Naoh Hcl Net Ionic Equation

7.ane Writing and Balancing Chemical Equations

1.

What does it hateful to say an equation is counterbalanced? Why is it important for an equation to be balanced?

ii .

Consider molecular, complete ionic, and cyberspace ionic equations.

(a) What is the deviation betwixt these types of equations?

(b) In what circumstance would the complete and internet ionic equations for a reaction exist identical?

three.

Remainder the post-obit equations:

(a) ${\text{PCl}}_{\mathrm{v}}(s)+{\text{H}}_2\text{O}(\mathrm{fifty})⟶{\text{POCl}}_3(\mathrm{50})+\text{HCl}(aq)$

(b) $\text{Cu}(s)+{\text{HNO}}_3(aq)⟶\text{Cu}{({\text{NO}}_{\mathrm{three}})}_2(aq)+{\text{H}}_{\mathrm{two}}\text{O}(\mathrm{50})+\text{NO}(\mathrm{thou})$

(c) ${\text{H}}_{\mathrm{two}}(\mathrm{1000})+{\text{I}}_{\mathrm{two}}(\mathrm{south})⟶\text{Hi}(s)$

(d) $\text{Fe}(s)+{\text{O}}_2(\mathrm{thou})⟶{\text{Fe}}_2{\text{O}}_3(\mathrm{south})$

(e) $\text{Na}(s)+{\text{H}}_2\text{O}(\mathrm{fifty})⟶\text{NaOH}(aq)+{\text{H}}_2(\mathrm{yard})$

(f) $({\text{NH}}_4{)}_2{\text{Cr}}_2{\text{O}}_7(s)⟶{\text{Cr}}_2{\text{O}}_3(s)+{\text{N}}_2(k)+{\text{H}}_2\text{O}(\mathrm{grand})$

(grand) ${\text{P}}_{\mathrm{four}}(s)+{\text{Cl}}_{\mathrm{ii}}(g)⟶{\text{PCl}}_3(\mathrm{fifty})$

(h) ${\text{PtCl}}_4(\mathrm{southward})⟶\text{Pt}(s)+{\text{Cl}}_{\mathrm{two}}(g)$

4 .

Balance the following equations:

(a) $\text{Ag}(s)+{\text{H}}_2\text{S}(\mathrm{one\; thousand})+{\text{O}}_2(\mathrm{grand})⟶{\text{Ag}}_2\text{S}(\mathrm{due\; south})+{\text{H}}_2\text{O}(l)$

(b) ${\text{P}}_{\mathrm{iv}}(s)+{\text{O}}_2(\mathrm{thou})⟶{\text{P}}_4{\text{O}}_{\mathrm{x}}(\mathrm{due\; south})$

(c) $\text{Pb}(s)+{\text{H}}_2\text{O}(l)+{\text{O}}_{\mathrm{ii}}(\mathrm{one\; thousand})⟶{\text{Lead(OH)}}_2(s)$

(d) $\text{Fe}(\mathrm{south})+{\text{H}}_2\text{O}(\mathrm{50})⟶{\text{Fe}}_3{\text{O}}_{\mathrm{iv}}(\mathrm{south})+{\text{H}}_{\mathrm{two}}(g)$

(e) ${\text{Sc}}_2{\text{O}}_{\mathrm{iii}}(s)+{\text{SO}}_3(l)⟶{\text{Sc}}_{\text{2}}({\text{S}{\text{O}}_4)}_3(\mathrm{south})$

(f) ${\text{Ca}}_{\text{3}}({\text{P}{\text{O}}_4)}_{\mathrm{ii}}(aq)+{\text{H}}_3{\text{PO}}_{\mathrm{four}}(aq)⟶\text{Ca}{({\text{H}}_2{\text{PO}}_{\mathrm{iv}})}_2(aq)$

(g) $\text{Al}(s)+{\text{H}}_2{\text{SO}}_{\mathrm{iv}}(aq)⟶{\text{Al}}_{\text{two}}({\text{S}{\text{O}}_{\mathrm{iv}})}_3(s)+{\text{H}}_2(g)$

(h) ${\text{TiCl}}_{\mathrm{four}}(\mathrm{south})+{\text{H}}_{\mathrm{ii}}\text{O}(g)⟶{\text{TiO}}_2(\mathrm{southward})+\text{HCl}(m)$

5.

Write a counterbalanced molecular equation describing each of the following chemic reactions.

(a) Solid calcium carbonate is heated and decomposes to solid calcium oxide and carbon dioxide gas.

(b) Gaseous butane, C₄H₁₀, reacts with diatomic oxygen gas to yield gaseous carbon dioxide and water vapor.

(c) Aqueous solutions of magnesium chloride and sodium hydroxide react to produce solid magnesium hydroxide and aqueous sodium chloride.

(d) Water vapor reacts with sodium metal to produce solid sodium hydroxide and hydrogen gas.

six .

Write a balanced equation describing each of the following chemical reactions.

(a) Solid potassium chlorate, KClO₃, decomposes to form solid potassium chloride and diatomic oxygen gas.

(b) Solid aluminum metal reacts with solid diatomic iodine to form solid Al_iiI₆.

(c) When solid sodium chloride is added to aqueous sulfuric acid, hydrogen chloride gas and aqueous sodium sulfate are produced.

(d) Aqueous solutions of phosphoric acid and potassium hydroxide react to produce aqueous potassium dihydrogen phosphate and liquid water.

7.

Colorful fireworks oft involve the decomposition of barium nitrate and potassium chlorate and the reaction of the metals magnesium, aluminum, and iron with oxygen.

(a) Write the formulas of barium nitrate and potassium chlorate.

(b) The decomposition of solid potassium chlorate leads to the formation of solid potassium chloride and diatomic oxygen gas. Write an equation for the reaction.

(c) The decomposition of solid barium nitrate leads to the germination of solid barium oxide, diatomic nitrogen gas, and diatomic oxygen gas. Write an equation for the reaction.

(d) Write split up equations for the reactions of the solid metals magnesium, aluminum, and fe with diatomic oxygen gas to yield the respective metal oxides. (Presume the iron oxide contains Fe³⁺ ions.)

8 .

Fill in the bare with a unmarried chemical formula for a covalent compound that volition balance the equation:

9.

