Acids and Bases

Strong vs. Weak Acids & Bases

Strong acids and bases COMPLETELY disassociate in solution.

Weak acids and bases dissassociate less than 5%

Multiple Choice

Acids which dissociate almost completely in aqueous solutions are known as:

• Dilute acids

• Strong acids

• Weak acids

• Concentrated acids

Multiple Choice

A substance that does not dissociate completely. Ranges from 4-7 on the pH scale.

• Strong Acid

• Strong Base

• Weak Acid

• Weak Base

Multiple Select

When comparing a strong and weak acid of the same concentration, the strong acid will have...(choose 2 answers)

• A higher conductivity

• A lower conductivity

• A faster rate of reaction

• A slower rate of reaction

Multiple Select

When comparing a strong and weak acid of the same concentration, the strong acid will have...(choose 2 answers)

• A higher pH

• A lower pH

• a smaller temperature change on neutralisation with a strong base

• a bigger temperature change on neutralisation with a strong base

Multiple Choice

What are the formulas for the following?
--hydrochloric acid--
--hydrobromic acid--
--hydroiodic acid--

• HClO₃, HBrO₃, HIO₃

• HCl, HBr, HI

• HClO₄, HBrO₄, HIO₄

• HClO, HBrO, HIO

Multiple Choice

Ammonia has a pH of 12.  Ammonia is __________.

• an acid

• a base

• an element

• a metal

Multiple Choice

Which of these solutions is an acid?

• Dish Soap: pH of 12

• Tomato Soup: pH of 4

• Baking Soda: pH of 9

• Drain Cleaner: pH of 14

Multiple Choice

What does a pH of 1 indicate about a liquid?

• it is a very strong base

• it is a weak base 

• it is a weak acid

• it is a strong acid

Match

Match each pH with the correct category:

• strong acid

• strong base

• weak acid

• weak base

• neutral

1.0

13.5

5.5

8.5

7.0

• 1.0

• 13.5

• 5.5

• 8.5

• 7.0

Drag and Drop

Acids form​

Placeholder

when mixed with water, and they taste ​

Placeholder

.

Bases form ​

Placeholder

when mixed with water, and they taste ​

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.

Drag these tiles and drop them in the correct blank above

H+

sour

OH-

bitter

Electrolytes

Can be 3 things

- Acids (strong and weak)

- Bases ( Strong and weak)

- Salts (metal + nonmetal)

Disassociate in water.

NONelectrolytes do not.

Multiple Choice

Which of the following word pairs correctly completes the sentence below?
_______ are corrosive substances characterized as having a strong smell, a sour taste, and a _______.

• Acids; pH less than 7

• Acids; pH greater than 7

• Bases; pH greater than 7

• Bases; pH less than 7

Multiple Choice

What is the conjugate acid of HCO₃^1-?

Hint: charge of -1 so lost a proton (+1) so needs to get a proton back

• CO₃

• H₂CO₃

• CO₃^2-

• H₂CO₃^2-

Multiple Choice

Which two species would be identified as Bronsted-Lowry bases?

• HF and F^-

• NH₃ and F^-

• NH₃ and NH₄⁺

• NH₄⁺ and F^-

Multiple Choice

What is the conjugate base of HClO₄?

• H⁺

• Cl^-

• ClO₃^-

• ClO₄^-

Match

Match the following

H₂CO₃ (aq) + H₂O (l) <--> H₃O⁺ (aq) + HCO₃^-- (aq)

• H₂CO₃

• H₂O

• H₃O⁺

• HCO₃^--

Bronsted-Lowry

Acid

Bronsted- Lowry

Base

Conjugate Acid

Conjugate Base

• Bronsted-Lowry

  Acid

• Bronsted- Lowry

  Base

• Conjugate Acid

• Conjugate Base

Multiple Select

Check all that apply: According to the Arrhenius definition:

• An acid contains H and releases H⁺ ions in solution

• An acid contains OH and releases OH^- in solution

• A base contains OH and releases OH^- in solution

• A base contains H and releases H⁺ ions in solution

​Strength vs Concentration

Experience. Chemistry | Lesson 13.2

• Two factors contribute to the pH of a solution

  • Strength-how much the acid ionizes

    • Stronger acids will have a lower pH than weak acids in the same amounts

  • Concentration: How many moles there are of the acid

    • A high concentration will have a low pH​

Multiple Choice

Strong acids and bases...

