Question

In: Chemistry

Match the most appropriate answer choice to each statement provided. According to ionization principles, a...

Match the most appropriate answer choice to each statement provided.

According to ionization principles, a weak electrolyte will ionize or dissociate in a(n) ____________ process.

The common ion effect _______________ ionization because of the presence of an ion from an alternate source.

The difference in equilibrium caused by the common ion effect occurs because of ______________ principle.

The addition of a common ion from an alternate source effectively ___________ either product or reactant, shifting equilibrium to the opposite direction.

One of the most common applications of the common ion effect is in the formation of ____________ systems.

A buffer is formed from the combination of a weak acid or base and its corresponding ionic _______________.

Because of limited ionization in a buffer system, the pH of these systems ___________ from the pH of the weak acid/base.

The presence of both acid and base in a buffer allows it to ______________ pH changes from strong acid and base.

The pH of an acid buffer system can be calculated using the equation ______________________.

The pH of a buffer system of 0.1 M acetic acid and 0.24 M sodium acetate would be _______________, given a Ka value for acetic acid at 1.8x10-5.

Answers:

A. 4.74

B. buffer

C. supresses

D. differs

E. 5.60

F. enhances

G. adds

H. conjugate salt

I. 5.12

J. resist

K. predict

L. equilibrium

M. Le Chatelier's

N. pH = pKa + log ([A-]/[HA])

O. subtract

Solutions

Expert Solution

1. According to ionization principles, a weak electrolyte will ionize or dissociate in a(n) buffer process.

2. The common ion effect supressesionization because of the presence of an ion from an alternate source.

3. The difference in equilibrium caused by the common ion effect occurs because of Le Chatelier's principle.

4. The addition of a common ion from an alternate source effectively adds either product or reactant, shifting equilibrium to the opposite direction.

5. One of the most common applications of the common ion effect is in the formation of equilibrium systems.

6. A buffer is formed from the combination of a weak acid or base and its corresponding ionic conjugate salt.

7. Because of limited ionization in a buffer system, the pH of these systems differs from the pH of the weak acid/base.

8. The presence of both acid and base in a buffer allows it to predict pH changes from strong acid and base.

9. The pH of an acid buffer system can be calculated using the equation pH = pKa + log ([A-]/[HA]).

10. The pH of a buffer system of 0.1 M acetic acid and 0.24 M sodium acetate would be 5.12, given a Ka value for acetic acid at 1.8x10-5.

queen_honey_blossom answered 1 year ago

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