Aqueous hydrogen fluoride (hydrofluoric acid) is used to etch glass and to analyze minerals for their silicon content. Hydrogen fluoride will as well react with sand (silicon dioxide).

(a) Write an equation for the reaction of solid silicon dioxide with hydrofluoric acid to yield gaseous silicon tetrafluoride and liquid water.

(b) The mineral fluorite (calcium fluoride) occurs extensively in Illinois. Solid calcium fluoride can likewise be prepared by the reaction of aqueous solutions of calcium chloride and sodium fluoride, yielding aqueous sodium chloride as the other product. Write complete and net ionic equations for this reaction.

10 .

A novel process for obtaining magnesium from sea water involves several reactions. Write a balanced chemical equation for each stride of the process.

(a) The first step is the decomposition of solid calcium carbonate from seashells to class solid calcium oxide and gaseous carbon dioxide.

(b) The 2d step is the formation of solid calcium hydroxide as the merely product from the reaction of the solid calcium oxide with liquid water.

(c) Solid calcium hydroxide is so added to the seawater, reacting with dissolved magnesium chloride to yield solid magnesium hydroxide and aqueous calcium chloride.

(d) The solid magnesium hydroxide is added to a hydrochloric acid solution, producing dissolved magnesium chloride and liquid water.

(e) Finally, the magnesium chloride is melted and electrolyzed to yield liquid magnesium metal and diatomic chlorine gas.

11.

From the counterbalanced molecular equations, write the complete ionic and net ionic equations for the post-obit:

(a) ${\text{Yard}}_2{\text{C}}_{\mathrm{two}}{\text{O}}_4(aq)+\text{Ba}{\text{(OH)}}_2(aq)⟶\mathrm{two}\text{KOH}(aq)+{\text{BaC}}_{\mathrm{two}}{\text{O}}_4(\mathrm{due\; south})$

(b) $\text{Pb}({\text{N}{\text{O}}_3)}_2(aq)+{\text{H}}_2{\text{SO}}_{\mathrm{iv}}(aq)⟶{\text{PbSO}}_4(s)+2{\text{HNO}}_{\mathrm{iii}}(aq)$

(c) ${\text{CaCO}}_3(s)+{\text{H}}_2{\text{SO}}_4(aq)⟶{\text{CaSO}}_{\mathrm{iv}}(\mathrm{southward})+{\text{CO}}_2(k)+{\text{H}}_2\text{O}(l)$

vii.two Classifying Chemic Reactions

12 .

Use the post-obit equations to answer the side by side iv questions:

i. ${\text{H}}_2\text{O}(s)⟶{\text{H}}_{\mathrm{ii}}\text{O}(\mathrm{50})$

ii. ${\text{Na}}^{\text{+}}(aq)+{\text{Cl}}^{\text{−}}(\text{aq})+{\text{Ag}}^{\text{+}}(aq)+{\text{NO}}_{\mathrm{three}}{}^{\text{−}}(aq)⟶\text{AgCl}(\mathrm{southward})+{\text{Na}}^{\text{+}}(aq)+{\text{NO}}_{\mathrm{iii}}{}^{\text{−}}(aq)$

iii. ${\text{CH}}_{\mathrm{iii}}\text{OH}(g)+{\text{O}}_{\mathrm{two}}(g)⟶{\text{CO}}_{\mathrm{two}}(g)+{\text{H}}_2\text{O}(\mathrm{thousand})$

iv. $2{\text{H}}_2\text{O}(l)⟶\mathrm{ii}{\text{H}}_2(\mathrm{yard})+{\text{O}}_{\mathrm{two}}(g)$

v. ${\text{H}}^{\text{+}}(aq)+{\text{OH}}^{\text{−}}(aq)⟶{\text{H}}_{\mathrm{two}}\text{O}(l)$

(a) Which equation describes a physical change?

(b) Which equation identifies the reactants and products of a combustion reaction?

(c) Which equation is not balanced?

(d) Which is a net ionic equation?

13.

Bespeak what type, or types, of reaction each of the following represents:

(a) $\text{Ca}(s)+{\text{Br}}_2(l)⟶{\text{CaBr}}_2(s)$

(b) $\text{Ca}{\text{(OH)}}_2(aq)+2\text{HBr}(aq)⟶{\text{CaBr}}_{\mathrm{ii}}(aq)+\mathrm{ii}{\text{H}}_2\text{O}(l)$

(c) ${\text{C}}_{\mathrm{half\; dozen}}{\text{H}}_{12}(l)+\mathrm{nine}{\text{O}}_{\mathrm{ii}}(g)⟶6{\text{CO}}_2(\mathrm{thousand})+6{\text{H}}_{\mathrm{ii}}\text{O}(\mathrm{thou})$

xiv .

Signal what type, or types, of reaction each of the post-obit represents:

(a) ${\text{H}}_2\text{O}(g)+\text{C}(\mathrm{due\; south})⟶\text{CO}(g)+{\text{H}}_{\mathrm{ii}}(g)$

(b) ${\text{2KClO}}_3(\mathrm{due\; south})⟶\mathrm{two}\text{KCl}(s)+3{\text{O}}_2(\mathrm{yard})$

(c) $\text{Al}{\text{(OH)}}_{\mathrm{iii}}(aq)+3\text{HCl}(aq)⟶{\text{AlCl}}_3(aq)+3{\text{H}}_2\text{O}(\mathrm{fifty})$

(d) $\text{Pb}{({\text{NO}}_3)}_2(aq)+{\text{H}}_2{\text{And so}}_4(aq)⟶{\text{PbSO}}_{\mathrm{iv}}(s)+2{\text{HNO}}_3(aq)$

15.

Silver tin be separated from gold because silver dissolves in nitric acrid while gold does not. Is the dissolution of silver in nitric acid an acid-base reaction or an oxidation-reduction reaction? Explain your answer.

sixteen .

Determine the oxidation states of the elements in the post-obit compounds:

(a) NaI

(b) GdCl₃

(c) LiNO₃

(d) H_twoSe

(e) Mg₂Si

(f) RbO₂, rubidium superoxide

(g) HF

17.

Determine the oxidation states of the elements in the compounds listed. None of the oxygen-containing compounds are peroxides or superoxides.

(a) H_threePO₄

(b) Al(OH)₃

(c) SeO₂

(d) KNO_ii

(e) In_twoS₃

(f) P_ivO_{half dozen}

18 .

