5 Acid can dissociate in solution, which characterized by dissociation constant (Ka).Polyprotic acids can dissociate multiple times, which associated by multipledissociation constant (Kal, Ka2, Ka3 etc.)CO2 dissolve in water forms carbonic acid H2CO3CO2 (aq) = H2CO3 (aq)K-1.7x10-H2CO3 (aq)= HCO3+H (aq)Kal-2.5x104(aq)HCO3 (aq) = CO3 (aq) + H" (ag)Ka2- 5.0x10 ||(a) For soda water, the CO2 concentration is 6g/L and the pH is 4. Calculate theequilibrium molar concentration of HCO3 and CO32-(b) It is known that the CO2 concentration in air is 387ppm, and the CO2 Henryconstant KH= 29.4 atm/mol. The second dissociation is negligible.Calculate the pH of the pure water after equilibrium in airER WindowsBE R Windows-

(a) For soda water, the CO2 concentration is given to be 6 g/L.

Acid can dissociate in solution, which characterized by dissociation constant (Ka). Polyprotic acids can dissociate multiple times, which associated by multiple dissociation constant (Kal, Ka2, Ka3 etc.) CO2 dissolve in water forms carbonic acid H2CO3 CO2 (aq) = H2CO3 (aq) K-1.7x103 H2CO3 (aq) = HCO3 (aq) +H'(aq) Kal-2.5x104 HCO3 (aq) = CO3 (aq) + H Ka2 5.0x10-11 (aq) (a) For soda water, the CO2 concentration is 6g/L and the pH is 4. Calculate the equilibrium molar concentration of HCO; and CO32- (b) It is known that the CO2 concentration in air is 387ppm, and the CO2 Henry constant KH= 29.4 atm/mol. The second dissociation is negligible. Calculate the pH of the pure water after equilibrium in air 啟用

Acid can dissociate in solution, which characterized by dissociation constant (Ka). Polyprotic acids can dissociate multiple times, which associated by multiple dissociation constant (Kal, Ka2, Ka3 etc.) CO2 dissolve in water forms carbonic acid H2CO3 CO2 (aq) = H2CO3 (aq) K-1.7x103 H2CO3 (aq) = HCO3 (aq) +H'(aq) Kal-2.5x104 HCO3 (aq) = CO3 (aq) + H Ka2 5.0x10-11 (aq) (a) For soda water, the CO2 concentration is 6g/L and the pH is 4. Calculate the equilibrium molar concentration of HCO; and CO32- (b) It is known that the CO2 concentration in air is 387ppm, and the CO2 Henry constant KH= 29.4 atm/mol. The second dissociation is negligible. Calculate the pH of the pure water after equilibrium in air 啟用

Chemistry

10th Edition

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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Concept explainers

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.

Question

Acid can dissociate in solution, which characterized by dissociation constant (Ka).
Polyprotic acids can dissociate multiple times, which associated by multiple
dissociation constant (Kal, Ka2, Ka3 etc.)
CO2 dissolve in water forms carbonic acid H2CO3
CO2 (aq) = H2CO3 (aq)
K-1.7x10-
H2CO3 (aq)
= HCO3
+H (aq)
Kal-2.5x104
(aq)
HCO3 (aq) = CO3 (aq) + H" (ag)
Ka2- 5.0x10 ||
(a) For soda water, the CO2 concentration is 6g/L and the pH is 4. Calculate the
equilibrium molar concentration of HCO3 and CO32-
(b) It is known that the CO2 concentration in air is 387ppm, and the CO2 Henry
constant KH= 29.4 atm/mol. The second dissociation is negligible.
Calculate the pH of the pure water after equilibrium in air
ER Windows
BE R Windows-

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