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20 Nov 2019

Consider the bases in the table. Which base would be the bestchoice for preparing a pH = 9.00buffer?


ammonia methylamine ethylamine aniline pyridine



Find the ratio of base/acid to make 1.0 L of thisbuffer.


_____ (M base / M acid)?


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Patrina Schowalter
Patrina SchowalterLv2
25 Feb 2019

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Related questions

Preparing Buffer Solutions: Calculating the Volume of Weak Base Needed Use the table of K values given with this problem to choose the best weak base to start from for making a buffer that holds the pH of the solution at 4.70. Make your selection so that you maximize the capacity of the buffer. Assume that you want to make 100 mL of a buffer and you have already added enough of the conjugate acid salt to make the final buffer 0.30 M in this salt. How many mL of a 3.6 M solution of the weak base you selected must be added to the volumetric flask so that when filled to the mark, the pH of the buffer will equal 4.70. .09 Incorrect: Your answer is incorrect. mL Weak Base Kb NH3 (Ammonia) 1.76 X 10-5 C6H5NH2 (Aniline) 3.9 X 10-10 (CH3CH2)2NH (Diethyl amine) 6.9 X 10-4 C5H5N (Pyridine) 1.7 X 10-9 CH3CH2NH2 (Ethyl amine) 5.6 X 10-4 (CH3)3N (Trimethyl amine) 6.4 X 10-5 (CH3)2NH (Dimethyl amine) 5.4 X 10-4

Consider the following data on some weak acids and weak bases

acid

Ka
name formula
acetic acid

HCH3CO2

1.8 x10−5
hydrocyanic acid

HCN

4.9 x 10−10
base

Kb
name formula
pyridine

C5H5N

1.7 x 10−9
ammonia

NH3

1.8 x 10−5

Use this data to rank the following solutions in order of increasing pH. In other words, select a '1' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on.

0.1M NaCH3CO2

0.1M NH4Br

0.1M NaBr

0.1M KCN

Calculate the pH of a 0.4310 M aqueous solution of sodium dihydrogen phosphate, NaH2PO4.

Use the Tables link on the toolbar for any equilibrium constants that are required

Acid/Base Ionization Constants at 25 oC

Acid

Formula

Ka1

Ka2

Ka3

Acetic acid

CH3COOH

1.8 × 10-5

Acetylsalicylic acid (aspirin)

HC9H7O4

3.0 × 10-4

Aluminum ion

Al(H2O)43+

1.2 × 10-5

Arsenic acid

H3AsO4

2.5 × 10-4

5.6 × 10-8

3.0 × 10-13

Ascorbic acid

H2C6H6O6

7.9 × 10-5

1.6 × 10-12

Benzoic acid

C6H5COOH

6.3 × 10-5

Carbonic acid

H2CO3

4.2 × 10-7

4.8 × 10-11

Ferric ion

Fe(H2O)63+

4.0 × 10-3

Formic acid

HCOOH

1.8 × 10-4

Hydrocyanic acid

HCN

4.0 × 10-10

Hydrofluoric acid

HF

7.2 × 10-4

Hydrogen peroxide

H2O2

2.4 × 10-12

Hydrosulfuric acid

H2S

1.0 × 10-7

1.0 × 10-19

Hypochlorous acid

HClO

3.5 × 10-8

Nitrous acid

HNO2

4.5 × 10-4

Oxalic acid

H2C2O4

5.9 × 10-2

6.4 × 10-5

Phenol

C6H5OH

1.0 × 10-10

Phosphoric acid

H3PO4

7.5 × 10-3

6.2 × 10-8

3.6 × 10-13

Sulfuric acid

H2SO4

very large

1.2 × 10-2

Sulfurous acid

H2SO3

1.7 × 10-2

6.4 × 10-8

Zinc ion

Zn(H2O)42+

2.5 × 10-10

Base

Formula

Kb

Ammonia

NH3

1.8 × 10-5

Aniline

C6H5NH2

7.4 × 10-10

Caffeine

C8H10N4O2

4.1 × 10-4

Codeine

C18H21O3N

8.9 × 10-7

Diethylamine

(C2H5)2NH

6.9 × 10-4

Dimethylamine

(CH3)2NH

5.9 × 10-4

Ethylamine

C2H5NH2

4.3 × 10-4

Hydroxylamine

NH2OH

9.1 × 10-9

Isoquinoline

C9H7N

2.5 × 10-9

Methylamine

CH3NH2

4.2 × 10-4

Morphine

C17H19O3N

7.4 × 10-7

Piperidine

C5H11N

1.3 × 10-3

Pyridine

C5H5N

1.5 × 10-9

Quinoline

C9H7N

6.3 × 10-10

Triethanolamine

C6H15O3N

5.8 × 10-7

Triethylamine

(C2H5)3N

5.2 × 10-4

Trimethylamine

(CH3)3N

6.3 × 10-5

Urea

N2H4CO

1.5 × 10-14

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