Make up one's mind the oxidation states of the elements in the compounds listed. None of the oxygen-containing compounds are peroxides or superoxides.

(a) H₂So₄

(b) Ca(OH)₂

(c) BrOH

(d) ClNO₂

(e) TiCl₄

(f) NaH

19.

Allocate the following as acrid-base reactions or oxidation-reduction reactions:

(a) ${\text{Na}}_2\text{S}(aq)+2\text{HCl}(aq)⟶2\text{NaCl}(aq)+{\text{H}}_{\mathrm{ii}}\text{S}(\mathrm{chiliad})$

(b) $2\text{Na}(s)+\mathrm{ii}\text{HCl}(aq)⟶2\text{NaCl}(aq)+{\text{H}}_2(g)$

(c) $\text{Mg}(\mathrm{southward})+{\text{Cl}}_{\mathrm{ii}}(\mathrm{chiliad})⟶{\text{MgCl}}_2(s)$

(d) $\text{MgO}(\mathrm{southward})+\mathrm{two}\text{HCl}(aq)⟶{\text{MgCl}}_2(aq)+{\text{H}}_2\text{O}(l)$

(due east) ${\text{K}}_3\text{P}(s)+\mathrm{two}{\text{O}}_{\mathrm{ii}}(\mathrm{thousand})⟶{\text{K}}_{\mathrm{three}}{\text{PO}}_4(s)$

(f) $3\text{KOH}(aq)+{\text{H}}_{\mathrm{iii}}{\text{PO}}_4(aq)⟶{\text{K}}_3{\text{PO}}_4(aq)+3{\text{H}}_2\text{O}(\mathrm{50})$

twenty .

Identify the atoms that are oxidized and reduced, the alter in oxidation state for each, and the oxidizing and reducing agents in each of the following equations:

(a) $\text{Mg}(s)+{\text{NiCl}}_2(aq)⟶{\text{MgCl}}_{\mathrm{ii}}(aq)+\text{Ni}(s)$

(b) ${\text{PCl}}_{\mathrm{iii}}(l)+{\text{Cl}}_2(\mathrm{thou})⟶{\text{PCl}}_{\mathrm{v}}(\mathrm{south})$

(c) ${\text{C}}_2{\text{H}}_4(g)+3{\text{O}}_{\mathrm{ii}}(k)⟶2{\text{CO}}_2(\mathrm{one\; thousand})+2{\text{H}}_{\mathrm{ii}}\text{O}(\mathrm{one\; thousand})$

(d) $\text{Zn}(\mathrm{southward})+{\text{H}}_2{\text{SO}}_4(aq)⟶{\text{ZnSO}}_{\mathrm{four}}(aq)+{\text{H}}_{\mathrm{two}}(g)$

(e) $2{\text{K}}_2{\text{Southward}}_2{\text{O}}_3(s)+{\text{I}}_2(s)⟶{\text{K}}_2{\text{S}}_{\mathrm{four}}{\text{O}}_{\mathrm{six}}(s)+2\text{KI}(s)$

(f) $\mathrm{iii}\text{Cu}(\mathrm{due\; south})+8{\text{HNO}}_{\mathrm{iii}}(aq)⟶3\text{Cu}{({\text{NO}}_{\mathrm{three}})}_2(aq)+2\text{NO}(g)+4{\text{H}}_2\text{O}(\mathrm{fifty})$

21.

Complete and remainder the post-obit acid-base of operations equations:

(a) HCl gas reacts with solid Ca(OH)₂(s).

(b) A solution of Sr(OH)₂ is added to a solution of HNO_iii.

22 .

Consummate and balance the following acid-base equations:

(a) A solution of HClO₄ is added to a solution of LiOH.

(b) Aqueous H₂Then_four reacts with NaOH.

(c) Ba(OH)₂ reacts with HF gas.

23.

Consummate and balance the following oxidation-reduction reactions, which give the highest possible oxidation state for the oxidized atoms.

(a) $\text{Al}(\mathrm{south})+{\text{F}}_2(g)⟶$

(b) $\text{Al}(s)+{\text{CuBr}}_2(aq)⟶$ (unmarried displacement)

(c) ${\text{P}}_4(s)+{\text{O}}_{\mathrm{ii}}(\mathrm{yard})⟶$

(d) $\text{Ca}(\mathrm{south})+{\text{H}}_{\mathrm{ii}}\text{O}(l)⟶$ (products are a stiff base and a diatomic gas)

24 .

Complete and balance the following oxidation-reduction reactions, which requite the highest possible oxidation land for the oxidized atoms.

(a) $\text{M}(\mathrm{southward})+{\text{H}}_2\text{O}(\mathrm{50})⟶$

(b) $\text{Ba}(s)+\text{HBr}(aq)⟶$

(c) $\text{Sn}(s)+{\text{I}}_2(\mathrm{due\; south})⟶$

25.

Complete and remainder the equations for the following acid-base neutralization reactions. If water is used as a solvent, write the reactants and products equally aqueous ions. In some cases, there may exist more than than ane correct reply, depending on the amounts of reactants used.

(a) $\text{Mg}{\text{(OH)}}_2(s)+{\text{HClO}}_4(aq)⟶$

(b) ${\text{SO}}_3(\mathrm{chiliad})+{\text{H}}_2\text{O}(l)⟶\text{(presume an backlog of water and that the product dissolves)}$

(c) $\text{SrO}(s)+{\text{H}}_2{\text{So}}_{\mathrm{four}}(l)⟶$

26 .

When heated to 700–800 °C, diamonds, which are pure carbon, are oxidized by atmospheric oxygen. (They burn down!) Write the balanced equation for this reaction.

27.

The military has experimented with lasers that produce very intense lite when fluorine combines explosively with hydrogen. What is the balanced equation for this reaction?

28 .

Write the molecular, full ionic, and net ionic equations for the following reactions:

(a) $\text{Ca}{\text{(OH)}}_2(aq)+{\text{HC}}_{\mathrm{two}}{\text{H}}_3{\text{O}}_{\mathrm{ii}}(aq)⟶$

(b) ${\text{H}}_3{\text{PO}}_4(aq)+{\text{CaCl}}_{\mathrm{ii}}(aq)⟶$

29.

