The hydrogen ion concentration is 0.2 M ethanoic acid $({\mathrm{K}}_{\mathrm{C}}=2\times {10}^{-5} \mathrm{mol} {\mathrm{dm}}^{-3})$ 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 ${\mathrm{K}}_{\mathrm{b}} \left({\mathrm{NH}}_3\right)=1.8\times {10}^{-5}$ and ${\mathrm{K}}_{\mathrm{sp}} \left[\mathrm{Fe}{\left(\mathrm{OH}\right)}_3\right]=2.6\times {10}^{-39}.$

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. $4.458\times {10}^{-22} \mathrm{M}$

A base dissolved in water yields a solution with a hydroxyl ion concentration of \(0.05 \mathrm{~mol}~ \mathrm{litre}^{-1}\). The solution is:

1. Basic

2. Acid

3. Neutral

4. Either acid or neutral

Given that the ionization constant (\(K_a\)) of acetic acid \((\text{CH}_3\text{COOH})\) is \(1.7 \times 10^{-5}\) and the concentration of hydrogen ions (\(\text{H}^+ \)) is \(3.4 \times 10^{-4}\), what is the initial concentration of acetic acid (\(\text{CH}_3\text{COOH}\))?

1. \(3 . 4 \times \left(10\right)^{- 4}\)

2. \(3 . 4 \times \left(10\right)^{- 3}\)

3. \(6 . 8 \times \left(10\right)^{- 4}\)

4. \(6 . 8 \times \left(10\right)^{- 3}\)

At $25°\mathrm{C}$ the dissociation constant of a base, BOH is $1.0\times {10}^{-12}$, the concentration of hydroxyl ions 0.01 M aqueous solution of the base would become

1. $2.0\times {10}^{-6} \mathrm{mol} {\mathrm{L}}^{-1}$

2. $1.0\times {10}^{-5} \mathrm{mol} {\mathrm{L}}^{-1}$

3. $1.0\times {10}^{-6} \mathrm{mol} {\mathrm{L}}^{-1}$

4. $1.0\times {10}^{-7} \mathrm{mol} {\mathrm{L}}^{-1}$

The solubility product of AgI at $25°\mathrm{C}$ is $1.0\times {10}^{-16} {\mathrm{mol}}^2 {\mathrm{L}}^{-2}$. The solubility of AgI in 10^-4 N solution of KI at $25°\mathrm{C}$ is :  (in mol L^-1)

1. $1.0\times {10}^{-10}$

2. $1.0\times {10}^{-8}$

3. $1.0\times {10}^{-16}$

4. $1.0\times {10}^{-12}$

When 0.1 mole of CH₃NH₂ (ionization constant ${\mathrm{K}}_{\mathrm{b}}=5\times {10}^{-4}$) is mixed with 0.08 mol HCl and the volume is made up of 1 litre. The [H⁺] of resulting solution is -

(log 4 =  0.60)

1. $8\times {10}^{-2}$

2. $2\times {10}^{-11}$

3. $1.23\times {10}^{-4}$

4. $8\times {10}^{-11}$

The solution with pH value close to 1.0 among the following is:

If ${\mathrm{Ag}}^{+}+2{\mathrm{NH}}_3\rightleftharpoons \mathrm{Ag}{{\left({\mathrm{NH}}_3\right)}_2}^{+}; {\mathrm{K}}_1=1.8\times {10}^7$

${\mathrm{Ag}}^{+}+{\mathrm{Cl}}^{-}\rightleftharpoons \mathrm{AgCl}; {\mathrm{K}}_2=5.6\times {10}^9$

Then for

$\mathrm{AgCl}+2{\mathrm{NH}}_3\rightleftharpoons {\left[\mathrm{Ag}{\left({\mathrm{NH}}_3\right)}_2\right]}^{+}+{\mathrm{Cl}}^{-},$

Equilibrium constant will be

1. $0.32\times {10}^{-2}$

2. $3.11\times {10}^2$

2. $10.08\times {10}^{16}$

4. $1.00\times {10}^{-17}$