The strongest Bronsted base among the following ions is:

1. CH₃O^-

2. (CH₃)₂CHO^-

3. C₂H₅O^-

4. (CH₃)₃CO^-

The degree of ionization of water was found to be $1.8\times {10}^{-9}$. The ${\mathrm{K}}_{\mathrm{a}}$ (ionization constant) of water is

1. $1.8\times {10}^{-9}$

2. $1.8\times {10}^{-16}$

3. $1.8\times {10}^{-14}$

4. cannot be calculated

The decreasing order of the acidic nature of ${\mathrm{H}}_2{\mathrm{SO}}_4<mspace\; width="1em"></mspace>\left(\mathrm{I}\right),<mspace\; width="1em"></mspace>{\mathrm{H}}_3{\mathrm{PO}}_4<mspace\; width="1em"></mspace>\left(\mathrm{II}\right),<mspace\; width="1em"></mspace>\mathrm{and}<mspace\; width="1em"></mspace>{\mathrm{HClO}}_4<mspace\; width="1em"></mspace>\left(\mathrm{III}\right)$ is:

1. I>II>III

2. I>III>II

3. III>I>II

4. III>II>I

The number of H⁺ ions present in 1cm³ of a solution whose pH is 10 is:

1. ${10}^{-10}$

2. ${10}^{-13}$

3. $6.02\times {10}^{10}$

4. $6.02\times {10}^{13}$

The \(K_a\) values of formic acid and acetic acid are respectively $1.77\times {10}^{-4}$ and $1.75\times {10}^{-5}$. The ratio of the acid strength of 0.1 N acids is :

1. 0.1

2. 0.3

3. 3.178

4. 100

ZnS is not precipitated by passing H₂S in an acidic medium but CuS is precipitated. The reason for it is

1. ${\mathrm{K}}_{\mathrm{sp}}<mspace\; width="1em"></mspace>\mathrm{CuS}<<{\mathrm{K}}_{\mathrm{sp}}<mspace\; width="1em"></mspace>\mathrm{ZnS}$

2.$<mspace\; width="1em"></mspace>{\mathrm{K}}_{\mathrm{sp}}<mspace\; width="1em"></mspace>\mathrm{CuS}>>{\mathrm{K}}_{\mathrm{sp}}<mspace\; width="1em"></mspace>\mathrm{ZnS}$

3. ${\mathrm{K}}_{\mathrm{sp}}<mspace\; width="1em"></mspace>\mathrm{CuS}={\mathrm{K}}_{\mathrm{sp}}<mspace\; width="1em"></mspace>\mathrm{ZnS}$

4. None of these

Consider the following acids:

The correct order of strength is:
1. II>III>I>IV
2. IV>II>III>I
3. IV>III>II>I
4. III>II>IV>I

The hydrogen ion concentration is 0.2 M ethanoic acid $({\mathrm{K}}_{\mathrm{C}}=2\times {10}^{-5}<mspace\; width="1em"></mspace>\mathrm{mol}<mspace\; width="1em"></mspace>{\mathrm{dm}}^{-3})$ is approximately

1. ${10}^{-4}$

2. $2\times {10}^{-2}$

3. $2\times {10}^{-6}$

4. $2\times {10}^{-3}$

The pH of a solution made by mixing 50 mL of 0.01 M barium hydroxide solution with 50 mL of H₂O is

Find the molar solubility of Fe(OH)₃ in a buffer solution that 0.10 M in NH₄Cl and 0.10 M in NH₃. If ${\mathrm{K}}_{\mathrm{b}}<mspace\; width="1em"></mspace>\left({\mathrm{NH}}_3\right)=1.8\times {10}^{-5}$ and ${\mathrm{}}_{}$
\(\text K_{ \text {sp}} [ \text {Fe(OH)}_3] = 2.6 \times 10^{-39}\)

1. \(4 .458 \times 10^{-25}~ \mathrm{M} \)
2. \(3.458 \times 10^{-25}~ \mathrm{M} \)
3. \(2 .229 \times 10^{-24} ~\mathrm{M} \)
4. \(4.458 \times 10^{-22} ~\mathrm{M}\)