Sulphuric acid (H2SO4 ), used in the manufacture of fertilizers, undergo decomposition and the acid dissociation constants are given as: Ka1=1x 10^3 and Ka2=1.2 x 10^(-2) .The initial concentration of sulphuric acid is given as 0.040M.Write the dissociation reactions. Calculate the concentration of [HSO4^- ] and [SO4^(2-)]. Calculate the pH of the acid solution. Write a discussion on the behaviour of polyprotic acids. (50 -100 words) Given: Ion product constant for water, Kw=1 x 10 ^(-14)
Sulphuric acid (H2SO4 ), used in the manufacture of fertilizers, undergo decomposition and the acid dissociation constants are given as: Ka1=1x 10^3 and Ka2=1.2 x 10^(-2) .The initial concentration of sulphuric acid is given as 0.040M.Write the dissociation reactions. Calculate the concentration of [HSO4^- ] and [SO4^(2-)]. Calculate the pH of the acid solution. Write a discussion on the behaviour of polyprotic acids. (50 -100 words) Given: Ion product constant for water, Kw=1 x 10 ^(-14)
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter16: Reactions Between Acids And Bases
Section: Chapter Questions
Problem 16.77QE
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Sulphuric acid (H2SO4 ), used in the manufacture of fertilizers, undergo decomposition and the acid dissociation constants are given as: Ka1=1x 10^3 and Ka2=1.2 x 10^(-2) .
The initial concentration of sulphuric acid is given as 0.040M.
Write the dissociation reactions.
Calculate the concentration of [HSO4^- ] and [SO4^(2-)].
Calculate the pH of the acid solution.
Write a discussion on the behaviour of polyprotic acids. (50 -100 words)
Given: Ion product constant for water, Kw=1 x 10 ^(-14)
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