CHEM 1A Lecture Notes - Lecture 10: Analyte, Ionic Compound

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goldclam857

14 Oct 2016

School

UCSB

Department

Chemistry and Biochemistry

Course

CHEM 1A

Professor

Joseph

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CHEM 1A Full Course Notes

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Be careful when you see these things on the product side! Some may undergo another reaction or dangerous gases. Arrhenius defines acid as a substance that when dissolved in water it increases the h+ concentration of the water. Bronsted defines acid as a proton donor. Monoprotic - yields one h atom per molecule of acid. Diprotic yields two h atoms per molecule of acid. Arrhenius defines base as a substance that when dissolved in water increases oh- concentration of water. Bronsted defines base as a proton acceptor. Amphiprotic can react as either an acid or a base. H+ > oh- is an acidic solution. H+ = oh- is a neutral solution. H+ = oh- is a basic solution. Neutralization reactions between an acid and a metal hydroxide produces water and a salt (an ionic compound) Net ionic reaction: h+ (aq) + oh- (aq) -> h2o (l) Analyte: the solution of unknown concentration but known volume.

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 10: Analyte, Ionic Compound

CHEM 1A Full Course Notes

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