CHEM 112 Lecture Notes - Nitric Acid, Strontium Hydroxide, Colligative Properties

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29 Jan 2014

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Bronsted lowry acid and bases: acid is a proton (hydrogen ion) donor, base is a proton acceptor, however febr3, alcl3, zncl2 bf3, ch4 are all acids (see lewis acids later) ***slide 8: arrows should be reversed**: electrons always move towards the deficit of electron densities. Ionization constant: water is not used in calculation, no units; dimensionless, k = [reactants: ka or kb for acids and bases respectively. Self-ionozation (autoionization) of water: contains very low concentration of ions because of its amphiphrotic nature, amphiprotic means it can act as a base or an acid, depending on other reactants, kw for water, kw = 1. 0 x 10-14. To predict direction of acid-base reaction: cross out spectator ions. Identify each species as acid or base: use the table to identify which one is the acting or stronger acid and base, reaction favors the side of the weaker acid. P operator refers to :take negative log of what follows poh = -log[oh]

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Concepts and reason

The concept used to solve this problem is determined the Conjugated acid-Base.

Fundamentals

Bronsted-Lowry acid-base system:

Acid:

According to Bronsted-Lowry; acid is a substance that donates the (hydrogen ion) or proton. In general Bronsted-Lowry acid is a proton donor.

Base:

According to Bronsted-Lowry; base is a substance that accepts the (hydrogen ion) or proton. In general Bronsted-Lowry base is a proton acceptor.

HCI + NH, NH +CI
Acid base

Conjugated acid-Base Pairs:

The pair of Acid-Base which is differs by a proton is called conjugated Acid-Base pair. The acid of conjugated acid-base pair has one more hydrogen atom from base of conjugated acid-base pair.

HCI+NH,
Acid base
NH + CI
conjugated acid conjugated base

After donate one proton from an acid conjugate base will form; thus, is the conjugate base of .

HIO, +H* + 10
Acid conjugated base

After accepts one proton by a base conjugate acid will form; thus is the conjugate acid of .

H* +02- → OH
base conjugated acid

FIRST STEP | ALL STEPS | ANSWER ONLY

Step-by-step

Step 1 of 4

Part a

The conjugate acid of H,PO, will from after accept one proton by H,PO, as follows:

H,PO,+H* H,PO,

After donate one proton from an acid conjugate base will form and after accepts one proton by a base conjugate acid will form.

Explanation | Hint for next step

The pair of Acid-Base which is differs by a proton is called conjugated Acid-Base pair. The acid of conjugated acid-base pair has one more hydrogen atom from base of conjugated acid-base pair.

Step 2 of 4

The conjugate acid of will from after accept one proton by as follows:

Base Conjugate acid

Part a

The conjugate acid of H,PO, is H,PO, .

Explanation

The pair of Acid-Base which is differs by a proton is called conjugated Acid-Base pair. The acid of conjugated acid-base pair has one more hydrogen atom from base of conjugated acid-base pair.

Step 3 of 4

Part b

The conjugate base of HSO, will from after donate one proton from HSO, as follows:

HSO, → S0+H*

Explanation | Hint for next step

The pair of Acid-Base which is differs by a proton is called conjugated Acid-Base pair. The acid of conjugated acid-base pair has one more hydrogen atom from base of conjugated acid-base pair.

Step 4 of 4

The conjugate base of will from after donate one proton from as follows:

Acid Conjugate base

Part b

The conjugate base of HSO, is .

Explanation | Common mistakes

The pair of Acid-Base which is differs by a proton is called conjugated Acid-Base pair. The acid of conjugated acid-base pair has one more hydrogen atom from base of conjugated acid-base pair.

Answer

Part a

The conjugate acid of H,PO, is H,PO, .

Part b

The conjugate base of HSO, is .

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The conjugate acid of HPO42- is H2PO4 H3PO4 PO43- PO42- H2PO4-

Question 2 1) What is the conjugate base of HCO3−? Express your answer as a chemical formula. 2) What is the conjugate acid of HPO32− ? Express your answer as a chemical formula. 3) Among three bases, X−, Y−, and Z−, the strongest one is Y−, and the weakest one is Z−. Rank their conjugate acids, HX, HY, and HZ, in order of decreasing strength. Rank the acids from strongest to...

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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 112 Lecture Notes - Nitric Acid, Strontium Hydroxide, Colligative Properties

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