Brønsted–Lowry acid–base theory

Chemistry Level 1

In chemistry, the Brønsted–Lowry theory is an acid–base reaction theory, proposed independently by Johannes Nicolaus Brønsted and Thomas Martin Lowry in $1923.$ The fundamental concept of this theory is that an acid (or Brønsted acid) is defined as being able to lose, or "donate" a proton (the hydrogen cation, or $\ce{H+}$ ) while a base (or Brønsted base) is defined as a species with the ability to gain, or "accept," a proton. The above shows the reaction model where an ammonia $(\ce{NH3})$ and a hydrogen chloride $(\ce{HCl})$ molecules react to produce an ammonium ion $(\ce{NH4+})$ and a chloride ion $(\ce{Cl-})$ . Which of the following correctly lists all, if any, of the Brønsted acids and Brønsted bases?

acid:

\ce{NH4+}

, base:

\ce{Cl-}

acid:

\ce{HCl}

, base:

\ce{NH3}

acid:

\ce{HCl}

and

\ce{NH4+}

, base:

\ce{NH3}

and

\ce{Cl-}

acid:

\ce{NH3}

and

\ce{Cl-}

, base:

\ce{HCl}

and

\ce{NH4+}

1 solution

Anish Puthuraya
Mar 9, 2014

According to Bronsted-Lowry theory of acids,
An acid donates $\displaystyle H^+$ ions, while a base accepts $\displaystyle H^+$ ions (or supplies $\displaystyle OH^-$ ions)

Thus, in this case,
$HCl$ and $NH_4^+$ are the $H^+$ donating substances (acid)
$NH_3$ and $Cl^-$ are the $H^+$ accepting substances (base)

Brønsted–Lowry acid–base theory

1 solution

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