# <!--td {border: 1px solid #ccc;}br {mso-data-placement:same-cell;}--> The conjugate bases of Bronsted acids H2O and HF are respectively: 1.  H3O+ and H2F+, respectively 2.  OH- and H2F+, respectively 3.  H3O+ and F-, respectively 4.  OH- and F-, respectively

Subtopic:  Acids & Bases - Definitions & Classification |
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pH of a saturated solution of $\mathrm{Ca}{\left(\mathrm{OH}\right)}_{2}$ is 9. The solubility product $\left({\mathrm{K}}_{\mathrm{sp}}\right)$ of $\mathrm{Ca}{\left(\mathrm{OH}\right)}_{2}$ is:

1.  $0.5×{10}^{-10}$

2.  $0.5×{10}^{-15}$

3.  $0.25×{10}^{-10}$

4.  $0.125×{10}^{-15}$

Subtopic:  pH calculation |
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Which will make basic buffer:

1.  100 mL of 0.1 M HCl+100 mL of 0.1 M NaOH

2.  50 mL of 0.1 M NaOH+25 mL of 0.1 M CH3COOH

3.  100 mL of 0.1 M CH3COOH+100 mL of 0.1 M NaOH

4.  100 mL of 0.1 M HCl+200 mL of 0.1 M NH4OH

Subtopic:  Buffer |
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The hydrogen ion concentration of a 10-8 M HCl aqueous solution at 298 K (Kw = 10-14) is :

1.

2.

3.

4.

Subtopic:  pH calculation |
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Which of the following pairs constitutes a buffer?

1.

2.

3.

4.

Subtopic:  Buffer |
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For the reaction,
CH4(g) + 2O2(gCO2(g) + 2H2O(l
ΔrH = -170.8 kJ mol-1
Which of the following statements is not true?

1. At equilibrium, the concentration of $C{O}_{2}\left(g\right)$ and water (l) are not equal.

2. The equilibrium constant for the reaction is given by ${K}_{p}=\frac{\left[C{O}_{2}\right]}{\left[C{H}_{4}\right]\left[{O}_{2}\right]}$

3. Addition of  at equilibrium will cause a shift to the right

4. The reaction is exothermic

Subtopic:  Kp, Kc & Factors Affecting them |
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Which one of the following orders correctly represents the increasing acid strengths of the given acids?

1. $HOCl

2. $HOClO

3. $HOCl{O}_{2}

4. $HOCl{O}_{3}

Subtopic:  Acids & Bases - Definitions & Classification |
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Which ionic species has the greatest proton affinity to form stable compounds?

1. $H{S}^{-}$

2. $N{H}_{2}^{-}$

3. ${F}^{-}$

4. ${l}^{-}$

Subtopic:  Acids & Bases - Definitions & Classification |
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The following equilibrium constants are given :
N2 + 3H22NH3K1
N2 + O22NO; K2
H2 + 1/2O2H2O; K3
The equilibrium constant for the oxidation of NH3 by oxygen to give NO is:

1. ${K}_{2}{K}_{3}^{3}/{K}_{1}$

2. ${K}_{2}{K}_{3}^{2}/{K}_{1}$

3. ${K}_{2}^{2}{K}_{3}/{K}_{1}$

4. ${K}_{1}{K}_{2}/{K}_{3}$

Subtopic:  Kp, Kc & Factors Affecting them |
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A weak acid, HA, has a Ka of 1.00×10-5. If 0.100 mole of this acid is dissolved in one litre of water, the percentage of acid dissociated at equilibrium is closest to :

1. 99.0%

2. 1%

3. 99.9%

4. 0.100%

Subtopic:  Salt Hydrolysis & Titration |
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