CHM 142 Lecture Notes - Lone Pair, Conjugate Acid, Acid Strength

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crimsonchimpanzee229

7 Aug 2013

School

Miami University

Department

Chemistry & Biochemistry

Course

CHM 142

Professor

Dr.James D.Garrity

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Document Summary

Arrhenius definition molecules that dissociate in water to yield. Arrhenius definition molecules which dissociate in water to yield. All bronsted-lowry acids are arrhenius acids: with arrhenius, proton acceptor must be water. Bronsted-lowry expands definition of bases beyond metal hydroxides (ex. Strong acid completely ionized in water (technically, never true. Equilibrium constant (k) is called ka, the acid dissociation constant. Any molecule with a donateable h+ is a potential acid; any molecule with a lone pair is a potential base. Conjugate acid-base pairs differ from each other only by the presence of the h+ ion. The stronger an acid is, the weaker its conjugate base is. Strong base hydroxide or oxide of group i or ii metals. Amphiprotic/amphoteric capable of acting as a bronsted-lowry acid or base. (can donate or accept a proton). (ex. 14= ph + poh px = -log[x]

Related Questions

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

CHM 142 Lecture Notes - Lone Pair, Conjugate Acid, Acid Strength

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