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Chapter 14: Q14.1-11 E (page 827)

What are amphiprotic species? Illustrate with suitable equations.

Short Answer

Expert verified

Amphiprotic species are the compounds that can act both as a Bronsted-Lowry's acid and base. Example of water acting as an amphiprotic species:

\(\begin{aligned}{{\rm{HCl}}(aq) + {{\rm{H}}_2}{\rm{O}}(l) \to {\rm{C}}{{\rm{l}}^ - }(aq) + {{\rm{H}}_3}{{\rm{O}}^ + }(aq)}\\{{{\rm{S}}^{2 - }} + {{\rm{H}}_2}{\rm{O}}(l) \to {\rm{H}}{{\rm{S}}^ - }(aq) + {\rm{O}}{{\rm{H}}^ - }(aq)}\end{aligned}\)

Step by step solution

01

Amphiprotic species

Amphiprotic species are the compounds that can act both as a Bronsted-Lowry's acid and base. (Reminder: Bronsted-Lowry's acid is proton \(\left( {{H^ + }} \right)\)donor and its base is proton acceptor).

02

Explanation using equation

One example is water - here are following equations:

\({\rm{HCl}}(aq) + {{\rm{H}}_2}{\rm{O}}(l) \to {\rm{C}}{{\rm{l}}^ - }(aq) + {{\rm{H}}_3}{{\rm{O}}^ + }(aq)\)

Here water acts as a proton acceptor, hence it is Bronsted-Lowry's base.

\({S^{2 - }} + {H_2}O(l) \to {\rm{H}}{{\rm{S}}^ - }(aq) + O{H^ - }(aq)\)In this case water donates a proton to the hence it is Bronsted-Lowry's acid. With these two equations we see that water is amphiprotic - can act as an acid or a base.

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Most popular questions from this chapter

What is the conjugate acid of each of the following? What is the conjugate base of each?

  1. \({\rm{O}}{{\rm{H}}^{^ - }}\)
  2. \({{\rm{H}}_2}O\)
  3. \({\rm{HCO}}_3^ - \)
  4. \({\rm{N}}{{\rm{H}}_3}\)
  5. \({\rm{HSO}}_4^ - \)
  6. \({{\rm{H}}_2}{\rm{PO}}_4^ - \)
  7. \({\rm{H}}{{\rm{S}}^ - }\)
  8. \({{\rm{H}}_5}{{\rm{N}}_2}^ + \)

Gastric juice, the digestive fluid produced in the stomach, contains hydrochloric acid, and HCl. Milk of Magnesia, a suspension of solid Mg(OH)2 in an aqueous medium, is sometimes used to neutralize excess stomach acid. Write a complete balanced equation for the neutralization reaction, and identify the conjugate acid-base pairs

What are the hydronium and hydroxide ion concentrations in a solution whose \(pH\) is \(6.52?\)

What is the ionization constant at 25oC for the weak acid \(C{H_3}NH_3^ + \), the conjugate acid of the weak base \(C{H_3}N{H_2}\)\({K_b} = 4.4 \times 1{0^{ - 4}}\) ,.

14.2 What is the hydronium ion concentration in an aqueous solution with a hydroxide ion concentration of 0.001 M at 25虋C?
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