Great Lakes Chemic Company produces bromine, Br₂, from bromide salts such as NaBr, in Arkansas brine past treating the brine with chlorine gas. Write a counterbalanced equation for the reaction of NaBr with Cl_ii.

thirty .

In a mutual experiment in the general chemical science laboratory, magnesium metallic is heated in air to produce MgO. MgO is a white solid, simply in these experiments it oft looks gray, due to small amounts of Mg_iiiN₂, a compound formed as some of the magnesium reacts with nitrogen. Write a balanced equation for each reaction.

31.

Lithium hydroxide may be used to absorb carbon dioxide in enclosed environments, such as manned spacecraft and submarines. Write an equation for the reaction that involves two mol of LiOH per 1 mol of CO_two. (Hint: Water is 1 of the products.)

32 .

Calcium propionate is sometimes added to bread to retard spoilage. This compound tin can be prepared by the reaction of calcium carbonate, CaCO₃, with propionic acrid, C₂H₅CO_iiH, which has properties like to those of acerb acid. Write the balanced equation for the germination of calcium propionate.

33.

Consummate and residue the equations of the following reactions, each of which could be used to remove hydrogen sulfide from natural gas:

(a) $\text{Ca}{(\text{OH})}_2(s)+{\text{H}}_{\mathrm{two}}\text{Due south}(g)⟶$

(b) ${\text{Na}}_{\mathrm{two}}{\text{CO}}_3(aq)+{\text{H}}_2\text{S}(m)⟶$

34 .

Copper(II) sulfide is oxidized by molecular oxygen to produce gaseous sulfur trioxide and solid copper(2) oxide. The gaseous product then reacts with liquid h2o to produce liquid dihydrogen sulfate as the only production. Write the two equations which correspond these reactions.

35.

Write balanced chemical equations for the reactions used to prepare each of the post-obit compounds from the given starting fabric(southward). In some cases, additional reactants may be required.

(a) solid ammonium nitrate from gaseous molecular nitrogen via a two-step process (first reduce the nitrogen to ammonia, then neutralize the ammonia with an advisable acid)

(b) gaseous hydrogen bromide from liquid molecular bromine via a one-step redox reaction

(c) gaseous H₂S from solid Zn and S via a two-step process (start a redox reaction between the starting materials, so reaction of the production with a potent acid)

36 .

Calcium cyclamate Ca(C_viH₁₁NHSO₃)_ii is an artificial sweetener used in many countries around the world simply is banned in the United States. Information technology tin can be purified industrially by converting it to the barium salt through reaction of the acid C_half-dozenH₁₁NHSO₃H with barium carbonate, treatment with sulfuric acid (barium sulfate is very insoluble), and so neutralization with calcium hydroxide. Write the balanced equations for these reactions.

37.

Complete and balance each of the following half-reactions (steps ii–5 in half-reaction method):

(a) ${\text{Sn}}^{\mathrm{4+}}(aq)⟶{\text{Sn}}^{\mathrm{2+}}(aq)$

(b) ${\left[\text{Ag}{({\text{NH}}_3)}_{\mathrm{two}}\right]}^{\text{+}}(aq)⟶\text{Ag}(\mathrm{south})+{\text{NH}}_3(aq)$

(c) ${\text{Hg}}_2{\text{Cl}}_2(s)⟶\text{Hg}(l)+{\text{Cl}}^{\text{−}}(aq)$

(d) ${\text{H}}_2\text{O}(\mathrm{fifty})⟶{\text{O}}_2(g)$ (in acidic solution)

(due east) ${\text{IO}}_{\mathrm{iii}}{}^{\text{−}}(aq)⟶{\text{I}}_2(\mathrm{south})$ (in basic solution)

(f) ${\text{SO}}_3{}^{\mathrm{2-}}(aq)⟶{\text{And so}}_4{}^{\mathrm{2-}}(aq)$ (in acidic solution)

(g) ${\text{MnO}}_{\mathrm{iv}}{}^{\text{−}}(aq)⟶{\text{Mn}}^{\mathrm{2+}}(aq)$ (in acidic solution)

(h) ${\text{Cl}}^{\text{−}}(aq)⟶{\text{ClO}}_{\mathrm{iii}}{}^{\text{−}}(aq)$ (in basic solution)

38 .

Complete and balance each of the post-obit one-half-reactions (steps 2–5 in one-half-reaction method):

(a) ${\text{Cr}}^{\mathrm{2+}}(aq)⟶{\text{Cr}}^{\mathrm{iii+}}(aq)$

(b) $\text{Hg}(l)+{\text{Br}}^{\text{−}}(aq)⟶{\text{HgBr}}_4{}^{\mathrm{2-}}(aq)$

(c) $\text{ZnS}(s)⟶\text{Zn}(s)+{\text{Due south}}^{\mathrm{ii-}}(aq)$

(d) ${\text{H}}_2(\mathrm{grand})⟶{\text{H}}_2\text{O}(l$ (in bones solution)

(e) ${\text{H}}_{\mathrm{ii}}(\mathrm{1000})⟶{\text{H}}_3{\text{O}}^{\text{+}}(aq)$ (in acidic solution)

(f) ${\text{NO}}_{\mathrm{iii}}{}^{\text{−}}(aq)⟶{\text{HNO}}_2(aq)$ (in acidic solution)

(one thousand) ${\text{MnO}}_2(s)⟶{\text{MnO}}_4{}^{\text{−}}(aq)$ (in basic solution)

(h) ${\text{Cl}}^{\text{−}}(aq)⟶{\text{ClO}}_{\mathrm{three}}{}^{\text{−}}(aq)$ (in acidic solution)

39.

