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.
At 90ºC the vapor pressure of ortho-xylene is 20 kPa and that of meta-xylene is 18 kPa. What is the composition of the vapor in equilibrium with a mixture in which the mole fraction of o-xylene is 0.60?
Draw the products of this reduction of a ketone with sodium borohydride.
Use a dash or wedge bond to indicate the stereochemistry of substituents on
asymmetric centers, where applicableIgnore any inorganic byproducts.
1) NaBH4
2) HCI/H2O
Select to Draw
Why do you think people who live at high altitudes are advised to add salt to water when boiling food like pasta? What mole fraction of NaCl is needed to raise the boiling point of H2O by 3˚C? Does the amount of salt added to water (typically about one teaspoon to four quarts of water) substantially change the boiling point? (Kb (H2O) = 0.51˚C/molal.)
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, biology and related others by exploring similar questions and additional content below.
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell