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Chapter 14: Q33 E (page 829)

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

Short Answer

Expert verified

The conjugate acid-base pairs are

\[2HCl(aq) + Mg{(OH)_2}(aq) \to MgC{l_2}(aq) + 2{H_2}O(l)\]

Acid: HCl

Base: Mg(OH)2

Conjugated acid: Cl-

Conjugated base: Mg2+

Step by step solution

01

Definition of conjugate acid-base pairs

Conjugate acid-base pairs are acid-base pairs that differ only by one proton. The loss or gain of a proton leads to the formation of such acid-base couples.

02

Balancing equation for the neutralization reaction

Milk of magnesia is Mg(OH)2and it is used to neutralize gastric acid HCl for balanced neutralized reaction.

\[2HCl(aq) + Mg{(OH)_2}(aq) \to MgCl{l_2}(aq) + 2{H_2}O(l)\]

To determine acid or conjugated base and base or conjugated pairs in the ionic form

\[2HCl(aq) + Mg{(OH)_2}(aq) \to M{g^{2 + }}(aq) + 2{C^ - }(aq) + 2{H_2}O(l)\]

Bronsted-Lowry’s acid is a proton donor, while it is a base is proton acceptor.HCl after donating proton become as Cl-. Mg (OH)2accepts proton from HCl to produce a molecule of water and Mg2+, so that Mg (OH)2is a base .To determine if the product is an acid or a base it is called conjugate to from reactants Cl-to accept the proton in order to become HCl as a conjugated base. Mg2+is a conjugated acid.

The conjugate acid-base pairs are

\[2HCl(aq) + Mg{(OH)_2}(aq) \to MgC{l_2}(aq) + 2{H_2}O(l)\]

Acid:HCl

Base: Mg (OH)2

Conjugated acid: Cl-

Conjugated base: Mg2+

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Most popular questions from this chapter

What is the ionization constant at \(2{5^o}C\) for the weak acid \({\left( {C{H_3}} \right)_2}NH_2^ + \), the conjugate acid of the weak base \({\left( {C{H_3}} \right)_2}NH\), \({K_b} = 5.9 \times 1{0^{ - 4}}\)?

Identify and label the Brønsted-Lowry acid, its conjugate base, the Brønsted-Lowry base, and its conjugate acid in each of the following equations:

\({\rm{\;(a)\;HN}}{{\rm{O}}_3} + {{\rm{H}}_2}{\rm{O}} \to {{\rm{H}}_3}{{\rm{O}}^ + } + {\rm{NO}}_3^ - \)

\({\rm{b) C}}{{\rm{N}}^ - } + {{\rm{H}}_2}{\rm{O}} \to {\rm{HCN}} + {\rm{O}}{{\rm{H}}^ - }\)

\({\rm{\;(c)\;}}{{\rm{H}}_2}{\rm{S}}{{\rm{O}}_4} + {\rm{C}}{{\rm{l}}^ - } \to {\rm{HCl}} + {\rm{HSO}}_4^ - \)

\({\rm{\;(d)\;HSO}}_4^ - + {\rm{O}}{{\rm{H}}^ - } \to {\rm{SO}}_4^{2 - } + {{\rm{H}}_2}{\rm{O}}\)

\({\rm{\;(e)\;}}{{\rm{O}}^{2 - }} + {{\rm{H}}_2}{\rm{O}} \to 2{\rm{O}}{{\rm{H}}^ - }\)

\({\rm{\;(f)\;}}{\left( {{\rm{Cu}}{{\left( {{{\rm{H}}_2}{\rm{O}}} \right)}_3}({\rm{OH}})} \right)^ + } + {\left( {{\rm{Al}}{{\left( {{{\rm{H}}_2}{\rm{O}}} \right)}_6}} \right)^{3 + }} \to {\left( {{\rm{Cu}}{{\left( {{{\rm{H}}_2}{\rm{O}}} \right)}_4}} \right)^{2 + }} + {\left( {{\rm{Al}}{{\left( {{{\rm{H}}_2}{\rm{O}}} \right)}_5}({\rm{OH}})} \right)^{2 + }}\)

\({\rm{\;(g)\;}}{{\rm{H}}_2}{\rm{S}} + {\rm{NH}}_2^ - \to {\rm{H}}{{\rm{S}}^ - } + {\rm{N}}{{\rm{H}}_3}\)

Which acid in Table 14.2 is most appropriate for preparation of a buffer solution with a pH of 3.7? Explain your choice.

The odour of vinegar is due to the presence of acetic acid, \(C{H_3}C{O_2}H\), a weak acid. List, in order of descending concentration, all of the ionic and molecular species present in a \(1 - \)M aqueous solution of this acid.

Saccharin, \({{\bf{C}}_{\bf{7}}}{{\bf{H}}_{\bf{4}}}{\bf{NS}}{{\bf{O}}_{\bf{3}}}{\bf{H}}\), is a weak acid\(\left( {{\bf{Ka = 2}}{\bf{.1 \times 1}}{{\bf{0}}^{{\bf{ - 2}}}}} \right)\). If \({\bf{0}}.{\bf{250}}{\rm{ }}{\bf{L}}\) of diet cola with a buffered pH of \({\bf{5}}.{\bf{48}}\) was prepared from \({\bf{2}}.{\bf{00}}{\rm{ }} \times {\rm{ }}{\bf{1}}{{\bf{0}}^{ - {\bf{3}}}}{\bf{g}}\) of sodium saccharide, \({\bf{Na}}\left( {{{\bf{C}}_{\bf{7}}}{{\bf{H}}_{\bf{4}}}{\bf{NS}}{{\bf{O}}_{\bf{3}}}} \right)\), what are the final concentrations of saccharine and sodium saccharide in the solution?
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