6. Chemical Quantities & Aqueous Reactions

Complete Ionic Equations

How to Write Complete Ionic Equations and Net Ionic Equations

Which ions remain in solution, unreacted, after each of the 
following pairs of solutions is mixed? 
(c) ammonium phosphate and calcium chloride

Antacids are often used to relieve pain and promote healing
in the treatment of mild ulcers. Write balanced net ionic
equations for the reactions between the aqueous HCl in the
stomach and each of the following substances used in various
antacids: (d) NaAl1CO3)1OH221s2

5.0 &#215; 10&#8722;4M

You have calculated the diluted concentration of Cu2&#43; before complexation occurs.

2.9 &#215; 10&#8722;13M

Correct, complexation reduces the concentration of Cu2&#43; in the solution.

3.7 &#215; 10&#8722;14M

 You may have neglected the dilution factor when the two solutions are mixed. 

2.9 &#215; 10&#8722;16M

 The stoichiometry of the reaction needs to be considered in the equilibrium calculation. 

 Use the formation constant expression for the copper and ammonia complexation reaction. 

When 100.0 mL of a solution that is 0.00100 M in Cu(NO3)2 is mixed with 100 mL of a 0.20 M solution of NH3, what concentration of When 100.0 mL of a solution that is 0.00100 M in Cu(NO3)2 is mixed with 100 mL of a 0.20 M solution of NH3, what concentration of Cu2&#43; remains in solution? remains in solution?

Solution Chemistry and Net Ionic Equations

Predict whether a precipitation reaction will occur when aqueous solutions of the following substances are mixed. For those that form a precipitate, write the net ionic reaction.
(d)

Predict whether a precipitation reaction will occur when aqueous solutions of the following substances are mixed. For those that form a precipitate, write the net ionic reaction.
(b)

Write balanced complete ionic and net ionic equations for each
acid–base reaction.
a. HI(aq) + RbOH(aq)¡

Write balanced complete ionic and net ionic equations for each
reaction.
d. HC2H3O2(aq) + K2CO3(aq)¡ H2O(l ) + CO2( g) + KC2H3O2(aq)

Write balanced net ionic equations for the reactions that occur
in each of the following cases. Identify the spectator ion
or ions in each reaction.
(a) Ba1OH221aq2 + FeCl31aq2¡

Write balanced complete ionic and net ionic equations for each
reaction.
b. NH4Cl(aq) + NaOH(aq)¡H2O(l ) + NH3( g) + NaCl(aq)

Write the balanced molecular and net ionic equations for 
each of the following neutralization reactions: 
(a) Aqueous acetic acid is neutralized by aqueous barium 
hydroxide

A solution contains one or more of the following ions: Hg2
2 + ,
Ba2 + , and Fe2 + . When you add potassium chloride to the solution,
a precipitate forms. The precipitate is filtered off, and you
add potassium sulfate to the remaining solution, producing no
precipitate. When you add potassium carbonate to the remaining
solution, a precipitate forms. Write net ionic equations for the formation
of each of the precipitates observed.

Write balanced molecular and net ionic equations for the
following reactions, and identify the gas formed in each:
(a) solid cadmium sulfide reacts with an aqueous solution of
sulfuric acid

Predict whether a precipitation reaction will occur when aqueous solutions of the following substances are mixed. For those that form a precipitate, write the net ionic reaction.
(a)

Which of the following ions will always be a spectator ion in
a precipitation reaction?
(a) Cl-
(b) NO3-
(c) NH4+
(d) S2-
(e) SO42-

Write balanced complete ionic and net ionic equations for each 
reaction. 
c. NaOH(aq) + HC2H3O2(aq)¡H2O(l ) + NaC2H3O2(aq)

Consider the redox titration (Section 4.13) of 120.0 mL of 0.100 M FeSO4 with 0.120 M K2Cr2O7 at 25 °C, assuming that the pH of the solution is maintained at 2.00 with a suitable buffer. The solution is in contact with a platinum electrode and constitutes one half-cell of an electrochemical cell. The other half-cell is a standard hydrogen electrode. The two half-cells are connected with a wire and a salt bridge, and the progress of the titration is monitored by measuring the cell potential with a voltmeter.
(a) Write a balanced net ionic equation for the titration reaction, assuming that the products are Fe3+ and Cr3+.

The accompanying photo shows the reaction between a 
solution of Cd1NO322 and one of Na2S. (b) What ions remain in solution?

