When added small amount of strong base the changes of buffer solution concentration has to be discussed. Concept Introduction: A buffer is an aqueous solution containing substances that prevent major changes in solution pH when small amounts of acid or base are added to it. pH definition: The concentration of hydrogen ion is measured using pH scale. The acidity of aqueous solution is expressed by pH scale. The value pH of a solution is defined as the negative base-10 logarithm of the hydrogen or hydronium ion concentration. pH = -log[H 3 O + ] Based on the pH value, a solution can be classified as acidic, basic or neutral solution. pH < 7, acidic solution pH > 7, basic solution pH = 7, neutral solution Strong acid: In strong acids, the ionization of acid is complete. This implies that the concentration of the hydrogen ion or hydronium ion will be equal to the initial concentration of the acid at equilibrium. Weak acid: In weak acids, the ionization of acid is not complete. This implies that the concentration of the hydrogen ion or hydronium ion will not be equal to the initial concentration of the acid at equilibrium. For strong acids the concentration of acid will be same as that of the concentration of hydrogen ions, because strong acids undergo complete ionization. In case of weak acid, the concentration of hydrogen ion will be less than the concentration of given acid; since weak acid does not ionize completely.
When added small amount of strong base the changes of buffer solution concentration has to be discussed. Concept Introduction: A buffer is an aqueous solution containing substances that prevent major changes in solution pH when small amounts of acid or base are added to it. pH definition: The concentration of hydrogen ion is measured using pH scale. The acidity of aqueous solution is expressed by pH scale. The value pH of a solution is defined as the negative base-10 logarithm of the hydrogen or hydronium ion concentration. pH = -log[H 3 O + ] Based on the pH value, a solution can be classified as acidic, basic or neutral solution. pH < 7, acidic solution pH > 7, basic solution pH = 7, neutral solution Strong acid: In strong acids, the ionization of acid is complete. This implies that the concentration of the hydrogen ion or hydronium ion will be equal to the initial concentration of the acid at equilibrium. Weak acid: In weak acids, the ionization of acid is not complete. This implies that the concentration of the hydrogen ion or hydronium ion will not be equal to the initial concentration of the acid at equilibrium. For strong acids the concentration of acid will be same as that of the concentration of hydrogen ions, because strong acids undergo complete ionization. In case of weak acid, the concentration of hydrogen ion will be less than the concentration of given acid; since weak acid does not ionize completely.
Solution Summary: The author explains that a buffer solution contains substances that prevent major changes in solution pH when small amounts of acid or base are added.
In strong acids, the ionization of acid is complete. This implies that the concentration of the hydrogen ion or hydronium ion will be equal to the initial concentration of the acid at equilibrium.
Weak acid:
In weak acids, the ionization of acid is not complete. This implies that the concentration of the hydrogen ion or hydronium ion will not be equal to the initial concentration of the acid at equilibrium.
For strong acids the concentration of acid will be same as that of the concentration of hydrogen ions, because strong acids undergo complete ionization.
In case of weak acid, the concentration of hydrogen ion will be less than the concentration of given acid; since weak acid does not ionize completely.
If 4 mL of 1 M NaOH is added to 100 mL buffer, would it still be a usable buffer according to the conventions? Explain why or why not.
Define the following:- pH- Buffer- pKa
Refer to the following titration curve below:
13
12
11
10
7
5
4
3
2
8
10
12 14
16
18
20
22
24
26
28
30
Volume of Titrant / mL
Unknown Acid 0.10 mol/L - titrant = NaOH 0.1 mol/L
How many buffering regions are present in the titration curve of
the amino acid?
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