Among the following , the compound with highest pH is : 

1. CH3COOK

2. Na2CO3 

3. NH4Cl

4. NaNO3

Subtopic:  Acids & Bases - Definitions & Classification |
 53%
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The rapid change of pH near the stoichiometric point of an acid-base titration is the basis of indicator detection. pH of the solution is related to the concentrations of the conjugate acid (HIn) and base (In-) forms of the indicator by the expression: 

1. log [In-HIn]=pKIn-pH

2. log [HInIn-]=pKIn+pH

3. log [HInIn]=pH-pKIn

4. log [InHIn]=pH-pKIn

Subtopic:  Salt Hydrolysis & Titration |
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Solubility of a M2S salt is 3.5×10-6 then find out solubility product.

1. 1.7×10-6

2. 1.7×10-16

3. 1.7×10-18

4. 1.7×10-12

Subtopic:  Solubility Product |
 73%
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The solubility of MX2 type electrolyte is 0.5×10-4 mol L-1. Then find out Ksp of electrolytes.

1. 5×10-12

2. 25×10-10

3. 1×10-13

4. 5×10-13

Subtopic:  Solubility Product |
 78%
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The solubility product of a sparing soluble salt AX2 is 3.2×10-11. Its solubility (in mol L-1) is

1. 5.6×10-6

2. 3.1×10-4

3. 2×10-4

4. 4×10-4

Subtopic:  Solubility Product |
 83%
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An acid solution of 0.005 M has a pH of 5. The degree of ionization of acid is

1. 0.1×10-2

2. 0.2×10-2

3. 0.5×10-4

4. 0.6×10-6

Subtopic:  Salt Hydrolysis & Titration |
 80%
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pKa value of four acids are given below. The strongest acid is

(I) 4.0

(II) 3.5

(III) 2.5

(IV) 2

1. I

2. II

3. III

4. IV

Subtopic:  pH calculation |
 86%
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A solution has hydrogen ion concentration 0.0005 M, its pOH is

1. 8.2798

2. 10.6990

3. 12.7854

4. 13.3344

 

Subtopic:  pH calculation |
 84%
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At 25°C, the pH of a solution containing 0.10 M sodium acetate and 0.03 M acetic acid will be:

[pKa value of CH3COOH=4.57]-

1. 3.24

2. 4.59

3. 5.09

4. 6.67

Subtopic:  Buffer |
 76%
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Ionization constant of acetic acid is 1.8×10-5. The concentration of H+ ions in 0.1 M solution is

1. 1.8×10-3 M

2. 2.8×10-3 M

3. 1.3×10-3 M

4. 1.34×10-4 M

Subtopic:  Ionisation Constant of Acid, Base & Salt |
 66%
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