A tank is full of water. Water is coming in as well as going out at same rate. What will happen to level of water in a tank? What is name given to such a state?

What is the expression for \({ k }_{ sp } \ of \ { Ag }_{ 2 }Cr{ 0 }_{ 4 }?\)

Under the conditions is a substance precipitated from its solution?

pK_a  value of acids A,B,C,D are 1.5, 3.5, 2.0 and 5.0.Which of them is strongest acid?

The solubility product of silver bromide is 3.3 x 10^-13 Calculate its solubility.

The value of K_c for the reaction, \({ 3O }_{ 2 }(g)\rightleftharpoons { 2O }_{ 3 }(g)\) is 2.0 ×10^–50 at 25°C. If the equilibrium concentration of O₂ in air at 25°C is 1.6 ×10^–2, what is the concentration of O₃?

What will be the PH of 0.1 M ammonium acetate solution?\(P{ k }_{ a }=P{ k }_{ b }=4.74\)

For the following equilibrium, K_c = \(6.3\times { 10 }^{ 14 }\) at 1000 K  
\(NO(g)+{ O }_{ 3 }(g)\rightleftharpoons NO_{ 2 }(g)+{ O }_{ 2 }(g)\) Both the forward and reverse reactions in the equilibrium are elementary bimolecular reactions. What is K_c , for the reverse reaction?

What is the minimum volume of water required to dissolve 1g of calcium sulphate at 298 K? (For calcium sulphate, K_sp is 9.1 x 10^-6).

At 298 K, a 0.1M solution of acetic acid is 1.34% ionised. What is the ionisation constant K_a of acetic acid?

The solubility product of Agcl is 1.5\( \times10^{-10}\)Predict whether there will be any precipitation by mixing 50ml of 0.01 MAgno3 solution.

Equal volumes of 0.002 M solutions of sodium iodate and cupric chlorate are mixed together. Will it lead to precipitation of copper iodate? (For cupric iodate \(K_{sp}\) = 7.4 x \(10^{-8}\))

The following concentrations were obtained for the formation of NH₃ from N₂ and H₂ at equilibrium at 500K. [N₂] = 1.5 × 10^–2M. [H₂] = 3.0 × 10^–2 M and [NH₃] = 1.2 × 10^–2M. Calculate equilibrium constant.

The species: H₂O,HCO₃^- ,HSO₄^- and NH₃ can act both as Bronsted acids and bases. For each case give the corresponding conjugate acid and conjugate base.

Calculate the pH of the resultant mixtures 10 mL of 0.01 M H₂SO₄+10 mL of 0.01 M Ca(OH)₂

Calculate the pH of a buffer which is 0.1 M in acetic acid and 0.15 M in sodium acetate. Given that the ionisation costants of acetic acid is 1.75 x 10^-5. Also calculate the change in pH of the buffer if to 1L of the buffer 1 cc of 1 M NaOH are added.