CHMA10H3 Lecture Notes - Lecture 15: Lone Pair, Hydronium, Lewis Acids And Bases

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CHMA10H3 Full Course Notes

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Chma10h3 - introductory to chemistry i: structure and bonding lecture 15: hydrogen in water and in the atmosphere. The reaction is called acid-base neutralization: strong acids and bases are strong electrolytes, weak acids and bases are weak electrolytes. Complexation reactions: complexation reactions involve bonding to species with lone pairs. Aquated metal ions: complexation reactions of aquated metal ions are the result of competition between water and other lewis bases to bond with the metal. Solution concentration: the concentration of a solute represents the amount of solute in a specified quantity of solution, amount concentration (morality) is the amount of solute per litre of solution: C = amount of solute (mcl) / volume of solution (l: the concentration of particular species in solution, indicated by the symbol [species]m may be different from the solute concentration. Burning energy questions: the usage of carbon-based fuels as energy sources leads to increased levels of co2 in the atmosphere, fossil fuel reserves are limited.

Related Questions

Please Help. This is a Smart-work question, and requires alllone pairs and radicals to be shown if necessary.

THANKS!!!!!!

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

CHMA10H3 Lecture Notes - Lecture 15: Lone Pair, Hydronium, Lewis Acids And Bases

CHMA10H3 Full Course Notes

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