The following reactions apply to Exercises 99 through 109 . (a) H2 SO4(aq)+2 KOH(aq) ⟶K2 SO4(aq)

Name: Problem 99, Chapter 6: Chemistry
Uploaded: 2021-05-28T19:17:52-08:00
Duration: 1 min 7 s
Channel: Ronald Prasad

step 1 From the list of chemical reactions, let's identify the precipitation reaction. So a precipitati

Question

The following reactions apply to Exercises 99 through $109 .$ (a) $\mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq})+2 \mathrm{KOH}(\mathrm{aq}) \longrightarrow \mathrm{K}_{2} \mathrm{SO}_{4}(\mathrm{aq})+2 \mathrm{H}_{2} \mathrm{O}(\ell)$ (b) $2 \mathrm{Rb}(\mathrm{s})+\mathrm{Br}_{2}(\ell) \stackrel{\text { heat }}{\longrightarrow} 2 \mathrm{RbBr}(\mathrm{s})$ (c) $2 \mathrm{KI}(\mathrm{aq})+\mathrm{F}_{2}(\mathrm{~g}) \longrightarrow 2 \mathrm{KF}(\mathrm{aq})+\mathrm{I}_{2}(\mathrm{~s})$ (d) $\mathrm{CaO}(\mathrm{s})+\mathrm{SiO}_{2}(\mathrm{~s}) \stackrel{\text { heat }}{\longrightarrow} \mathrm{CaSiO}_{3}(\mathrm{~s})$ (e) $\mathrm{S}(\mathrm{s})+\mathrm{O}_{2}(\mathrm{~g}) \stackrel{\text { heat }}{\longrightarrow} \mathrm{SO}_{2}(\mathrm{~g})$ (f) $\mathrm{BaCO}_{3}(\mathrm{~s}) \stackrel{\text { heat }}{\longrightarrow} \mathrm{BaO}(\mathrm{s})+\mathrm{CO}_{2}(\mathrm{~g})$ (g) $\mathrm{HgS}(\mathrm{s})+\mathrm{O}_{2}(\mathrm{~g}) \stackrel{\text { heat }}{\longrightarrow} \mathrm{Hg}(\ell)+\mathrm{SO}_{2}(\mathrm{~g})$ (h) $\mathrm{AgNO}_{3}(\mathrm{aq})+\mathrm{HCl}(\mathrm{aq}) \longrightarrow \mathrm{AgCl}(\mathrm{s})+\mathrm{HNO}_{3}(\mathrm{aq})$ (i) $\mathrm{Pb}(\mathrm{s})+2 \mathrm{HBr}(\mathrm{aq}) \longrightarrow \mathrm{PbBr}_{2}(\mathrm{~s})+\mathrm{H}_{2}(\mathrm{~g})$ (j) $2 \mathrm{HI}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}_{2}(\mathrm{aq}) \longrightarrow \mathrm{I}_{2}(\mathrm{~s})+2 \mathrm{H}_{2} \mathrm{O}(\ell)$ (k) $\mathrm{RbOH}(\mathrm{aq})+\mathrm{HNO}_{3}(\mathrm{aq}) \longrightarrow \mathrm{Rb} \mathrm{NO}_{3}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell)$ (l) $\mathrm{N}_{2} \mathrm{O}_{5}(\mathrm{~s})+\mathrm{H}_{2} \mathrm{O}(\ell) \longrightarrow 2 \mathrm{HNO}_{3}(\mathrm{aq})$ $(\mathrm{m}) \mathrm{H}_{2} \mathrm{O}(\mathrm{g})+\mathrm{CO}(\mathrm{g}) \stackrel{\text { heat }}{\longrightarrow} \mathrm{H}_{2}(\mathrm{~g})+\mathrm{CO}_{2}(\mathrm{~g})$ (n) $\mathrm{MgO}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(\ell) \longrightarrow \mathrm{Mg}(\mathrm{OH})_{2}(\mathrm{~s})$ (o) $\mathrm{PbSO}_{4}(\mathrm{~s})+\mathrm{PbS}(\mathrm{s}) \stackrel{\text { heat }}{\longrightarrow} 2 \mathrm{~Pb}(\mathrm{~s})+2 \mathrm{SO}_{2}(\mathrm{~g})$ Identify the precipitation reactions.

