of oxygen at a steel electrode in neutral 0.6 M NaCl solution. The diffusion-limited cathodic current density will be calculated at various rotating disk electrode rotation rates and compared to the cathodic polarization curve generated at the same rotation rate. 

Often impure reactants are the cause of a percentage yield of less than 100%. Impurities cause the mass data to be incorrect. For example, suppose that you have 1.00 g of sodium chloride and you want to carry out a reaction with it. You think that the sodium chloride may have absorbed some water, so you do not know exactly how much pure sodium chloride you have. If you calculate a theoretical yield for your reaction based on... 

When electrolyte solutions are subjected to such measurements, abnormal results are obtained. When substances like sodium chloride or magnesium sulphate are examined, the depression of freezing point or the elevation of boiling point is about twice that calculated from the relative molecular mass, with calcium chloride or sodium sulphate these quantities are three times those expected. Keeping in mind what has been said above, we can say that the number of particles in the solution of sodium chloride or magnesium sulphate is twice the number of molecules present, while in the case of calcium chloride or sodium sulphate there are three particles present for each molecule. 

Calculate the density of a 25.0% by mass sodium chloride solution in water if 253 g of sodium chloride is used to make 850 mL of the solution. 

The density of a solution 25.0% by mass sodium chloride (table salt) in water is 1.19 g/mL. Calculate the mass of sodium chloride in 842 mL of the solution. 

Electrolysis of concentrated aqueous sodium chloride solution (called brine) yields aqueous sodium hydroxide, hydrogen gas, and chlorine gas— three important industrial chemicals. Calculate the mass of chlorine that can be produced by electrolysis of 50.0 kg of sodium chloride in concentrated aqueous solution ... 

Practice Problem 10.7 The industrial process for the production of sodium metal and chlorine gas involves electrolysis of molten (melted) sodium chloride (in the absence of water). Calculate the mass of sodium that can be prepared by electrolysis of 207 kg of sodium chloride. The balanced equation is... 

EXAMPLE 3.1. Calculate the mass of sodium chloride formed by the complete reaction of 10.0 g of sodium with 15.4 g of chlorine. What law allows this calculation ... 

A sample of a mixture containing only sodium chloride and potassium chloride has a mass of 4.000 g. When this sample is dissolved in water and excess silver nitrate is added, a white precipitate (silver chloride) forms. After filtration and drying, this precipitate has the mass 8.5904 g. Calculate the mass percent of each mixture component. 

At elevated temperatures, sodium chlorate decomposes to produce sodium chloride and oxygen gas. A 0.8765-g sample of impure sodium chlorate was heated until the production of oxygen gas ceased. The oxygen gas collected over water occupied 57.2 mL at a temperature of 22° and a pressure of 734 torr. Calculate the mass percent ... 

Calculate the mass of either sodium chloride or sodium carbonate required to maKe up the solution ... 

Sodium benzoate, the sodium salt of benzoic acid, is used as a food preservative. A sample containing solid sodium benzoate mixed with sodium chloride is dissolved in 50.0 mL of 0.500 M HCl, giving an acidic solution (benzoic acid mixed with HCl). This mixture is then titrated with 0.393 M NaOH. After the addition of 46.50 mL of the NaOH solution, the pH is found to be 8.2. At this point, the addition of one more drop (0.02 mL) of NaOH raises the pH to 9.3. Calculate the mass of sodium benzoate (NaC H5COO) in the original sample. (Hint At the equivalence point, the total number of moles of acid [here HCl] equals the total number of moles of base [here, both NaOH and NaCgH5COO].)... 

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. 

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. 

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. 

Consider an aqueous solution containing sodium chloride that has a density of 1.01 g/mL. Assume the solution behaves ideally. The freezing point of this solution at 1.0 atm is -1.28X. Calculate the percent composition of this solution (by mass). 

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