Buffers

Presentation

•

Chemistry

•

12th Grade

•

Practice Problem

•

Medium

MERLIE WASAWAS

Used 7+ times

FREE Resource

15 Slides • 19 Questions

Multiple Choice

What is the normal pH range of the human blood?

7.25-8.0

3.30-3.45

7.3 - 7.45

7.0-7.25

Multiple Choice

What will happen to the pH of the blood if there is a higher concentration of carbon dioxide? It will become...

More acidic

More alkaline

Neutral

Buffer

Multiple Choice

To maintain the pH of the blood to 7.3 - 7.45, which of the following will happen if there is an excess of OH^-?

HCO₃^– + H⁺ $\rightarrow$ H₂CO₃

H₂CO₃ + OH $\rightarrow$ HCO₃^–+ H₂O

H₂CO₃ $\rightarrow$ CO₂ + H₂O

CO₂ + H₂O $\rightarrow$ H₂CO₃

REVIEW

Multiple Choice

What do you call the product that will be formed after a base accepts H⁺?

Bronsted acid

Bronsted base

Conjugate base

Conjugate acid

Multiple Choice

What do you call the product that will be formed after an acid loses H⁺?

Bronsted acid

Bronsted base

Conjugate base

Conjugate acid

Multiple Choice

Which of the following is not TRUE about buffers?

it contains a weak acid and its

conjugate base

it can absorb excess H⁺ ions or OH^– ions

maintaining an overall steady pH

it is formed when a proton is removed from an acid

Multiple Choice

How can a buffer maintain the pH of a solution when acid is added?

the conjugate base of the buffer neutralizes the acid

the conjugate base of the buffer neutralizes the base

the conjugate acid of the buffer neutralizes the base added

the conjugate acid of the buffer neutralizes the base acid

Multiple Choice

How can a buffer maintain the pH of a solution when acid is added?

the conjugate base of the buffer neutralizes the acid

the conjugate base of the buffer neutralizes the base

the conjugate acid of the buffer neutralizes the base added

the conjugate acid of the buffer neutralizes the base acid

Multiple Choice

How can a buffer maintain the pH when base is added to the solution?

the conjugate base of the buffer neutralizes the acid added

the conjugate base of the buffer neutralizes the base added

the conjugate acid of the buffer neutralizes the base added

the conjugate acid of the buffer neutralizes the acid added

Multiple Choice

Which equation is used calculate the specific pH of a given buffer?

Henderson-Hasselbalch

Lowry-Bronsted

Arrhenius

Henderson-Hasslebalch

Match

Match the following.

the concentration of [H⁺]

the "dissociation constant" for the weak acid

the concentration of conjugate base

the concentration of the weak acid

K_a

[A^-]

[HA]

Multiple Choice

To calculate the specific pH of a given buffer, you need to use the Henderson-Hasselbalch equation for acidic buffers:

𝑝𝐾_𝑎 + 𝑙𝑜𝑔 $\frac{\left[A^-\right]}{\left[HA\right]}$

𝑝𝐾_𝑎 + 𝑙𝑜𝑔 $\frac{\left[B^+\right]}{\left[BOH\right]}$

𝑝𝐾_𝑎 + 𝑙𝑜𝑔 $\frac{\left[conjugate\ acid\right]}{\left[weak\ base\right]}$

-logK_a

Match

Match the following.

the concentration of [H⁺]

the "dissociation constant" for the weak base

the concentration of conjugate acid

the concentration of the weak base

K_b

[A⁺]

[BOH]

Fill in the Blanks

Type answer...

Fill in the Blanks

Type answer...

EVALUATION

Multiple Choice

A buffer is an aqueous solution consisting of a mixture of a weak acid and its conjugate base, or vice versa.

True

False

Multiple Choice

A conjugate acid is a species formed by the gain of a proton by a base while in reverse, a conjugate base is a species formed by the removal of a proton from an acid.

True

False

Multiple Choice

The Henderson-Hasselbalch equation can be used to calculate the specific pH of a given buffer.

True

False

Multiple Choice

If an acid is added to the substance, the conjugate base of the buffer neutralizes the acid added. If a base is added to the substance, the conjugate acid of the buffer neutralizes the base added.

True

False

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