Find out the solubility of NiOH2 in 0.1 M NaOH, given that the ionic product of NiOH2 is 2x 10-15 

1. 2 x 10-8 M.

2. 1 x 10-13 M

3. 1 x 108

4. 2 x 10-13 

Subtopic:  Solubility Product |
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Which of the following salt solutions is basic in nature?

1. Ammonium chloride

2. Ammonium sulphate

3. Ammonium nitrate

4. Sodium acetate

Subtopic:  Salt Hydrolysis & Titration |
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The molar solubility of CaF2 (Ksp=5.3 x 10-11) in 0.1 M solution of NaF will be:

1. 5.3 x 10-11 mol L-1

2. 5.3 x 10-8 mol L-1

3. 5.3 x 10-9 mol L-1

4. 5.3 x 10-10 mol L-1

Subtopic:  Solubility Product |
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Which of the following cannot act both as a Bronsted acid and as a Bronsted base?

1. HCO3-

2. NH3

3. HCl

4. HSO4-

Subtopic:  Acids & Bases - Definitions & Classification |
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The pH of a 0.01 M NaOH (aq) solution will be:

1. 7.01

2. 2

3. 12

4. 9

Subtopic:  pH calculation |
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Given that the equilibrium constant for the reaction 

2SO2(g) + O2(g)  2SO3(g) 

has a value of 278 at a particular temperature, the value of the equilibrium constant for the following reaction at the same temperature will be:

SO3(g)   SO2(g) + 1/2 O2(g) 

1.  3.6 × 10-3 

2.  6.0 × 10-2 

3.  1.3 × 10-5 

4.  1.8 × 10-3 

Subtopic:  Kp, Kc & Factors Affecting them |
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Given reaction: A2(g) + B2(g)   2AB(g) 

At equilibrium , the concentrations of A2 = 3.0 × 10-3 M ; B2 = 4.2 × 10-3 M and AB = 2.8 × 10-3 M

If the reaction takes place in a sealed vessel at 527°C, then the value of KC will be : 

1.  3.9 

2.  0.6 

3.  4.5

4.  2.0 

 

Subtopic:  Kp, Kc & Factors Affecting them |
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In qualitative analysis, the metals of Group I can be separated from other ions by precipitating them as chloride salts. A solution initially contains Ag+
and Pb2+ at a concentration of 0.10 M. Aqueous HCl is added to this solution until the Cl– concentration is 0.10 M. What will the concentration of Ag+
and Pb2+ at equilibrium?

Ksp for AgCl=1.8×10-10(Ksp for PbCl2=1.7×10-5)

1. Ag+=1.8×10-11 M;

    Pb2+=1.7×10-4M

2. Ag+=1.8×10-7 M;

    Pb2+=1.7×10-6M

3. Ag+=1.8×10-11 M;

   Pb2+=8.5×10-5M

4. Ag+=1.8×10-9 M;

   Pb2+=1.7×10-3M

Subtopic:  Solubility Product |
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The reaction

2A+B(g)  3C(g)+D(g)

begins with the concentrations of A and B both at an intial value of 1.00 M. When equilibrium is reached, the concentration of D is measured and found to be 0.25 M. The value for the equilibrium constant for this reaction is given by the expression.

1. [(0.75)3(0.25)]÷[(0.50)2(0.75)]

2. [(0.75)3(0.25)]÷[(0.50)2(0.25)]

3. [(0.75)3(0.25)]÷[(0.75)2(0.25)]

4. [(0.75)3(0.25)]÷[(1.00)2(1.00)]

Subtopic:  Kp, Kc & Factors Affecting them |
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The equilibrium constant Kp for the following reaction is-

MgCO3(s)MgO(s)+CO2(g)

1. Kp=PCO2

2. Kp=PCO2×PCO2×PMgOPMgCO3

3. Kp=PCO2+PMgOPMgCO3

4. Kp=PMgCO3PCO2×PMgO

Subtopic:  Kp, Kc & Factors Affecting them |
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