Stoichiometry of Reactions in Aqueous Solutions Titrations

A newspaper account of an accidental spill of hydrochloric acid in an area where sodium hydroxide solution was also stored spoke of the potential hazardous release of chlorine gas if the two solutions should come into contact. Was this an accurate accounting of the hazard involved Explain. 

A solution of one reactant is placed in a small beaker or flask. Another reactant, also in solution and commonly referred to as titrant, is in a buret, a long, graduated tube equipped with a stopcock valve. The second solution is slowly added to the first by manipulating the stopcock. In a titration, a reaction is carried out by the carefully controlled addition of one solution to another. The trick is to stop the titration at the point where both reactants have reacted completely, a condition called the equivalence point of the 

Standardizing a solution of an oxidizing agent through a redox titration—Example 5-10 illustrated 

EXAMPLE 5-9 Using Titration Data to Establish the Concentrations of Acids and Bases 

Vinegar is a dilute aqueous solution of acetic add produced by the bacterial fermentation of apple cider, wine, or other carbohydrate material. The legal rniiiimiim acetic acid content of vinegar is 4% by mass. A 5.00 mL sample of a particular vinegar is titrated with 38.08 mL of 0.1000 M NaOH. Does this sample exceed the minimum limit (Vinegar has a density of about 1.01 g/mL.) 

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Distinguish between an electrolyte and a nonelectrolyte, and provide examples of each. 5.2 Use the solubility guidelines tor common ionic solids to determine whether 5-4 Oxidation-Reduction Reactions Some General Principles 5-7 Stoichiometry of Reactions in Aqueous Solutions Titrations... 

Stoichiometry of Reactions in Aqueous Solutions Titrations— A common laboratory technique applicable to precipitation, acid-base, and redox reactions is titration. The key point in a titration is the equivalence point, which can be observed with the aid of an indicator. Titration data can be used to establish a solution s molarity, called standardization of a solution, or to provide other information about the compositions of samples being analyzed. 

Now that we have discussed the concentration and dilution of solutions, we can examine the quantitative aspects of reactions in aqueous solution, or solution stoichiometry. Sections 4.6. 8 focus on two techniques for studying solution stoichiometry gravimetric analysis and titration. These techniques are important tools of quantitative analysis, which is the determination of the amount or concentration of a substance in a sample. 

Calculating The concentration of thallium(I) ions in solution may be determined by oxidizing to thallium(III) ions with an aqueous solution of potassium permanganate (KMn04) under acidic conditions. Suppose that a 100.00 mL sample of a solution of unknown T1+ concentration is titrated to the endpoint with 28.23 mL of a 0.0560M solution of potassium permanganate. What is the concentration of T1+ ions in the sample You must first balance the redox equation for the reaction to determine its stoichiometry. 

Certain aqueous reactions are useful for determining how much of a particular substance is present in a sample. For example, if we want to know the concentration of lead in a sample of water, or if we need to know the concentration of an acid, knowledge of precipitation reactions, acid-base reactions, and solution stoichiometry will be useful. Two common types of such quantitative analyses are gravimetric analysis and acid-base titration. 

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