(a)
To explain: Which proton is dissociated at a lower pH – the proton of the
Concept introduction: As per chemistry, the substance which is capable of donating a proton (H+) is considered as an acid and is able to form a covalent bond with an electron. Also, the substance which accepts a proton is called a base. The pH of a solution is denoted as the negative logarithm of the hydrogen ion concentration of that solution. The pH in a solution decreases as H+ ion concentration increases in the solution.
(b)
To explain: The chemical formula to describe the dissociation of the first and second protons of glycine hydrochloride (Cl-H3N+CH2COOH)
Concept introduction: As per chemistry, the substance which is capable of donating a proton (H+) is considered as an acid and is able to form a covalent bond with an electron. Also, the substance which accepts a proton is called a base. The pH of a solution is denoted as the negative logarithm of the hydrogen ion concentration of that solution. The pH in a solution decreases as H+ ion concentration increases in the solution.
(c)
To calculate: The pK of the solution as per the given data.
Concept introduction: As per chemistry, the substance which is capable of donating a proton (H+) is considered as an acid and is able to form a covalent bond with an electron. Also, the substance which accepts a proton is called a base. The pH of a solution is denoted as the negative logarithm of the hydrogen ion concentration of that solution. The pH in a solution decreases as H+ ion concentration increases in the solution.
(d)
To sketch: The titration curve of glycine hydrochloride (Cl-H3N+CH2COOH) in an analogy with Fig. 2-18 in the textbook.
Concept introduction: As per chemistry, the substance which is capable of donating a proton (H+) is considered as an acid and is able to form a covalent bond with an electron. Also, the substance which accepts a proton is called a base. The pH of a solution is denoted as the negative logarithm of the hydrogen ion concentration of that solution. The pH in a solution decreases as H+ ion concentration increases in the solution.
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