The trend in acid strength has to be explained. Concept Introduction: A carboxylic acid can behave as a stronger bronsted acids when the hydrogen atom of alpha carbon is replaced by an anion. This condition is enhanced by: ( 1 ) The presence of electronegative atom. ( 2 ) The Greater positive formal charge on the central atom. ( 3 ) The Possibility of resonating structures for the anion that delocalize the negative charge on the anion, which lead to stability.
The trend in acid strength has to be explained. Concept Introduction: A carboxylic acid can behave as a stronger bronsted acids when the hydrogen atom of alpha carbon is replaced by an anion. This condition is enhanced by: ( 1 ) The presence of electronegative atom. ( 2 ) The Greater positive formal charge on the central atom. ( 3 ) The Possibility of resonating structures for the anion that delocalize the negative charge on the anion, which lead to stability.
Solution Summary: The author explains that a carboxylic acid behaves as stronger bronsted acids when the hydrogen atom of alpha carbon is replaced by an anion.
Definition Definition Number that is expressed before molecules, ions, and atoms such that it balances out the number of components present on either section of the equation in a chemical reaction. Stoichiometric coefficients can be a fraction or a whole number and are useful in determining the mole ratio among the reactants and products. In any equalized chemical equation, the number of components on either side of the equation will be the same.
Chapter 16, Problem 112IL
(a)
Interpretation Introduction
Interpretation:
The trend in acid strength has to be explained.
Concept Introduction:
A carboxylic acid can behave as a stronger bronsted acids when the hydrogen atom of alpha carbon is replaced by an anion. This condition is enhanced by:
(1) The presence of electronegative atom.
(2) The Greater positive formal charge on the central atom.
(3) The Possibility of resonating structures for the anion that delocalize the negative charge on the anion, which lead to stability.
(b)
Interpretation Introduction
Interpretation:
The trend in acid strength and the acid which have the highest pH and which have the lowest pH is to be stated.
Concept Introduction:
The pH is a measure of Hydronium ion concentration. The expression for pH is,
pH=−log[H3O+] (1)
Higher the value of Ka, stronger the acid and for the acidic solution pH<7, which means higher the value of Ka, smaller the value of pH.
Q3.
This question is about the pH of several solutions.
Give all values of pH to 2 decimal places.
(a) (i)
Write an expression for pH.
(b)
(ii)
Calculate the pH of the solution formed when 10.0 cm³ of 0.154 mol dm-³
hydrochloric acid are added to 990 cm³ of water.
The acid dissociation constant, Ka, for the weak acid HX has the value
4.83 x 10-5 mol dm-³ at 25 °C.
A solution of HX has a pH of 2.48
Calculate the concentration of HX in the solution.
Page 4 of 14
6. Acids and bases are defined by their donation or acceptance of a proton according to the
(a) Arrhenius model.
(b) Bronsted-Lowry model.
(c) Lewis model.
Ammonia, NH3, is amphoteric. (a) Give the formula for the conjugate acid of NH3. (b) Give the formula for the conjugate base of NH3.