CHEM 1210 Lecture Notes - Lecture 12: Sodium Hydroxide, Strong Electrolyte, Lithium Hydroxide

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sapphiremoose590

17 Sep 2018

School

Ohio State University

Department

Chemistry

Course

CHEM 1210

Professor

Shiyu Zhang

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CHEM 1210 Lecture Notes - Lecture 4: Lead, Mass Spectrometry, Sodium Sulfate

CHEM 1210 Lecture Notes - Lecture 12: Sodium Hydroxide, Strong Electrolyte, Lithium Hydroxide

CHEM 1210 Lecture Notes - Fall 2018 Lecture 13 - Chemical equation, Spectator ion, Sodium hydroxide

9/17

Precipitation reactions and particle representations continued

Arrhenius:

● Figured dissociation of ions (in A solution)(won a Nobel prize for his work)

● Interested in global temperature and CO2 levels—> this lead to the discovery of the

greenhouse effect down the road.

All ionic compounds produce ions in the extent to which they dissolve

No molecules are present

Not all ionic compounds are highly soluble in water, however this is different than a weak

electrolyte

Electrolytes and nonelectrolytes:

● Strong electrolytes: ions are produced when in a solution. No molecules when dissolved

in water

○ Ionic (No metal to metal) compounds are the most common strong electrolytes

○ Strong acids and strong bases are most often strong electrolytes

● Weak electrolytes: mostly exist as molecules in solution. Some ions are produced when

dissolved in water.

○ Weak acids and bases are most often weak electrolytes

● Nonelectrolytes: no ions are produced in solution

Precipitation reactions:

● A precipitation reaction yields a precipitate

○ Precipitate is an insoluble solid formed by a reaction in a solution

● By referring to table 4.1(in book or on note slides) it can be predicted from the beginning

of a reaction if a precipitate will be formed or not.

○ Examples: Does a precipitate form?

■ NaNO3+K2SO4 —> no precipitate (there are no exceptions that would

mean a precipitate forming based off of table 4.1)

■ NaOH+KCl —> no precipitate

■ AgNO3+NH4I —> precipitate

○ Table 4.1 is expected to be memorized for the exam

● Most common form is a Metathesis reaction/ exchange reaction/ double displacement

○ They are all the same thing

○ Metathesis is from Greek to mean putting in different order

○ Form: Ax+By—>Ay+Bx

● The end goal with this type of reaction is to find the net ionic equation (this is different

than the molecular equation)

● Steps to get to the net ionic equation:

○ Break apart all of the aqueous compounds into ions

○ Keep solids/precipitate as it is

○ Cancel out spectator ions (these go through the reaction unchanged) (they

appear the same on both sides)

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Related Questions

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.

indigolouse566

QUESTION 1

Which of the following substances is most acidic?

		Cowâs milk - pH 6.6
		Apple juice - pH 3.0
		Tomato juice - pH 4.5
		Distilled water - pH 7.0

2 points

QUESTION 2

A buffer is a substance that converts:

Alkaline solutions to neutral solutions.

Acidic solutions to alkaline solutions.

Strong bases or acids to weak bases or acids.

Acidic solutions to neutral solutions.

QUESTION 3

How does a solution of pH 7 compare to a solution of pH 10?

		pH 7 has more OH^- ions
		pH 7 is more basic
		pH 7 has a higher pH
		pH 7 has more H⁺ ions

2 points

QUESTION 4

According to the Arrhenius Theory of acids and bases, a base is:

A substance that decrease the amount of hydroxide ions present.

A substance that increases the amount of hydroxide ions present when it is dissolved in water.

A substance that increase the amount of hydrogen ions present.

A substance that increases the amount of hydrogen ions present when it is dissolved in water.

QUESTION 5

Which of the following are true regarding acid-base titrations?

		They are used to determine the concentration of an unknown acid or base.
		The acid or the base must be a standard solution with a known concentration
		The standard solution is titrated into the chemical with the unknown concentration.
		All of the above are true regarding acid-base titrations.

2 points

QUESTION 6

Which of the following is not an example of a neutralization reaction?

HCl + NaOH NaCl +H₂O

2 NaOH + H₂CO₃ Na₂CO₃ +2 H₂O

H₂SO₄ + 2 NH₄OH (NH₄)₂SO₄ + 2 H₂O

2 AgNO₃ + Zn 2Ag +Zn(NO₃)₂

QUESTION 7

Which acid base theory defines an acid as a proton donor and a base as a proton acceptor?

		Arrhenius Theory
		Bronsted-Lowery Theory
		Conjugate Pairs Theory
		Lewis Theory

2 points

QUESTION 8

The Arrhenius Theory states that acid-base reactions create a solution composed of a water and a salt. This is because mixing an acidic and basic solution together yields:

A neutral solution

A solution with a pH at or near 7

Both A and B are correct

QUESTION 9

Which of the following correctly defines a standard solution?

		A solution which always has the same molecular geometry.
		A solution in which the concentration is precisely known.
		A solution in which the volume is precisely known.
		A solution which always has different levels of solutes and solvents.

2 points

QUESTION 10

Acids naturally present in food are generally safe to eat because they are usually:

		Concentrated
		Dilute
		Weak
		Strong

None of the above are correct

CHEM 1210 Lecture Notes - Lecture 12: Sodium Hydroxide, Strong Electrolyte, Lithium Hydroxide

CHEM 1210 Lecture Notes - Lecture 4: Lead, Mass Spectrometry, Sodium Sulfate

CHEM 1210 Lecture Notes - Lecture 12: Sodium Hydroxide, Strong Electrolyte, Lithium Hydroxide

CHEM 1210 Lecture Notes - Fall 2018 Lecture 13 - Chemical equation, Spectator ion, Sodium hydroxide

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