Concept explainers
Calculate [OH-] and pH in a solution in which the hydrogen sulfite ion, HSO3-, is 0.429 M and the sulfite ion is
(a) 0.0249 M (b) 0.247 M
(c) 0.504 M (d) 0.811 M
(e) 1.223 M
(a)
Interpretation:
The molality of HSO3- ion is 0.429 M and that of
Concept Introduction :
From the hydrogen ion concentration, the concentration of hydroxide ion can be calculated as follows:
Here,
From the hydrogen ion concentration, the pH of the solution can be calculated as follows:
Answer to Problem 10QAP
Explanation of Solution
For, a buffer solution, the concentration of H+ can be calculated using the following equation:
Ka = equilibrium constant,
[HB] = concentration of weak acid.
[B-] = concentration of conjugate base.
Since,
The pH of a solution can be calculated using the formula:
pH = -log[H+]
In a buffer, the weak acid HB is the hydrogen sulfite while the conjugate base is sulfite ion.
The concentration of the sulfite ion [SO32-] is 0.0249 M. substituting the given values in equation (1)
pH of the buffer is calculated using equation (3) as follows:
[OH-] is calculated using equation (2) as follows:
So, the pH of the solution is 5.99 and [OH-] is
(b)
Interpretation:
The molality of HSO3- ion is 0.429 M and that of
Concept Introduction :
From the hydrogen ion concentration, the concentration of hydroxide ion can be calculated as follows:
Here,
From the hydrogen ion concentration, the pH of the solution can be calculated as follows:
Answer to Problem 10QAP
Explanation of Solution
The concentration of the sulfite ion [SO32-] is 0.0247 M. substituting the given values in equation (1)
pH of the buffer is calculated using equation (3) as follows:
[OH-] is calculated using equation (2) as follows:
So, the pH of the solution is 6.98 and [OH-] is
(c)
Interpretation:
The molality of HSO3- ion is 0.429 M and that of
Concept Introduction :
From the hydrogen ion concentration, the concentration of hydroxide ion can be calculated as follows:
Here,
From the hydrogen ion concentration, the pH of the solution can be calculated as follows:
Answer to Problem 10QAP
Explanation of Solution
The concentration of the sulfite ion [SO32-] is 0.504 M. substituting the given values in equation (1)
pH of the buffer is calculated using equation (3) as follows:
[OH-] is calculated using equation (2) as follows:
So, the pH of the solution is 7.29 and [OH-] is
(d)
Interpretation:
The molality of HSO3- ion is 0.429 M and that of
Concept Introduction :
From the hydrogen ion concentration, the concentration of hydroxide ion can be calculated as follows:
Here,
From the hydrogen ion concentration, the pH of the solution can be calculated as follows:
Answer to Problem 10QAP
Explanation of Solution
The concentration of the sulfite ion [SO32-] is 0.811 M. substituting the given values in equation (1)
pH of the buffer is calculated using equation (3) as follows:
[OH-] is calculated using equation (2) as follows:
So, the pH of the solution is 7.50 and [OH-] is
(e)
Interpretation:
The molality of HSO3- ion is 0.429 M and that of
Concept Introduction :
From the hydrogen ion concentration, the concentration of hydroxide ion can be calculated as follows:
Here,
From the hydrogen ion concentration, the pH of the solution can be calculated as follows:
Answer to Problem 10QAP
Explanation of Solution
The concentration of the sulfite ion [SO32-] is 1.223 M. substituting the given values in equation (1)
pH of the buffer is calculated using equation (3) as follows:
[OH-] is calculated using equation (2) as follows:
So, the pH of the solution is 7.68and [OH-] is
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Chapter 14 Solutions
OWLV2 FOR MASTERTON/HURLEY'S CHEMISTRY:
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