A pH 7.0 buffer solution is made using NaOH and phosphoric acid. The sum of the concentrations of all phosphoric acid species is 0.1 M. The equilibrium constant Kw for the ionization of water is 10-14 and K's for the following equilibria are given: H3PO4 H* + H2PO4 K1 = 7.1×10-3 H2PO4 2- H* + HPO4 K2 = 6.2x10 8 HPO,? H* + PO4 3- K3 = 4.5x10-13 Calculate the concentrations of all species in solution. Formulas: pH =-log10[H*], pK=-log,,K

A pH 7.0 buffer solution is made using NaOH and phosphoric acid. The sum of the concentrations of all phosphoric acid species is 0.1 M. The equilibrium constant Kw for the ionization of water is 10-14 and K's for the following equilibria are given: H3PO4 H* + H2PO4 K1 = 7.1×10-3 H2PO4 2- H* + HPO4 K2 = 6.2x10 8 HPO,? H* + PO4 3- K3 = 4.5x10-13 Calculate the concentrations of all species in solution. Formulas: pH =-log10[H*], pK=-log,,K

Chemistry

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ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

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A pH 7.0 buffer solution is made using NaOH and phosphoric acid. The sum of the
concentrations of all phosphoric acid species is 0.1 M. The equilibrium constant Kw for the
ionization of water is 10-14 and Ks for the following equilibria are given:
H3PO4
H* + H2PO4
K1 = 7.1×10-3
2-
H2PO4
H* + HPO4
K2 = 6.2x10-8
3-
НРОД
H* + PO4
K3 = 4.5×10-13
Calculate the concentrations of all species in solution.
Formulas:
pH=-log1o[H"], pK=-log1„K

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