Predict how each molecule or ion would act, in the Brønsted-Lowry sense, in aqueous solution by writing "acid," "base," "both,"
or "neither" on the line provided.
2 answers:
Answer:
Both
Explanation:
produce OH− (hydroxide) ions. According to this view, an acid–base reaction involves the reaction of a proton with a hydroxide ion to form water. Although Brønsted and Lowry defined an acid similarly to Arrhenius by describing an acid as any substance that can donate a proton, the Brønsted–Lowry definition of a base is much more general than the Arrhenius definition. In Brønsted–Lowry terms, a base is any substance that can accept a proton, so a base is not limited to just a hydroxide ion. This means that for every Brønsted–Lowry acid, there exists a corresponding conjugate base with one fewer proton, as we demonstrated in Chapter 4 "Reactions in Aqueous Solution". Consequently, all Brønsted–Lowry acid–base reactions actually involve two conjugate acid–base pairs and the transfer of a proton from one substance (the acid) to another (the base). In contrast, the Lewis definition of acids and bases, discussed in Chapter 8 "Ionic versus Covalent Bonding", focuses on accepting or donating pairs of electrons rather than protons. A Lewis base is an electron-pair donor, and a Lewis acid is an electron-pair acceptor.
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Answer: The pH of 0.10 M is 4.49.
Explanation:
Given: Initial concentration of = 0.10 M
Let us assume that amount of dissociates is x. So, ICE table for dissociation of
is as follows.
Initial: 0.10 M 0 0
Change: -x +x +x
Equilibrium: (0.10 - x) M x x
As the value of is very small. So, it is assumed that the compound will dissociate very less. Hence, x << 0.10 M.
And, (0.10 - x) will be approximately equal to 0.10 M.
The expression for value is as follows.
Hence,
Formula to calculate pH is as follows.
Substitute the values into above formula as follows.
Thus, we can conclude that the pH of 0.10 M is 4.49.