For numbers F to J, consider the given case: Blood contains several acid-base systems that tend to keep its pH constant at about 7.40. One of the most important buffer systems involves Carbonic acid and Bicarbonate ion. Ka=4.4 x 10-7. F. In the carbonic acid-bicarbonate ion buffersystem, which of the following functions as a weak acid? H3CO3+ H2CO3 HCO3- CO32- CO2 G. In the carbonic acid-bicarbonate ion buffersystem, which of the following functions as a conjugate base? H3CO3+ H2CO3 HCO3- CO32-CO2 H. Whatmust be the ratio of bicarbonate to carbonic acid in the blood if the pH is 7.40? 11.05:1 2.95:2 11.05:2.95 33.15:2
Ionic Equilibrium
Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
Arrhenius Acid
Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
For numbers A to E, each of the following items concerns a 0.10 M solution of a weak organic base, B. Identify whether the statements are true or false. Shade A if the statement is correct and accurate; if otherwise, shade B.
A. OH-]equals 10 M.
B. [B]is much lesser than [HB+].
C. [H3O+]is greater than [HB+].
D. ThepH is
E. [HB+]is approximately equal to [OH-].
For numbers F to J, consider the given case: Blood contains several acid-base systems that tend to keep its pH constant at about 7.40. One of the most important buffer systems involves Carbonic acid and Bicarbonate ion. Ka=4.4 x 10-7.
F. In the carbonic acid-bicarbonate ion buffersystem, which of the following functions as a weak acid?
-
- H3CO3+
- H2CO3
- HCO3-
- CO32-
- CO2
G. In the carbonic acid-bicarbonate ion buffersystem, which of the following functions as a conjugate base?
-
- H3CO3+
- H2CO3
- HCO3-
- CO32-CO2
H. Whatmust be the ratio of bicarbonate to carbonic acid in the blood if the pH is 7.40? 11.05:1
- 2.95:2
- 11.05:2.95
- 33.15:2
I. Whatis the pH of a buffer solution containing
1.00 M of sodium bicarbonate and 0.10 M carbonic acid?
- 7.40
- 7.36
- 6.32
- 6.35
- 6.64
J. What will be the resulting pH of a buffersolution containing 00 M of sodium bicarbonate and 0.10 M carbonic acid if 0.05 mol of NaOH is added?
- 5.53
- 7.36
- 7.18
- 7.68
- 7.63
K. Calculate for the % unionized if the pH of theacid is 4.66 and its dissociation constant is 1.8 x 10-5.
- 0.003%
- 45.41%
- 54.59%
- 99.99%
- Whichof the following is NOT considered as a strong acid?
- Sulfuricacid
- Hydrofluoricacid
- Hydrobromicacid
- Nitricacid
L. Whichof the following is considered as a weak base?
-
- Ammonia
- Potassiumhydroxide
- Bariumhydroxide
- All three are strong bases
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