The concentration of CH_{3}COOH that will have the same [H^{+}] as obtained from 10^{2} M HCOOH, is
$\left(\mathrm{Ka}\right({\mathrm{CH}}_{3}\mathrm{COOH})={10}^{5},$ $\mathrm{Ka}\left(\mathrm{HCOOH}\right)={10}^{4})$
1. 10 M
2. 5 M
3. 10^{1} M
4. 6 M
The strongest acid among the following compounds is:
1.  HClO_{3}  2.  HClO_{4} 
3.  H_{2}SO_{3}  4.  H_{2}SO_{4} 
The ionization constant of acetic acid is 1.74 × 10^{–5}. The pH of acetic acid in its 0.05 M solution will be:
1. 7.81
2. 3.03
3. 8.54
4. 1.45
The ionization constant of propanoic acid is 1.32 × 10^{–5}. The degree of ionization of 0.05M acid solution will be:
1. $\mathrm{\alpha}$ = 0.63 × 10^{–}^{2}
2. $\mathrm{\alpha}$ = 1.63 × 10^{–}^{4}
3. $\mathrm{\alpha}$ = 1.63 × 10^{–}^{2}
4. $\mathrm{\alpha}$ = 0.05 × 10^{–}^{2}
The pH of a 0.1 M solution of cyanic acid (HCNO) is 2.34. The ionization constant of the acid will be:
$1.$ $2.02$ $\times $ ${10}^{4}$
$2.$ $3.14$ $\times $ ${10}^{3}$
$3.$ $2.02$ $\times $ ${10}^{4}$
$4.$ $1.01$ $\times $ ${10}^{4}$
The ionization constant of phenol is 1.0 × 10^{–10}. The concentration of phenolate ion in 0.05 M solution of phenol will be:
1.  4.2 × 10^{–}^{4} M

2.  3.6 × 10^{–}^{5} M

3.  7.8 × 10^{–}^{6} M

4.  2.2 × 10^{–}^{6} M 
The ionization constants of HCOOH, and HCN at 298K are 1.8 × 10^{–4} and 4.8 × 10^{–9} respectively. The ionization constants of the corresponding conjugate bases of HCOOH and HCN will be
1.  5.6 × 10^{–11}, 2.08 × 10^{–6}

2.  2.4 × 10^{–11}, 4.2 × 10^{–6}

3.  3.5 × 10^{–11}, 1.7 × 10^{–6}

4.  4.2 × 10^{–11}, 1.2 × 10^{–6} 
The degree of ionization of 0.05 M acetic acid is:
(pK_{a} = 4.74)
1.  $$ 1.91$$ \times {10}^{2}$$  2.  $$ 2.46$$ \times $$ {10}^{2}$$ 
3.  $$ 1.93$$ \times $$ {10}^{2}$$  4.  $$ 2.34$$ \times $$ {10}^{3}$$ 
The first ionization constant of H_{2}S is 9.1 × 10^{–8}. The concentration of HS^{–} ion in its 0.1 M solution will be:
1.  12.3 × 10^{–7 }M  2.  11.4 × 10^{–6} M 
3.  3.5 × 10^{–4} M  4.  9.54 × 10^{–5} M 
$1.$ $8.95$
$2.$ $1.43$
$3.$ $3.56$
$4.$ $6.30$