   The following reactions apply to Exercises 99 through $109 .$
(a) $\mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq})+2 \mathrm{KOH}(\mathrm{aq}) \longrightarrow \mathrm{K}_{2} \mathrm{SO}_{4}(\mathrm{aq})+2 \mathrm{H}_{2} \mathrm{O}(\ell)$
(b) $2 \mathrm{Rb}(\mathrm{s})+\mathrm{Br}_{2}(\ell) \stackrel{\text { heat }}{\longrightarrow} 2 \mathrm{RbBr}(\mathrm{s})$
(c) $2 \mathrm{KI}(\mathrm{aq})+\mathrm{F}_{2}(\mathrm{~g}) \longrightarrow 2 \mathrm{KF}(\mathrm{aq})+\mathrm{I}_{2}(\mathrm{~s})$
(d) $\mathrm{CaO}(\mathrm{s})+\mathrm{SiO}_{2}(\mathrm{~s}) \stackrel{\text { heat }}{\longrightarrow} \mathrm{CaSiO}_{3}(\mathrm{~s})$
(e) $\mathrm{S}(\mathrm{s})+\mathrm{O}_{2}(\mathrm{~g}) \stackrel{\text { heat }}{\longrightarrow} \mathrm{SO}_{2}(\mathrm{~g})$
(f) $\mathrm{BaCO}_{3}(\mathrm{~s}) \stackrel{\text { heat }}{\longrightarrow} \mathrm{BaO}(\mathrm{s})+\mathrm{CO}_{2}(\mathrm{~g})$
(g) $\mathrm{HgS}(\mathrm{s})+\mathrm{O}_{2}(\mathrm{~g}) \stackrel{\text { heat }}{\longrightarrow} \mathrm{Hg}(\ell)+\mathrm{SO}_{2}(\mathrm{~g})$
(h) $\mathrm{AgNO}_{3}(\mathrm{aq})+\mathrm{HCl}(\mathrm{aq}) \longrightarrow \mathrm{AgCl}(\mathrm{s})+\mathrm{HNO}_{3}(\mathrm{aq})$
(i) $\mathrm{Pb}(\mathrm{s})+2 \mathrm{HBr}(\mathrm{aq}) \longrightarrow \mathrm{PbBr}_{2}(\mathrm{~s})+\mathrm{H}_{2}(\mathrm{~g})$
(j) $2 \mathrm{HI}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}_{2}(\mathrm{aq}) \longrightarrow \mathrm{I}_{2}(\mathrm{~s})+2 \mathrm{H}_{2} \mathrm{O}(\ell)$
(k) $\mathrm{RbOH}(\mathrm{aq})+\mathrm{HNO}_{3}(\mathrm{aq}) \longrightarrow \mathrm{Rb} \mathrm{NO}_{3}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell)$
(l) $\mathrm{N}_{2} \mathrm{O}_{5}(\mathrm{~s})+\mathrm{H}_{2} \mathrm{O}(\ell) \longrightarrow 2 \mathrm{HNO}_{3}(\mathrm{aq})$
$(\mathrm{m}) \mathrm{H}_{2} \mathrm{O}(\mathrm{g})+\mathrm{CO}(\mathrm{g}) \stackrel{\text { heat }}{\longrightarrow} \mathrm{H}_{2}(\mathrm{~g})+\mathrm{CO}_{2}(\mathrm{~g})$
(n) $\mathrm{MgO}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(\ell) \longrightarrow \mathrm{Mg}(\mathrm{OH})_{2}(\mathrm{~s})$
(o) $\mathrm{PbSO}_{4}(\mathrm{~s})+\mathrm{PbS}(\mathrm{s}) \stackrel{\text { heat }}{\longrightarrow} 2 \mathrm{~Pb}(\mathrm{~s})+2 \mathrm{SO}_{2}(\mathrm{~g})$
Identify the precipitation reactions.

Chemistry

Kenneth W. Whitten,… 10th Edition

Chapter 6, Problem 99

Instant Answer

Solved by Expert Ronald Prasad

05/28/2021

Step 1

In this case, we are looking for precipitation reactions. Precipitation reactions are reactions where two aqueous (water-based) solutions combine to form an insoluble solid (the precipitate) and another aqueous solution. Show more…

