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Chapter 14: Q34 E (page 829)

Nitric acid reacts with insoluble copper (II) oxide to form soluble copper (II) nitrate,Cu (NO3)2, a compound that has been used to prevent the growth of algae in swimming pools. Write the balanced chemical equation for the reaction of an aqueous solution of HNO3 with CuO.

Short Answer

Expert verified

The balanced chemical reaction for an aqueous solution is

\[2HN{O_3}(aq) + CuO(s) \to Cu{\left( {N{O_3}} \right)_2}(aq) + {H_2}O(l)\]

Step by step solution

01

Definition of the aqueous solution

Aqueousis a term used to describe a water-based system. The term aqueous can also refer to a solution or mixture in which water serves as the solvent

02

Writing balanced equation for aqueous solution

Nitric acid reacts with copper oxide and the product is Cu (NO3)2. The balanced equation is

\[2HN{O_3}(aq) + CuO(s) \to Cu{\left( {N{O_3}} \right)_2}(aq) + {H_2}O(l)\]

Cu (NO3)2also receives water and the equation is of the ionic form. The dissociate CuO is in solid state and not dissolved in water.

\[2{H^ + } + 2NO_3^ - + C{u^{2 + }} + {O^{2 - }} \to C{u^{2 + }} + 2NO_3^ - + {H_2}O\]

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Most popular questions from this chapter

Question: Show by suitable net ionic equations that each of the following species can act as a Bronsted-Lowry base: (a) \({H_2}O\) (b) \(O{H^ - }\)(c) \(N{H_3}\)(d) \(C{N^ - }\)(e) \({S^{2 - }}\)(f) \({H_2}PO_4^ - \)

Both \(HF and HCN\)ionize in water to a limited extent. Which of the conjugate bases \(F - or CN - \), is the stronger base? See Table 14.3.

What is the effect on the concentration of acetic acid, hydronium ion, and acetate ion when the following are added to an acidic buffer solution of equal concentrations of acetic acid and sodium acetate:

(a)\(HCl\)

(b)\(KC{H_3}C{O_2}\)

(c)\(NaCl\)

(d)\(KOH\)

(e)\(C{H_3}C{O_2}H\)

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 3.1? Explain your choice.
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