CHEM 1A Lecture Notes - Lecture 21: Conjugate Acid, Duodecimal, Hydronium

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29 Nov 2016

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UCSB

Department

Chemistry and Biochemistry

Course

CHEM 1A

Professor

Joseph C A

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CHEM 1A Full Course Notes

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Le chatlier"s pri(cid:374)(cid:272)iple: reduce volume of container, t = constant. To alleviate stress, the rxn will shift to the side with fewer moles of gas to reduce the pressure: increase volume. To alleviate stress, the rxn will shift to the side with greater moles of gas to increase the pressure: pressure is how we evaluate where our reaction is. Acids and bases: arrehenius (only with water as solvent) Bases produce oh: bronsted-lowry (any solvent) Hydronium ion: unknown to arrhenius free h+ ions do not exist in water. They covalently react with water to produce hydronium ions, h3o+ Generic acid: ha: a = placeholder. Ha = hcl, hbr, hcn: ha + h20 a- + h30+ Reverse acid: conjugate base = resulting product when h+ is taken off acid, conjugate acid = resulting product when h+ is added to base, ha + h2o a- + h3o+ A- is conjugate base of the acid ha. H3o+ is conjugate acid of the base h2o.

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

CHEM 1A Lecture Notes - Lecture 21: Conjugate Acid, Duodecimal, Hydronium

CHEM 1A Full Course Notes

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