Self-Assessment Exercises SAE 16.22 Which of the following molecules will act as a weak base? H C-N "ལེགས་”ཡི་ ད་རི་ཨིན་ཡ O-H H H H N H H H H (i) C3N2H4 (ii) CH3CH2COOH a. only i HHHH H-C-C-C-C-O-H HHHH (iii) CH3CH2CH2CH₂OH b. only ii c. only iii d. i and iii e. all three molecules
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.
My book says, "Weak bases fall into two general categories. The first category is neutral substances that have an atom with a nonbonding pair of electrons that can accept a proton."
Then at the end of the chapter, it asks "Which of the following molecules will act as a weak base?"
Among the options on the list that are not weak bases is CH3CH2CH2CH2OH, with an O atom singly bonded to a C and an H (see picture).
So it should have 2 nonbonding electron pairs, right? So why doesn't the O on this molecule act as a base by letting an H+ ion share its non-bonded electron?
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