• do not break apart into ions (non-electrolyte)

• partially break apart into ions (weak electrolyte)

• completely break apart into ions (non-electrolyte)

• completely break apart into ions (strong electrolyte)

Multiple Choice

Which is the stronger acid?

• pH 1

• pH 4

• pH 8

• pH 13

Multiple Choice

If an acid is combined with a base of equal strength, the result will most likely be

• a neutral solution.

• a stronger acid.

• impossible to tell without testing the pH.

• a stronger base

Multiple Choice

Which of the following is a base?

• orange juice

• water

• vinegar

• dishwashing detergent

Multiple Choice

 Which of the following is an acid?

• shampoo

• baking soda

• orange juice

• water

Multiple Choice

Pure water has a pH of 7. Pure water _______.

• is a base

• is a neutral substance

• could be either an acid or a base

• is an acid

Multiple Choice

Which type of ion does a base produce when it is dissolved in water?

• oxide

• oxygen

• hydrogen

• hydroxide

Multiple Choice

Which of the following is true about acids and bases?

• The lower the pH, the stronger the acid

• the higher the pH, the stronger the acid

• The lower the pH, the more neutral the acid

• The higher the pH, the weaker the base

Multiple Choice

Explain what happens when a strong acid and a strong base are poured into the same container.

• they form separate layers

• they mix physically but not chemically

• they break apart into separate elements

• they react chemically to form a salt

Multiple Choice

On the pH scale what numbers are bases?

• 8-14

• 0-7

• 7

• 1

Multiple Choice

On the pH scale what numbers are acids?

• 8-14

• 0-7

• 7

• 1

Multiple Choice

On the pH scale what numbers are neutrals?

• 8-14

• 0-7

• 7

• 1

Multiple Choice

The pH scale measures...

• ...the strength of an acid.

• ...the strength of hydrogen ions.

• ...the concentration of hydrogen ions.

• ...the concentration of an acid

Multiple Choice

Which of the following word pairs correctly completes the sentence below?

_______ are corrosive substances characterized as having a oily feel, a bitter taste, and a _______.

• Acids; pH less than 7

• Acids; pH greater than 7

• Bases; pH greater than 7

• Bases; pH less than 7

Multiple Choice

Which type of ion does an acid produce when it is dissolved in water?

• oxide

• oxygen

• hydronium

• hydroxide

Multiple Choice

When an equal strength acid and base are mixed, what kind of chemical reaction occurs?

• Neutralization

• Combustion

• Oxdation

• Decomposition

Multiple Choice

A substance is found to have the following characteristics:

Very bitter taste

Feels slippery to the touch

Produces OH- ions when dissolved in water

In what category would the substance be classified?

• acid

• base

• enzyme

• fatty acid

Multiple Choice

HF is...

• an acid

• a base

• a salt

• an ionic compound

Multiple Choice

HNO₂

• a base

• a salt

• an acid

• an ionic compound

Multiple Choice

Releases hydrogen in an aqueous solution.

• base

• strong base

• acid

• weak base

Multiple Choice

KOH is ...

• an acid

• a base

• a salt

• an ionic compound

Multiple Choice

An arrhenius acid

• produces hydroxide ions in a solution

• is a proton donor

• produces hydrogen ions in a solution

• is a proton acceptor

Multiple Choice

An arrhenius base

• produces hydroxide ions in a solution

• is a proton donor

• produces hydrogen ions in a solution

• is a proton acceptor

Multiple Choice

A bronsted lowry base

• produces hydroxide ions in a solution

• is a proton donor

• produces hydrogen ions in a solution

• is a proton acceptor

Multiple Choice

A bronsted lowry acid

• produces hydroxide ions in a solution

• is a proton donor

• produces hydrogen ions in a solution

• is a proton acceptor

Multiple Choice

Identify the true statement about the following reaction:

F^- + H₂O --> HF +OH^-

• H₂O is a bronsted lowry base

• H₂O is not an acid or base according to either model

• H₂O is a bronsted lowry acid

• H₂O is an arrhenius acid

Multiple Choice

Acid-base conjugate pairs differ by a single

• Electron

• Proton

• Neutron

• Oxygen

Multiple Choice

Which of the following show an acid and its conjugate base pair (in that order)

• H₂SO₄, SO₄^2-

• OH^-, H₂O

• NH₄⁺, H₂O

• H₂CO₃, HCO₃^-