CHEM 110 Lecture Notes - Protein Structure, Chemical Polarity, Acid Dissociation Constant

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Legend: water has no buffer capacity-that is, its ph changes sharply when even small quantities. 17. 1-common-ion effect in acid-base equilibria: when the concentrations of acid and base in a buffer solution are equal, [h3o+] =ka and ph=pka, when there is more acid than base, [h3o+] > ka and ph < pka. Solution of weak acids & their salts: salt of a weak acid is a strong electrolyte-its ions become completely dissociated from one another in aqueous solution h2o. Acid-base properties of salt solutions: a salt is an ionic compound that is produced when a cation and an anion from an acid-base reaction combine. In other words, the cation from a base replaces a proton on an acid: a simple example is the reaction of the strong base naoh with the strong acid hcl. In solution, the and ions react to form h2o, leaving a solution of salt ions, na+and cl-.

Related Questions

Can someone answer number 5

Buffers are:

a) a mixture of weak acids or bases and their salts.

b) chosen so that the desired pH is within 2 pH units of the pKa of the acid.

c) solutions that resists changes in pH, regardless of amount of acid or base added to the buffer.

d) best made by titrating the weak acid to its equivalence point.

e) measured with a pH meter that has been previously calibrated with water.

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 110 Lecture Notes - Protein Structure, Chemical Polarity, Acid Dissociation Constant

CHEM 110 Full Course Notes

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