Balance each of the post-obit equations according to the half-reaction method:

(a) ${\text{Sn}}^{\mathrm{two+}}(aq)+{\text{Cu}}^{\mathrm{ii+}}(aq)⟶{\text{Sn}}^{\mathrm{4+}}(aq)+{\text{Cu}}^{\text{+}}(aq)$

(b) ${\text{H}}_{\mathrm{two}}\text{S}(\mathrm{chiliad})+{\text{Hg}}_2{}^{\mathrm{ii+}}(aq)⟶\text{H}g(\mathrm{fifty})+\text{South}(s)\text{(in acid)}$

(c) ${\text{CN}}^{\text{−}}(aq)+{\text{ClO}}_2(aq)⟶{\text{CNO}}^{\text{−}}(aq)+{\text{Cl}}^{\text{−}}(aq)\text{(in acid)}$

(d) ${\text{Fe}}^{\mathrm{ii+}}(aq)+{\text{Ce}}^{\mathrm{4+}}(aq)⟶{\text{Fe}}^{\mathrm{iii+}}(aq)+{\text{Ce}}^{\mathrm{3+}}(aq)$

(e) $\text{HBrO}(aq)⟶{\text{Br}}^{\text{−}}(aq)+{\text{O}}_2(g)\text{(in acrid)}$

40 .

Rest each of the following equations according to the half-reaction method:

(a) $\text{Zn}(s)+{\text{NO}}_{\mathrm{iii}}{}^{\text{−}}(aq)⟶{\text{Zn}}^{\mathrm{2+}}(aq)+{\text{N}}_{\mathrm{ii}}(\mathrm{1000})\text{(in acid)}$

(b) $\text{Zn}(\mathrm{south})+{\text{NO}}_{\mathrm{three}}{}^{\text{−}}(aq)⟶{\text{Zn}}^{\mathrm{2+}}(aq)+{\text{NH}}_3(aq)\text{(in base)}$

(c) $\text{CuS}(\mathrm{due\; south})+{\text{NO}}_{\mathrm{three}}{}^{\text{−}}(aq)⟶{\text{Cu}}^{\mathrm{2+}}(aq)+\text{S}(\mathrm{southward})+\text{NO}(g)\text{(in acrid)}$

(d) ${\text{NH}}_3(aq)+{\text{O}}_2(g)⟶{\text{NO}}_{\mathrm{ii}}(\mathrm{thousand})\text{(gas phase)}$

(east) ${\text{H}}_2{\text{O}}_2(aq)+{\text{MnO}}_4{}^{\text{−}}(aq)⟶{\text{Mn}}^{\mathrm{2+}}(aq)+{\text{O}}_{\mathrm{ii}}(g)\text{(in acrid)}$

(f) ${\text{NO}}_2(g)⟶{\text{NO}}_3{}^{\text{−}}(aq)+{\text{NO}}_2{}^{\text{−}}(aq)\text{(in base)}$

(g) ${\text{Fe}}^{\mathrm{iii+}}(aq)+{\text{I}}^{\text{−}}(aq)⟶{\text{Atomic number 26}}^{\mathrm{2+}}(aq)+{\text{I}}_2(aq)$

41.

Rest each of the following equations according to the half-reaction method:

(a) ${\text{MnO}}_4{}^{\text{−}}(aq)+{\text{NO}}_2{}^{\text{−}}(aq)⟶{\text{MnO}}_2(s)+{\text{NO}}_{\mathrm{three}}{}^{\text{−}}(aq)\text{(in base)}$

(b) ${\text{MnO}}_4{}^{\mathrm{2-}}(aq)⟶{\text{MnO}}_4{}^{\text{−}}(aq)+{\text{MnO}}_2(s)\text{(in base)}$

(c) ${\text{Br}}_{\mathrm{two}}(\mathrm{50})+{\text{SO}}_2(g)⟶{\text{Br}}^{\text{−}}(aq)+{\text{SO}}_4{}^{\mathrm{ii-}}(aq)\text{(in acid)}$

seven.3 Reaction Stoichiometry

42 .

Write the balanced equation, then outline the steps necessary to determine the information requested in each of the following:

(a) The number of moles and the mass of chlorine, Cl₂, required to react with 10.0 g of sodium metal, Na, to produce sodium chloride, NaCl.

(b) The number of moles and the mass of oxygen formed past the decomposition of 1.252 g of mercury(Two) oxide.

(c) The number of moles and the mass of sodium nitrate, NaNO_three, required to produce 128 yard of oxygen. (NaNO₂ is the other product.)

(d) The number of moles and the mass of carbon dioxide formed by the combustion of 20.0 kg of carbon in an excess of oxygen.

(e) The number of moles and the mass of copper(Two) carbonate needed to produce 1.500 kg of copper(Two) oxide. (CO_two is the other product.)

(f)

43.

Determine the number of moles and the mass requested for each reaction in Exercise 7.42.

44 .

Write the counterbalanced equation, and then outline the steps necessary to determine the information requested in each of the following:

(a) The number of moles and the mass of Mg required to react with 5.00 g of HCl and produce MgCl_two and H₂.

(b) The number of moles and the mass of oxygen formed by the decomposition of 1.252 k of silverish(I) oxide.

(c) The number of moles and the mass of magnesium carbonate, MgCO_three, required to produce 283 g of carbon dioxide. (MgO is the other product.)

(d) The number of moles and the mass of water formed by the combustion of 20.0 kg of acetylene, C₂H₂, in an excess of oxygen.

(eastward) The number of moles and the mass of barium peroxide, BaO₂, needed to produce 2.500 kg of barium oxide, BaO (O₂ is the other product.)

(f)

45.

Determine the number of moles and the mass requested for each reaction in Exercise vii.44.

46 .

H₂ is produced by the reaction of 118.five mL of a 0.8775-M solution of H₃PO₄ co-ordinate to the post-obit equation: $2\text{Cr}+2{\text{H}}_3{\text{PO}}_4⟶\mathrm{iii}{\text{H}}_2+2{\text{CrPO}}_4.$

(a) Outline the steps necessary to determine the number of moles and mass of H_two.

(b) Perform the calculations outlined.

47.

Gallium chloride is formed past the reaction of 2.6 L of a i.44 Grand solution of HCl according to the following equation: $2\text{Ga}+6\text{HCl}⟶\mathrm{ii}{\text{GaCl}}_3+3{\text{H}}_{\mathrm{ii}}.$

(a) Outline the steps necessary to determine the number of moles and mass of gallium chloride.

(b) Perform the calculations outlined.

48 .

I₂ is produced by the reaction of 0.4235 mol of CuCl₂ according to the following equation: $\mathrm{ii}{\text{CuCl}}_{\mathrm{two}}+4\text{KI}⟶2\text{CuI}+4\text{KCl}+{\text{I}}_{\mathrm{ii}}.$

(a) How many molecules of I_ii are produced?

(b) What mass of I₂ is produced?

