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CH 110 Lecture Notes - Lecture 5: Aqueous Solution, Strong Electrolyte, Hydrochloric Acid

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coralbear227
6 Jan 2017
School
University of Hartford
Department
Chemistry - A&S
Course
CH 110
Professor
Krause Tatum

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Document Summary

Aqueous solution- a solution in which water is the dissolving medium. Most reactions you will encounter take place in water. A solution is a homogeneous mixture of two or more substances. Solutions can be quantitatively be described by their concentration. The concentration of a solute in solution is expressed in terms of molarity (m) M= moles solute/ volume of solution in liters. A solution containing 1. 20 mol of substance [a] in 2. 50 l of solution would have a molarity (m) equal to: If we know any two of the 3 quantities we can calculate the third: A dilution occurs when a solution of known molarity is diluted with more solvent. Key to remember: when a solvent is added to a solution, the number of moles of solute does not change. When a solvent is added to a solution, the number of moles of solute remains unchanged.

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Related Questions

A titration is a procedure for determining the concentration of a solution by allowing it to react with another solution of known concentration (called a standard solution). Acid-base reactions and oxidation-reduction reactions are used in titrations. For example, to find the concentration of an HCl solution (an acid), a standard solution of NaOH (a base) is added to a measured volume of HCl from a calibrated tube called a buret. An indicator is also present and it will change color when all the acid has reacted. Using the concentration of the standard solution and the volume dispensed, we can calculate molarity of the HCl solution.



A) A volume of 90.0 mL of aqueous potassium hydroxide (KOH) was titrated against a standard solution of sulfuric acid (H2SO4). What was the molarity of the KOH solution if 14.7 mL of 1.50 M H2SO4 was needed? The equation is 2KOH(aq)+H2SO4(aq)→K2SO4(aq)+2H2O(l)

B) Redox titrations are used to determine the amounts of oxidizing and reducing agents in solution. For example, a solution of hydrogen peroxide, H2O2, can be titrated against a solution of potassium permanganate, KMnO4. The following equation represents the reaction:

2KMnO4(aq)+H2O2(aq)+3H2SO4(aq)→3O2(g)+2MnSO4(aq)+K2SO4(aq)+4H2O(l)

A certain amount of hydrogen peroxide was dissolved in 100. mL of water and then titrated with 1.68 M KMnO4. What mass of H2O2 was dissolved if the titration required 18.8 mL of the KMnO4 solution?

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