How to Write Total and Net Ionic Equations (Easy)

Write the balanced molecular and net ionic equations for 
each of the following neutralization reactions: 
(c) Aqueous nitric acid and aqueous ammonia react.

Lead(II) ions can be removed from solution by precipitation
with sulfate ions. Suppose that a solution contains lead(II) nitrate.
Write complete ionic and net ionic equations for the reaction
of aqueous lead(II) nitrate with aqueous potassium sulfate
to form solid lead(II) sulfate and aqueous potassium nitrate.

Complete Ionic Equations Example 1

Write a net ionic equation for the reaction that occurs when 10 mL of 0.5 M ammonium carbonate is mixed with 10 mL of 0.5 M silver nitrate. (LO 4.9, 4.11) 
(a) 
(b) 
(c) 
(d) A net ionic reaction cannot be written because a reaction does not take place.

Complete Ionic Equations Example 2

Mercury(I) ions (Hg22 + ) can be removed from solution by precipitation
with Cl - Suppose that a solution contains aqueous
Hg2(NO3)2. Write complete ionic and net ionic equations for
the reaction of aqueous Hg2(NO3)2 with aqueous sodium chloride
to form solid Hg2Cl2 and aqueous sodium nitrate.

TiC2H3O2

Which of the following reagents could be used to separate the two cations from a solution containing Lead (IV) acetate and cesium permanganate?

Citric acid, C6H8O7, is a triprotic acid. It occurs naturally in
citrus fruits like lemons and has applications in food flavouring
and preservatives. A solution containing an unknown
concentration of the acid is titrated with KOH. It requires
23.20 mL of 0.500 M KOH solution to titrate all three acidic
protons in 100.00 mL of the citric acid solution. Write a balanced
net ionic equation for the neutralization reaction.

Write balanced molecular and net ionic equations for the reaction
between nitric acid and calcium hydroxide.

 There are other possibilities based on the given data.  Examine the other choices. 

Ba2&#43; and Mg2&#43;

Ba2&#43;, Mg2&#43; and Na&#43;

Correct, precipitation might indicate the presence of either or Ba2&#43; and Mg2&#43; but the presence of Na&#43; cannot be ruled out.

Ag&#43;, Ba2&#43;, Mg2&#43; and NH4&#43;

Ag&#43; would have produced a precipitation upon the addition of HCl in the first step.

An unknown sample is analyzed using the general qualitative analysis scheme shown in Figure 18.16. The sequence of reagents shown in the figure are used and a precipitate in only produced when (NH4)2HPO4 in NH3 is added. Which of the following describes a set of ions that might be present in the solution?

The reaction of MnO4- with oxalic acid (H2C2O4) in acidic solution, yielding Mn2+ and CO2 gas, is widely used to determine the concentration of permanganate solutions. 
(a) Write a balanced net ionic equation for the reaction.

Write balanced net ionic equations for the following reactions.
(b)

Write balanced net ionic equations for the following reactions.
Note that HClO3 is a strong acid.
(a)

Predict whether a precipitation reaction will occur when aqueous solutions of the following substances are mixed. For those that form a precipitate, write the net ionic reaction.
(c)

Which of the following reagents could be used to separate the two anions from a solution containing magnesium nitrate and cesium hydroxide?

Write balanced complete ionic and net ionic equations for each 
reaction. 
b. MgS(aq) + CuCl2(aq)¡CuS(s) + MgCl2(aq)

Write balanced net ionic equations for the following reactions.
(a)

How To Write Net Ionic Equations In Chemistry - A Simple Method!

Write the balanced molecular and net ionic equations for 
each of the following neutralization reactions: 
(b) Solid chromium(III) hydroxide reacts with nitrous acid.

Write net ionic equations for the reactions listed in Problem 4.73.

Write balanced net ionic equations for the following reactions.
Note that HClO3 is a strong acid.
(b)

Write balanced complete ionic and net ionic equations for each 
acid–base reaction. 
b. HCHO2(aq) + NaOH(aq)¡

Molecular, Complete Ionic, and Net Ionic Equations

Which ions remain in solution, unreacted, after each of the 
following pairs of solutions is mixed? 
(a) potassium carbonate and magnesium sulfate

A solution contains one or more of the following ions: Ag+ ,
Ca2 + , and Cu2 + . When you add sodium chloride to the solution,
no precipitate forms. When you add sodium sulfate to the
solution, a white precipitate forms. You filter off the precipitate
and add sodium carbonate to the remaining solution, producing
another precipitate. Write net ionic equations for the formation of each of the precipitates observed.