49.

Silver is often extracted from ores such equally K[Ag(CN)_ii] and then recovered past the reaction
$2\text{K}\left[\text{Ag}{(\text{CN})}_2\right](aq)+\text{Zn}(s)⟶\text{2Ag}(s)+\text{Zn}{(\text{CN})}_{\mathrm{two}}(aq)+2\text{KCN}(aq)$

(a) How many molecules of Zn(CN)₂ are produced past the reaction of 35.27 grand of K[Ag(CN)₂]?

(b) What mass of Zn(CN)₂ is produced?

50 .

What mass of silver oxide, Ag₂O, is required to produce 25.0 grand of argent sulfadiazine, AgC₁₀H_nineN_fourSo_ii, from the reaction of argent oxide and sulfadiazine?
$2{\text{C}}_{10}{\text{H}}_{10}{\text{North}}_4{\text{SO}}_2+{\text{Ag}}_2\text{O}⟶\mathrm{ii}{\text{AgC}}_{\mathrm{x}}{\text{H}}_9{\text{N}}_{\mathrm{iv}}{\text{SO}}_{\mathrm{ii}}+{\text{H}}_{\mathrm{ii}}\text{O}$

51.

Carborundum is silicon carbide, SiC, a very hard fabric used as an abrasive on sandpaper and in other applications. It is prepared by the reaction of pure sand, SiO_ii, with carbon at high temperature. Carbon monoxide, CO, is the other product of this reaction. Write the balanced equation for the reaction, and calculate how much SiO₂ is required to produce 3.00 kg of SiC.

52 .

Automotive air numberless inflate when a sample of sodium azide, NaN_three, is very rapidly decomposed.
$2{\text{NaN}}_3(s)⟶2\text{Na}(s)+3{\text{N}}_2(\mathrm{thousand})$
What mass of sodium azide is required to produce 2.6 ft^three (73.half-dozen 50) of nitrogen gas with a density of ane.25 g/L?

53.

Urea, CO(NH₂)_two, is manufactured on a big scale for use in producing urea-formaldehyde plastics and equally a fertilizer. What is the maximum mass of urea that can exist manufactured from the CO_two produced by combustion of $1.00\times {10}^{\mathrm{iii}}\text{kg}$ of carbon followed by the reaction?
${\text{CO}}_2(g)+2{\text{NH}}_3(\mathrm{thou})⟶\text{CO}{({\text{NH}}_{\mathrm{two}})}_{\mathrm{ii}}(\mathrm{southward})+{\text{H}}_2\text{O}(l)$

54 .

In an accident, a solution containing 2.5 kg of nitric acid was spilled. 2 kilograms of Na₂CO₃ was quickly spread on the area and CO₂ was released by the reaction. Was sufficient Na₂CO₃ used to neutralize all of the acid?

55.

A compact car gets 37.five miles per gallon on the highway. If gasoline contains 84.2% carbon by mass and has a density of 0.8205 one thousand/mL, make up one's mind the mass of carbon dioxide produced during a 500-mile trip (three.785 liters per gallon).

56 .

What book of 0.750 K hydrochloric acrid solution tin exist prepared from the HCl produced by the reaction of 25.0 grand of NaCl with excess sulfuric acrid?
$\text{NaCl}(s)+{\text{H}}_2{\text{And so}}_4(\mathrm{50})⟶\text{HCl}(g)+{\text{NaHSO}}_4(s)$

57.

What volume of a 0.2089 K KI solution contains enough KI to react exactly with the Cu(NO₃)₂ in 43.88 mL of a 0.3842 Thou solution of Cu(NO_three)₂?
$\mathrm{two}\text{Cu}{({\text{NO}}_{\mathrm{iii}})}_2+\mathrm{four}\text{KI}⟶2\text{CuI}+{\text{I}}_2+4{\text{KNO}}_{\mathrm{three}}$

58 .

A mordant is a substance that combines with a dye to produce a stable fixed color in a dyed fabric. Calcium acetate is used as a mordant. It is prepared past the reaction of acetic acid with calcium hydroxide.
$\mathrm{two}{\text{CH}}_3{\text{CO}}_{\mathrm{ii}}\text{H}+\text{Ca}{\text{(OH)}}_{\mathrm{ii}}⟶\text{Ca}{({\text{CH}}_3{\text{CO}}_2)}_2+2{\text{H}}_{\mathrm{two}}\text{O}$

What mass of Ca(OH)₂ is required to react with the acetic acid in 25.0 mL of a solution having a density of 1.065 grand/mL and containing 58.0% acetic acid by mass?

59.

The toxic pigment called white lead, Pb₃(OH)₂(CO₃)_two, has been replaced in white paints by rutile, TiO₂. How much rutile (g) can be prepared from 379 g of an ore that contains 88.3% ilmenite (FeTiO_iii) by mass?
$2{\text{FeTiO}}_{\mathrm{three}}+4\text{HCl}+{\text{Cl}}_2⟶2{\text{FeCl}}_3+\mathrm{two}{\text{TiO}}_2+\mathrm{two}{\text{H}}_2\text{O}$

7.4 Reaction Yields

lx .

The following quantities are placed in a container: 1.5 $\times$ 10²⁴ atoms of hydrogen, 1.0 mol of sulfur, and 88.0 g of diatomic oxygen.

(a) What is the total mass in grams for the collection of all iii elements?

(b) What is the total number of moles of atoms for the three elements?

(c) If the mixture of the three elements formed a compound with molecules that contain two hydrogen atoms, one sulfur atom, and four oxygen atoms, which substance is consumed first?

(d) How many atoms of each remaining element would remain unreacted in the alter described in (c)?

61.

What is the limiting reactant in a reaction that produces sodium chloride from 8 yard of sodium and viii g of diatomic chlorine?

62 .

Which of the postulates of Dalton's atomic theory explains why nosotros can calculate a theoretical yield for a chemic reaction?

63.

A educatee isolated 25 g of a chemical compound following a procedure that would theoretically yield 81 g. What was his per centum yield?

64 .

A sample of 0.53 one thousand of carbon dioxide was obtained by heating one.31 g of calcium carbonate. What is the percent yield for this reaction?

${\text{CaCO}}_3(s)⟶\text{CaO}(\mathrm{south})+{\text{CO}}_2(s)$

65.