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The following reactions apply to Exercises 99 through $109 .$ (a) $\mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq})+2 \mathrm{KOH}(\mathrm{aq}) \longrightarrow \mathrm{K}_{2} \mathrm{SO}_{4}(\mathrm{aq})+2 \mathrm{H}_{2} \mathrm{O}(\ell)$ (b) $2 \mathrm{Rb}(\mathrm{s})+\mathrm{Br}_{2}(\ell) \stackrel{\text { heat }}{\longrightarrow} 2 \mathrm{RbBr}(\mathrm{s})$ (c) $2 \mathrm{KI}(\mathrm{aq})+\mathrm{F}_{2}(\mathrm{~g}) \longrightarrow 2 \mathrm{KF}(\mathrm{aq})+\mathrm{I}_{2}(\mathrm{~s})$ (d) $\mathrm{CaO}(\mathrm{s})+\mathrm{SiO}_{2}(\mathrm{~s}) \stackrel{\text { heat }}{\longrightarrow} \mathrm{CaSiO}_{3}(\mathrm{~s})$ (e) $\mathrm{S}(\mathrm{s})+\mathrm{O}_{2}(\mathrm{~g}) \stackrel{\text { heat }}{\longrightarrow} \mathrm{SO}_{2}(\mathrm{~g})$ (f) $\mathrm{BaCO}_{3}(\mathrm{~s}) \stackrel{\text { heat }}{\longrightarrow} \mathrm{BaO}(\mathrm{s})+\mathrm{CO}_{2}(\mathrm{~g})$ (g) $\mathrm{HgS}(\mathrm{s})+\mathrm{O}_{2}(\mathrm{~g}) \stackrel{\text { heat }}{\longrightarrow} \mathrm{Hg}(\ell)+\mathrm{SO}_{2}(\mathrm{~g})$ (h) $\mathrm{AgNO}_{3}(\mathrm{aq})+\mathrm{HCl}(\mathrm{aq}) \longrightarrow \mathrm{AgCl}(\mathrm{s})+\mathrm{HNO}_{3}(\mathrm{aq})$ (i) $\mathrm{Pb}(\mathrm{s})+2 \mathrm{HBr}(\mathrm{aq}) \longrightarrow \mathrm{PbBr}_{2}(\mathrm{~s})+\mathrm{H}_{2}(\mathrm{~g})$ (j) $2 \mathrm{HI}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}_{2}(\mathrm{aq}) \longrightarrow \mathrm{I}_{2}(\mathrm{~s})+2 \mathrm{H}_{2} \mathrm{O}(\ell)$ (k) $\mathrm{RbOH}(\mathrm{aq})+\mathrm{HNO}_{3}(\mathrm{aq}) \longrightarrow \mathrm{Rb} \mathrm{NO}_{3}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell)$ (l) $\mathrm{N}_{2} \mathrm{O}_{5}(\mathrm{~s})+\mathrm{H}_{2} \mathrm{O}(\ell) \longrightarrow 2 \mathrm{HNO}_{3}(\mathrm{aq})$ $(\mathrm{m}) \mathrm{H}_{2} \mathrm{O}(\mathrm{g})+\mathrm{CO}(\mathrm{g}) \stackrel{\text { heat }}{\longrightarrow} \mathrm{H}_{2}(\mathrm{~g})+\mathrm{CO}_{2}(\mathrm{~g})$ (n) $\mathrm{MgO}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(\ell) \longrightarrow \mathrm{Mg}(\mathrm{OH})_{2}(\mathrm{~s})$ (o) $\mathrm{PbSO}_{4}(\mathrm{~s})+\mathrm{PbS}(\mathrm{s}) \stackrel{\text { heat }}{\longrightarrow} 2 \mathrm{~Pb}(\mathrm{~s})+2 \mathrm{SO}_{2}(\mathrm{~g})$ Identify the precipitation reactions.

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Key Concepts

Precipitation Reaction

A precipitation reaction is a type of chemical reaction in which two aqueous solutions combine to form an insoluble solid called a precipitate. This reaction is driven by the formation of a product that is not soluble in water, causing it to separate from the solution and appear as a solid.

Double Displacement Reaction

Double displacement reactions involve the exchange of ions between two reactants in aqueous solution. In these reactions, the cations and anions swap partners, and if one of the products is insoluble, a precipitation reaction occurs. This is a common mechanism for producing precipitates.

Solubility Rules

Solubility rules are empirical guidelines that help predict whether a particular ionic compound will dissolve in water. By knowing these rules, one can determine whether the mixing of two aqueous solutions will result in the formation of a precipitate based on the solubility of the potential products.

Aqueous Solutions

Aqueous solutions are mixtures where substances (typically ionic compounds) are dissolved in water. The behavior of ions in an aqueous solution, including their potential combination to form an insoluble compound, is fundamental to understanding precipitation reactions.

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