CHEM 1127Q Lecture Notes - Lecture 9: Chemical Equation, Solution, Chlorate

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tealkoala495

1 Mar 2019

School

UConn

Department

Chemistry

Course

CHEM 1127Q

Professor

Dr. Niluka Wasalathanthri

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CHEM 1127Q Full Course Notes

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A precipitation reaction is one in which dissolved substances react to form one or more solid products. A compound is soluble in a particular liquid if it dissolves in that liquid. A compound is insoluble if it does not dissolve in the liquid. An aqueous solution is a homogenous mixture of a substance with water. When ionic compounds dissolve in water, they usually dissociate into their component ions. Group 1 metal cations and ammonium ion. Halides of ag+, hg2 2+, and pb 2+ Sulfates of ag+, ba2+, ca2+, hg2 2+, pb 2+, sr2+ Compounds of these anions with group 1 metal cations and ammonium anion. Hydroxides of group 1 metal cations and ba2+ A molecular equation is an equation showing the complete neutral formulas for every compound in the reaction. Complete ionic equations show aqueous ionic compounds that normally dissociate in solution as they are actually present in solution.

Related Questions

The nitrate ion, NO3-, is in a separate group from the anions used in todayâs experiment. The groups are listed below. Suggest a reason why the procedure used today would make the determination of the nitrate ion difficult.

1. Group I: the sulfate group. This group is named the same as the sulfate ion but it also contains other âate ions, like carbonate (CO₃^2â) and phosphate (PO₄^3â). These anions selectively react with Ba²⁺ cation (or other alkaline earth metal cations like Ca²⁺) under basic conditions (eg. ammonia solution) and generate precipitations. The reaction can be either reversible or irreversible depends on the chemical property of the precipitation.

2. Group II: the halide group. This group includes or the halides and sulfide (S^2â). These anions can react with Ag⁺ cation under acidic or neutral conditions. The reaction usually generates very insoluble and chemically stable precipitation.

3. Group III: the nitrate group. The nitrate (NO₃^â) anion forms water soluble salt with all the common cations.

The Behavior of Substances in Water

Part 1:

Ammonia, NH₃, is a weak electrolyte. It forms ions in solution by reacting with water molecules to form the ammonium ion and hydroxide ion. Write the balanced chemical reaction for this process, including state symbols.
From everyday experience, you are probably aware that table sugar (sucrose), C₁₂H₂₂O₁₁, is soluble in water. When sucrose dissolves in water, it doesn’t form ions through any reaction with water. It just dissolves without forming ions, so it is a nonelectrolyte. Write the chemical equation for the dissolving of sucrose in water.
Both NH₃ and C₁₂H₂₂O₁₁ are soluble molecular compounds, yet they behave differently in an aqueous solution. Briefly explain why one is a weak electrolyte and the other is a nonelectrolyte.
Hydrochloric acid, HCl, is a molecular compound that is a strong electrolyte. Write the chemical reaction of HCl with water.
Compare the ammonia reaction with that of hydrochloric acid. Why are both of these substances considered electrolytes?
Explain why HCl is a strong electrolyte and ammonia is a weak electrolyte.
Classify each of the following substances as either ionic or molecular:

KCl
NH₃
CO₂
MgBr₂
HCl
Ca(OH)₂
PbS
HC₂H₃O₂

For those compounds above that, you classified as ionic, use the solubility rules to determine which are soluble.
The majority of ionic substances are solids at room temperature. Describe what you would observe if you placed a soluble ionic compound and an insoluble ionic compound in separate beakers of water.
Write the chemical equation(s), including state symbols, for what happens when each soluble ionic compound that you identified above is placed in water. Are these substances reacting with water when they are added to water?
How would you classify the soluble ionic compounds: strong electrolyte, weak electrolyte, or nonelectrolyte? Explain your answer.
Sodium chloride, NaCl, is a strong electrolyte, as is hydroiodic acid, HI. Write the chemical equations for what happens when these substances are added to water. m
Are NaCl and HI strong electrolytes because they have similar behavior in an aqueous solution? If not, describe, using words and equations, the different chemical process that takes place in each case.

Part 2:

You have two hypothetical molecular compounds, AX and AY. AX is a strong electrolyte and AY is a weak electrolyte. The compounds undergo the following chemical reactions when added to water.

AX (aq) + H₂O (l) → AH₂O⁺ (aq) + X⁻ (aq)

AY (aq) + H₂O (l) → AH₂O⁺ (aq) + Y⁻ (aq)

Explain how the relative amounts of AX ( aq ) and AY ( aq ) would compare if you had a beaker of water with AX and a beaker of water with AY.
How would the relative amounts of X⁻ ( aq) and Y⁻ ( aq) in the two beakers compare? Be sure to explain your answer.

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CHEM 1127Q Lecture Notes - Lecture 9: Chemical Equation, Solution, Chlorate

CHEM 1127Q Full Course Notes

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