(a) Write the net ionic equation for the reaction that occurs 
when a solution of hydrochloric acid (HCl) is mixed with a 
solution of sodium formate 1NaCHO22.

Write net ionic equations for the reactions listed in Problem 4.72.

Because the oxide ion is basic, metal oxides react readily 
with acids. (b) Based on the equation in part (a), write the net ionic 
equation for the reaction that occurs between NiO(s) and an 
aqueous solution of nitric acid.

Net Ionic Equation shows only the ions participating in the chemical reaction, without the spectator ions.

Molecular, Ionic, and Net Ionic Equations

Total Ionic Equation

Write balanced net ionic equations for the reactions that occur 
in each of the following cases. Identify the spectator ion 
or ions in each reaction. 
(c) Na2S1aq2 + CoSO41aq2¡

Write net ionic equations for the reactions that take place when
aqueous solutions of the following substances are mixed:
a. sodium cyanide and nitric acid

Complete and balance the following molecular equations,
and then write the net ionic equation for each:
(b) Cu1OH221s2 + HClO41aq2¡
Write the net ionic equation for it. 

Write balanced molecular and net ionic equations for the reaction
between hydrobromic acid and potassium hydroxide.

The&nbsp;complete ionic equation shows all the aqueous compounds broken up into ions.

Write balanced complete ionic and net ionic equations for each
reaction.
a. HCl(aq) + LiOH(aq)¡H2O(l ) + LiCl(aq)

Provide the net ionic equation that occurs when the following aqueous compounds are mixed together:&nbsp;Copper (II) Bromide and Lithium Hydroxide

Complete Ionic &  Net Ionic Equations

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Clutch Prep

1. Intro to General Chemistry

2. Atoms & Elements

3. Chemical Reactions

4. BONUS: Lab Techniques and Procedures

5. BONUS: Mathematical Operations and Functions

7. Gases

8. Thermochemistry

9. Quantum Mechanics

10. Periodic Properties of the Elements

11. Bonding & Molecular Structure

12. Molecular Shapes & Valence Bond Theory

13. Liquids, Solids & Intermolecular Forces

14. Solutions

15. Chemical Kinetics

16. Chemical Equilibrium

17. Acid and Base Equilibrium

18. Aqueous Equilibrium

19. Chemical Thermodynamics

20. Electrochemistry

21. Nuclear Chemistry

22. Organic Chemistry

23. Chemistry of the Nonmetals

24. Transition Metals and Coordination Compounds

[BOOK CHEM] Clutch Version

Solutions

Solutions represent homogeneous mixtures made of 2 or more components that form a uniform composition.&nbsp;

Osmolarity

Osmolarity (ionic molarity) represents the number of moles of ions per liter of solution.&nbsp;

Gas Evolution Equations

A Gas Evolution Equation is a molecular equation that involves the creation of specific gases.&nbsp;

Molecular Equations

Molecular Equations show reacting molecules involved in a chemical reaction.&nbsp;

Complete Ionic Equations show aqueous compounds as fully dissociated ions.&nbsp;

Solubility Rules

The Solubility Rules are a convenient set of guidelines to help us determine if a compound will be soluble or insoluble.

Molarity

Ever wonder how a mass amount such as moles can be converted into the volume amount of liters? Well, molarity serves as the bridge between moles and liters.&nbsp;

Electrolytes

Electrolytes are compounds that can conduct electricity once they are dissolved in a solvent.&nbsp;

Solution Stoichiometry

Solution Stoichiometry deals with stoichiometric calculations in solutions that involve volume and molarity.

Calculate Oxidation Numbers

Calculating Oxidation Numbers is the first pivotal step in understanding redox reactions.&nbsp;

Dilutions

In Dilutions, a solvent (usually water) is added to a concentrated solution.&nbsp;

Redox Reactions

Redox Reactions (oxidation-reduction reactions) involve transference of an electron(s) between reactants.

Activity Series

Activity Series is a list of single displacement reactions in order of reactivity.

Balancing Redox Reactions: Acidic Solutions

Balancing Redox Reactions requires a new approach that accounts for the transfer of electrons between reactants.

Balancing Redox Reactions: Basic Solutions

Balancing Basic Redox Reactions requires all the same steps as balancing in an acidic solution plus an additional step.