Salts of carbonate ion behave as a weak base, undergoing hydrolysis in water according to the equation: CO3²- + H₂O HCO3 + OH K for carbonate ion = 0.00018. Calculate the [H*] and pH of a 0.294 M solution of Na₂CO3. 400.00727 x Now calculate the [H*] and pH of a 0.0087 M solution of Na₂CO3.

Salts of carbonate ion behave as a weak base, undergoing hydrolysis in water according to the equation: CO3²- + H₂O HCO3 + OH K for carbonate ion = 0.00018. Calculate the [H] and pH of a 0.294 M solution of Na₂CO3. 400.00727 x Now calculate the [H] and pH of a 0.0087 M solution of Na₂CO3.

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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Salts of carbonate ion behave as a weak base, undergoing hydrolysis in water according to the equation:
CO3²- + H₂O HCO3 + OH
K for carbonate ion = 0.00018.
Calculate the [H+] and pH of a 0.294 M solution of Na₂CO3.
0.00727
Now calculate the [H*] and pH of a 0.0087 M solution of Na₂CO3.
40
4.07

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