The concentration of CH3COOH that will have the same [H+] as obtained from 10-2 M HCOOH, is-

(Ka(CH3COOH)=10-5, Ka(HCOOH)=10-4)

1. 10 M

2. 5 M

3. 10-1 M

4. 6 M

Subtopic:  Ionisation Constant of Acid, Base & Salt |
 79%
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When NH4Cl is added to an aqueous solution of NH4OH, then

1. Concentration of [OH-] ions decreases.

2. Concentration of [OH-] ions increases.

3. Concentration of [NH4+] ions as well as concentration [OH-] ions increase.

4. Concentration of [NH4+] ions decreases.

Subtopic:  Common Ion Effect |
 62%
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500 ml of 0.2 M HCl is mixed with 500 ml of 0.2 M CH3COOH. 25 ml of the mixture is titrated with 0.1 M NaOH solution. By how many units does the pH change from the start to the stage when HCl is just completely neutralized. Ka for acetic acid=2.0×10-5.

1. 3.7

2. 4.4

3. 2.0

4. 3.0

Subtopic:  pH calculation |
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When 60 ml of 0.1 M Ca(NO3)2 is mixed with 40 ml of 0.125 M Na2CO3CaCO3 precipitates. If Ksp of CaCO3 is 5×10-9 , then [CO32-] in the resulting solution is

1. 5×10-8 M

2. 5×10-9 M

3. 5×10-6 M

4. 5×10-7 M

Subtopic:  Solubility Product |
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100 ml of 0.3 M NH4OH is mixed with 100 ml of 0.2 M NaOH. Kb NH4OH is 1.8×10-5. The degree of dissociation of NH4OH is

1. 1.02×10-2

2. 1.8×10-5

3. 1.8×10-4

4. 1.02×10-4

Subtopic:  Ionisation Constant of Acid, Base & Salt |
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The ionization constant  of [NH4+] in water is 5.6×10-10 at 25°C. The rate constant for the reaction of [NH4+] and [OH-] to form NH3 and H2O is 3.4×1010 lit mol-1 sec-1 at 25°C. The rate constant for the proton transfer from water to NH3 in lit mol-1 sec-1 is

1. 6.07×105

2. 6.07×10-5

3. 6.07×10-3

4. 6.07×10-4

Subtopic:  Ionisation Constant of Acid, Base & Salt |
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Equilibrium constant of NH4+ to NH3 and H+ is 10-10. The rate constant for NH4++OH-NH3+H2O is 1010. The rate constant for NH3+H2ONH4++OH- is

1. 105

2. 106

3. 108

4. 109

Subtopic:  Ionisation Constant of Acid, Base & Salt |
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An acid base indicator has Ka=3×10-5. The acid form of the indicator is red and the basic form is blue. By how much must the pH change in order to change the indicator from 75% red to 75% blue (log 3=0.4770)

1. 0.95

2. 2.3

3. 0.75

4. 5

Subtopic:  Buffer |
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The dissociation constants for aniline, acetic acid and ionic product of water at 25°C are 3.83×10-10, 1.75×10-5 and 1.008×10-14 respectively. The degree of hydrolysis of aniline acetate in a decinormal solution is

1. 0.56%

2. 55%

3. 5.6%

4. 2.75%

 

Subtopic:  Salt Hydrolysis & Titration |
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A solution of benzoic acid (a weak monobasic acid) is titrated with NaOH. The pH of the solution is 4.2 when half of the acid is neutralized. The dissociation constant of the acid will be:

1. 3.2×10-5

2. 6.42×10-4

3. 6.31×10-5

4. 8.7×10-8

Subtopic:  Buffer |
 56%
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