Molarity of solutions

Equation 5 shows how the Gibbs free energy of reaction varies with the activities (the partial pressures of gases or molarities of solutes) of the reactants and products. The expression for Q has the same form as the expression for K, but the activities refer to any stage of the reaction. 

Pressures of gases and molarities of solutes in aqueous solution appear in thermodynamic equilibrium constant expressions. Pure solids and liquids (including solvents) do not appear. 

Calculations involving equivalents, milliequivalents, normalities, and volumes of solutions are made in just the same way as those involving molarities of solutions. The unique and useful feature about the use of equivalents is that, for any chemical reaction, when reactant A has just exactly consumed reactant B, we can say... 

Determination of the operational molarity of solutions of bovine O-chytnotrypsin, trypsin, thro mb to and factor Xa by spectre flu orometric titration. Biochem. J. 131 107 moth. 

This represents the total molarity of solute particles. But NaCl gives two ions per formula unit. Therefore, the concentration of NaCl needed is 0.315/2, or 0.158 M. That is,... 

W Weak Anionic Absorption I Moderate Anionic Absorption S Strong Anionic Absorption M Molarity of Solution... 

In this section, we describe two types of volumetric calculations. The first involves computing the molarity of solutions that have been standardized against either a primary-standard or another standard solution. The second involves calculating the amount of analyte in a sample from titration data. Both types are based on three algebraic relationships. Two of these are Equations 13-1 and 13-3, both of which are based on millimoles and milliliters. The third relationship is the stoichiometric ratio of the number of millimoles of the analyte to the number of millimoles of titrant. 

Stoichiometry concerns calculations based on balanced chemical equations, a topic that was presented in Chapter 8. Remember that the coefficients in the balanced equations indicate the number of moles of each reactant and product. Because many reactions take place in solution, and because the molarity of solutions relates to moles of solute and volumes, it is possible to extend stoichiometric calculations to reactions involving solutions of reactants and products. The calculations involving balanced equations are the same as those done in Chapter 8, but with the additional need to do some molarity calculations. Let s get our feet wet by working a couple of problems involving solutions in chemical reactions. 

Osmotic pressure = n = MSO UteRT Msoiute = Molarity of solute particles... 

M] = molarity of solution before dilution M2 = molarity of solution after dilution V] = volume of solution before dilution V2 = volume of solution after dilution... 

This represents the total molarity of solute particles. But NaCI gives two ions per formula... 

Molarity of solution made x Volume of solution made) is equal to (Molarity of the stock solution X Volume of the stock solution required). With this in mind, let s plug in the values that we know. 

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