Freon-12, CCl_iiF_ii, is prepared from CCl₄ by reaction with HF. The other product of this reaction is HCl. Outline the steps needed to decide the per centum yield of a reaction that produces 12.v thou of CCl₂F₂ from 32.9 grand of CCl₄. Freon-12 has been banned and is no longer used every bit a refrigerant because it catalyzes the decomposition of ozone and has a very long lifetime in the atmosphere. Determine the percentage yield.

66 .

Citric acrid, C_{half dozen}H₈O₇, a component of jams, jellies, and fruity soft drinks, is prepared industrially via fermentation of sucrose by the mold Aspergillus niger. The equation representing this reaction is
${\text{C}}_{12}{\text{H}}_{22}{\text{O}}_{\mathrm{xi}}+{\text{H}}_{\mathrm{ii}}\text{O}+3{\text{O}}_2⟶\mathrm{ii}{\text{C}}_6{\text{H}}_8{\text{O}}_{\mathrm{vii}}+\mathrm{iv}{\text{H}}_{\mathrm{ii}}\text{O}$

What mass of citric acid is produced from exactly i metric ton (1.000 $\times$ ten³ kg) of sucrose if the yield is 92.30%?

67.

Toluene, C_half-dozenH₅CH_iii, is oxidized by air under advisedly controlled conditions to benzoic acid, C_viH_fiveCO₂H, which is used to prepare the food preservative sodium benzoate, C₆H_vCO₂Na. What is the percent yield of a reaction that converts 1.000 kg of toluene to ane.21 kg of benzoic acid?

$2{\text{C}}_6{\text{H}}_5{\text{CH}}_3+3{\text{O}}_{\mathrm{ii}}⟶\mathrm{two}{\text{C}}_{\mathrm{half-dozen}}{\text{H}}_5{\text{CO}}_2\text{H}+2{\text{H}}_2\text{O}$

68 .

In a laboratory experiment, the reaction of iii.0 mol of H₂ with 2.0 mol of I₂ produced 1.0 mol of HI. Determine the theoretical yield in grams and the per centum yield for this reaction.

69.

Outline the steps needed to solve the following trouble, then do the calculations. Ether, (C₂H₅)₂O, which was originally used as an anesthetic just has been replaced by safer and more than effective medications, is prepared by the reaction of ethanol with sulfuric acid.

2C₂H_vOH + H_iiAnd then_iv ⟶ (C₂H₅)_iiO + H_iiThen₄·H₂O

What is the percent yield of ether if 1.17 Fifty (d = 0.7134 k/mL) is isolated from the reaction of i.500 50 of C_iiH_vOH
(d = 0.7894 g/mL)?

70 .

Outline the steps needed to determine the limiting reactant when 30.0 g of propane, C₃H₈, is burned with 75.0 g of oxygen.

Decide the limiting reactant.

71.

Outline the steps needed to decide the limiting reactant when 0.50 mol of Cr and 0.75 mol of H_threePO₄ react co-ordinate to the following chemical equation.
$2\text{Cr}+2{\text{H}}_3{\text{PO}}_4⟶\mathrm{two}{\text{CrPO}}_{\mathrm{iv}}+3{\text{H}}_{\mathrm{two}}$

Determine the limiting reactant.

72 .

What is the limiting reactant when ane.fifty 1000 of lithium and 1.50 1000 of nitrogen combine to grade lithium nitride, a component of avant-garde batteries, according to the post-obit unbalanced equation?
$\text{Li}+{\text{N}}_{\mathrm{ii}}⟶{\text{Li}}_3\text{N}$

73.

Uranium tin can be isolated from its ores by dissolving it equally UO_ii(NO_iii)₂, then separating it equally solid UO₂(C₂O_four)·3H₂O. Addition of 0.4031 g of sodium oxalate, Na₂C₂O₄, to a solution containing 1.481 g of uranyl nitrate, UO₂(NO₃)₂, yields 1.073 g of solid UO_two(C_twoO₄)·3H_twoO.

Na₂C_iiO₄ + UO₂(NO_iii)_ii + 3H_twoO ⟶ UO₂(C₂O₄)·3H₂O + 2NaNO₃

Determine the limiting reactant and the percent yield of this reaction.

74 .

How many molecules of C₂H₄Cl₂ can be prepared from 15 C₂H_four molecules and eight Cl₂ molecules?

75.

How many molecules of the sweetener saccharin tin exist prepared from 30 C atoms, 25 H atoms, 12 O atoms, 8 S atoms, and xiv N atoms?

76 .

The phosphorus pentoxide used to produce phosphoric acid for cola soft drinks is prepared by called-for phosphorus in oxygen.

(a) What is the limiting reactant when 0.200 mol of P₄ and 0.200 mol of O_two react according to ${\text{P}}_4+5{\text{O}}_2⟶{\text{P}}_4{\text{O}}_{10}$

(b) Calculate the per centum yield if 10.0 grand of P₄O₁₀ is isolated from the reaction.

77.

Would you agree to purchase 1 trillion (1,000,000,000,000) gold atoms for $5? Explicate why or why non. Find the current price of gilt at http://coin.cnn.com/data/commodities/ $(\text{1 troy ounce}=\text{31.1 g})$

seven.v Quantitative Chemical Analysis

78 .

What volume of 0.0105-1000 HBr solution is required to titrate 125 mL of a 0.0100-Grand Ca(OH)₂ solution?
$\text{Ca}{(\text{OH})}_2(aq)+2\text{HBr}(aq)⟶{\text{CaBr}}_2(aq)+2{\text{H}}_2\text{O}(l)$

79.

Titration of a 20.0-mL sample of acid rain required 1.7 mL of 0.0811 G NaOH to reach the stop point. If nosotros assume that the acerbity of the rain is due to the presence of sulfuric acrid, what was the concentration of sulfuric acrid in this sample of rain?

80 .

What is the concentration of NaCl in a solution if titration of fifteen.00 mL of the solution with 0.2503 G AgNO₃ requires 20.22 mL of the AgNO₃ solution to reach the end indicate?
${\text{AgNO}}_3(aq)+\text{NaCl}(aq)⟶\text{AgCl}(\mathrm{due\; south})+{\text{NaNO}}_3(aq)$

81.

