The pH of a solution made by mixing 50 mL of 0.01 M barium hydroxide solution with 50 mL of H2O is
1. | 3.0 | 2. | 6.0 |
3. | 12.0 | 4. | 15.0 |
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 and
1.
2.
3.
4.
A base dissolved in water yields a solution with a hydroxyl ion concentration of 0.05 mol litre-1. The solution is
1. basic
2. acid
3. neutral
4. either 2 or 3
Ionization constant of CH3COOH is and concentration of H+ ion is . Then initial concentration of CH3COOH is
1.
2.
3.
4.
At the dissociation constant of a base, BOH is , the concentration of hydroxyl ions 0.01 M aqueous solution of the base would become
1.
2.
3.
4.
The solubility product of AgI at is . The solubility of AgI in 10-4 N solution of KI at is : (in mol L-1)
1.
2.
3.
4.
When 0.1 mole of CH3NH2 (ionization constant ) 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.
2.
3.
4.
The solution with pH value close to 1.0 among the following is:
1. | 100 ml of (M/10) HCl + 100 ml of (M/10) NaOH |
2. | 55 ml of (M/10) HCl + 45 ml of (M/10) NaOH |
3. | 10 ml of (M/10) HCl + 90 ml of (M/10) NaOH |
4. | 85 ml of (M/10) HCl + 15 ml of (M/10) NaOH |
If
Then for
Equilibrium constant will be
1.
2.
2.
4.
There sparingly soluble saltrs A2X, AX and AX3 have the same solubility product.Their solubilities will be in the order
1. AX3>AX>A2X
2. AX3 < A2X>AX
3. AX>AX3>A2X
4. AX>A2X>AX3