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.
Concentration
Trial1
Concentration of iodide solution (mA)
255.8
Concentration of thiosulfate solution (mM)
47.0
Concentration of hydrogen peroxide solution (mM)
110.1
Temperature of iodide solution ('C)
25.0
Volume of iodide solution (1) used (mL)
10.0
Volume of thiosulfate solution (5:03) used (mL)
Volume of DI water used (mL)
Volume of hydrogen peroxide solution (H₂O₂) used (mL)
1.0
2.5
7.5
Time (s)
16.9
Dark blue
Observations
Initial concentration of iodide in reaction (mA)
Initial concentration of thiosulfate in reaction (mA)
Initial concentration of hydrogen peroxide in reaction (mA)
Initial Rate (mA's)
Draw the condensed or line-angle structure for an alkene with the formula C5H10.
Note: Avoid selecting cis-/trans- isomers in this exercise.
Draw two additional condensed or line-angle structures for alkenes with the formula C5H10.
Record the name of the isomers in Data Table 1.
Repeat steps for 2 cyclic isomers of C5H10
Explain why the following names of the structures are incorrect.
CH2CH3
CH3-C=CH-CH2-CH3
a. 2-ethyl-2-pentene
CH3
|
CH3-CH-CH2-CH=CH2
b. 2-methyl-4-pentene
Chapter 10 Solutions
Study Guide with Selected Solutions for Stoker's General, Organic, and Biological Chemistry, 7th
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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