In a common medical laboratory decision of the concentration of costless chloride ion in blood serum, a serum sample is titrated with a Hg(NO_three)₂ solution.
$2{\text{Cl}}^{\text{−}}(aq)+\text{Hg}{({\text{NO}}_3)}_{\mathrm{ii}}(aq)⟶\mathrm{two}{\text{NO}}_{\mathrm{iii}}{}^{\text{−}}(aq)+{\text{HgCl}}_2(s)$

What is the Cl⁻ concentration in a 0.25-mL sample of normal serum that requires 1.46 mL of viii.25 $\times$ x⁻⁴ Grand Hg(NO₃)₂(aq) to achieve the end point?

82 .

Potatoes can be peeled commercially past soaking them in a 3-M to 6-G solution of sodium hydroxide, then removing the loosened skins by spraying them with h2o. Does a sodium hydroxide solution have a suitable concentration if titration of 12.00 mL of the solution requires 30.6 mL of 1.65 M HCI to accomplish the cease point?

83.

A sample of gallium bromide, GaBr₃, weighing 0.165 grand was dissolved in h2o and treated with silver nitrate, AgNO₃, resulting in the precipitation of 0.299 grand AgBr. Use these information to compute the %Ga (by mass) GaBr₃.

84 .

The principal component of mothballs is naphthalene, a chemical compound with a molecular mass of virtually 130 amu, containing only carbon and hydrogen. A 3.000-mg sample of naphthalene burns to give 10.3 mg of CO_two. Determine its empirical and molecular formulas.

85.

A 0.025-k sample of a compound equanimous of boron and hydrogen, with a molecular mass of ~28 amu, burns spontaneously when exposed to air, producing 0.063 k of B₂O_three. What are the empirical and molecular formulas of the chemical compound?

86 .

Sodium bicarbonate (baking soda), NaHCO₃, can be purified by dissolving it in hot water (60 °C), filtering to remove insoluble impurities, cooling to 0 °C to precipitate solid NaHCO_three, and so filtering to remove the solid, leaving soluble impurities in solution. Whatever NaHCO₃ that remains in solution is not recovered. The solubility of NaHCO₃ in hot water of lx °C is 164 thousand/L. Its solubility in cold h2o of 0 °C is 69 thousand/L. What is the pct yield of NaHCO_three when it is purified by this method?

87.

What book of 0.600 G HCl is required to react completely with 2.50 g of sodium hydrogen carbonate?
${\text{NaHCO}}_3(aq)+\text{HCl}(aq)⟶\text{NaCl}(aq)+{\text{CO}}_2(k)+{\text{H}}_{\mathrm{two}}\text{O}(l)$

88 .

What volume of 0.08892 M HNO₃ is required to react completely with 0.2352 g of potassium hydrogen phosphate?
$\mathrm{two}{\text{HNO}}_3(aq)+{\text{1000}}_2{\text{HPO}}_4(aq)⟶{\text{H}}_3{\text{PO}}_4(aq)+2{\text{KNO}}_{\mathrm{three}}(aq)$

89.

What volume of a 0.3300-M solution of sodium hydroxide would be required to titrate 15.00 mL of 0.1500 K oxalic acid?
${\text{C}}_{\mathrm{two}}{\text{O}}_4{\text{H}}_2(aq)+2\text{NaOH}(aq)⟶{\text{Na}}_{\mathrm{two}}{\text{C}}_2{\text{O}}_{\mathrm{four}}(aq)+2{\text{H}}_2\text{O}(l)$

90 .

What volume of a 0.00945-1000 solution of potassium hydroxide would be required to titrate 50.00 mL of a sample of acid rain with a H_twoSo_iv concentration of 1.23 $\times$ 10^−iv Yard.
${\text{H}}_2{\text{So}}_4(aq)+\mathrm{two}\text{KOH}(aq)⟶{\text{K}}_{\mathrm{ii}}{\text{SO}}_{\mathrm{iv}}(aq)+2{\text{H}}_2\text{O}(\mathrm{fifty})$

91.

A sample of solid calcium hydroxide, Ca(OH)₂, is allowed to stand in water until a saturated solution is formed. A titration of 75.00 mL of this solution with 5.00 $\times$ x^−two Grand HCl requires 36.6 mL of the acrid to attain the end betoken.
$\text{Ca}{(\text{OH})}_2(aq)+2\text{HCl}(aq)⟶{\text{CaCl}}_2(aq)+2{\text{H}}_2\text{O}(l)$

What is the molarity?

92 .

What mass of Ca(OH)_two will react with 25.0 grand of butanoic to form the preservative calcium butanoate according to the equation?

93.

How many milliliters of a 0.1500-M solution of KOH volition be required to titrate 40.00 mL of a 0.0656-M solution of H₃PO₄?
${\text{H}}_3{\text{PO}}_4(aq)+2\text{KOH}(aq)⟶{\text{G}}_{\mathrm{ii}}{\text{HPO}}_4(aq)+2{\text{H}}_{\mathrm{ii}}\text{O}(l)$

94 .

Potassium hydrogen phthalate, KHC₈H_fourO₄, or KHP, is used in many laboratories, including full general chemistry laboratories, to standardize solutions of base. KHP is one of only a few stable solid acids that tin can be dried by warming and weighed. A 0.3420-one thousand sample of KHC₈H_ivO_iv reacts with 35.73 mL of a NaOH solution in a titration. What is the molar concentration of the NaOH?
${\text{KHC}}_8{\text{H}}_4{\text{O}}_{\mathrm{four}}(aq)+\text{NaOH}(aq)⟶{\text{KNaC}}_8{\text{H}}_{\mathrm{four}}{\text{O}}_4(aq)+{\text{H}}_{\mathrm{ii}}\text{O}(aq)$

95.

The reaction of WCl₆ with Al at ~400 °C gives black crystals of a compound containing only tungsten and chlorine. A sample of this compound, when reduced with hydrogen, gives 0.2232 grand of tungsten metal and hydrogen chloride, which is absorbed in h2o. Titration of the hydrochloric acid thus produced requires 46.2 mL of 0.1051 Chiliad NaOH to reach the end point. What is the empirical formula of the black tungsten chloride?

Naoh Hcl Net Ionic Equation,

Source: https://openstax.org/books/chemistry-atoms-first-2e/pages/7-exercises

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