When added small amount of strong acid 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 acid 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 aqueous solutions can be classified as acidic, basic or neutral. Strong acids undergo complete ionization and weak acid does not.
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.
Explain thoroughly the Buffering Action of following Biological or Physiological Buffers:(a) Phosphate Buffer System.(b) Bicarbonate Buffer system.
Bicarbonate/carbonic acid buffer in blood is an example of an equilibrium reaction that is meant to be very insensitive to change. How does the bicarbonate/carbonic acid buffer re-establish equilibrium if acidity increases? How does the bicarbonate/carbonic acid buffer re-establish equilibrium if alkalinity increases?
Calcium carbonate (CaCO₃(s)) is an important building material (limestone) and a quick cure for acid indigestion (TUMS). Ksp = 8.7x10⁻⁹ for CaCO₃(s). What, if any, is the effect of lowering the pH (as occurs in acid rain and acid indigestion) on the solubility of CaCO₃(s). (hint: use Le Chatelier's principle)
A) there is no effect from lowering pH on CaCO₃(s) solubility
B) lowering pH increases the CaCO₃(s) solubility
C) additional information is required to determine the outcome
D) lowering the pH lowers the solubility
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