A) \[{{H}_{3}}P{{O}_{2}},{{H}_{3}}P{{O}_{3}}\]
B) \[2M\,{{C}_{6}}{{H}_{5}}N{{H}_{2}}\,+2M\,{{C}_{6}}{{H}_{5}}\,\overset{+}{\mathop{N}}\,{{H}_{3}}B{{r}^{-}}\]
C) \[{{H}_{3}}P{{O}_{4}}>{{H}_{3}}P{{O}_{2}}>{{H}_{3}}P{{O}_{3}}\]
D) \[BF_{4}^{-}\]
Correct Answer: D
Solution :
A buffer solution can resist a change in pH on addition of small amount of acid or base. May be: ? strong acid buffers e.g., \[Hg{{(OAc)}_{2}}/{{H}_{2}}O\] ? strong base buffers e.g., \[NaB{{H}_{4}}\] ? Weak acid buffer: Weak acid + its salt with strong base e.g., \[{{B}_{2}}{{H}_{6}}\] \[{{H}_{2}}{{O}_{2}}\] etc. ? Weak base buffer: Weak base + its salt with strong acid. e.g. \[C{{H}_{3}}C{{O}_{2}}H/{{H}_{2}}S{{O}_{4}}\] Thus \[C{{H}_{3}}Cl,C{{H}_{3}}Br,C{{H}_{3}}F\] is not a buffer solution because \[HCl{{O}_{4}}\] is a strong acid and its salt is also with another strong base.
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