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?

For the reaction,\({ H }_{ 2 }(g)+{ I }_{ 2 }(g)\rightleftharpoons 2HI(g)\) the standard free energy is  \(\Delta { G }^{ \circleddash }>0\) . How is the equilibrium constant effected?

What will be the pH of 1M\(N{ a }_{ 2 }{ so }_{ 4 }\)solution?

Is it possible to get a precipitate of \(Fe(OH{ ) }_{ 3 }\)at pH = 2? given reason.

Why pH of our blood remains almost constant at 7.4 though we quite often eat spicy food?

Can the following reaction,
\({ Cr }_{ 2 }{ O }_{ 7 }^{ 2- }+{ H }_{ 2 }O\rightleftharpoons { 2Cro }_{ 4 }^{ 2- }+{ 2H }^{ + }\) be regarded as a redox reaction?

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?

How much CH₃COONa should be added to 1 L of 0.1 M CH₃COOH to make a buffer of pH=4.0?
[K_a =1.8 x 10^-5]

The reaction, \(CO(g)+3{ H }_{ 2 }(g)\leftrightharpoons { CH }_{ 4 }+{ H }_{ 2 }O(g)\) is at equilibrium at 1300 K in a 1L flask. It also contains 0.30 mole of CO, 0.10 mole of H₂ and 0.02 mole of H₂ O, and an unknown amount of CH₄ in the mixture. The equilibrium constant, K_c for the reaction at the given temperature is 3.90.

Why does the following reaction occur?
\({ XEO }_{ 6 }^{ 4- }(aq)+{ 2F }^{ - }(aq)+{ 6H }^{ + }(aq)\longrightarrow { Xeo }_{ 3 }(g)+{ F }_{ 2 }(g)+3{ H }_{ 2 }O(l)\)
What conclusion about the compound Na₄CeO₆ (of which \(​​XeO_{ 6 }^{ 4- }\)is a part) can be drawn from the reaction?

Consider the reactions,
\(2{ S }_{ 2 }{ O }_{ 3 }^{ 2- }(aq)+{ I }_{ 2 }(s)\longrightarrow { S }_{ 4 }{ O }_{ 6 }^{ 2- }(aq)+{ 2I }^{ - }(aq)\)
\( { S }_{ 2 }{ O }_{ 3 }^{ 2- }(aq)+2{ Br }_{ 2 }(l)+5{ H }_{ 2 }O(l)\longrightarrow 2{ SO }_{ 4 }^{ 2- }(aq)+4{ Br }^{ - }(aq)+10{ H }^{ + }(aq)\)
Why does the same reductant, thiosulphate react differently with iodine and bromine?
Bromine is a stronger oxidising agent than iodine.

If 0.561 g of KOH is dissolved in water to give 200 mL of solution at 298 K. Calculate the concentrations of potassium, hydrogen and hydroxyl ions. What is its pH?

One of the reaction that takes place in producing steel from iron ore is the reduction of iron(II) oxide by carbon monoxide to give iron metal and CO₂.
\(Feo(s)+CO(g)\leftrightharpoons Fe(s)+{ CO }_{ 2 }(g); { K }_{ p }=0.265 \ atm \ at \ 1050 \ K\)
What are the equilibrium partial pressures of CO and CO₂ at 1050 K if the initial partial pressures are: \({ P }_{ co }=1.4 \ atm\) and \({ PCO }_{ 2 }=0.80\) atm?

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 700 K, equilibrium constant for the reaction:
\({ H }_{ 2 }(g)+{ I }_{ 2 }(g)\leftrightharpoons 2HI(g)\)
is 54.8. If 0.5 mol L^–1 of HI(g) is present at equilibrium at 700 K, what are the concentration of H₂(g) and I₂(g) assuming that we initially started with HI(g) and allowed it to reach equilibrium at 700K?

50.0 g of CaCO₃ are heated to 1073 K in a 5L vessel. What percent of the CaCO₃ would decompose at equilibrium? K_p for the reaction.
\({ CaCO }_{ 3 }(s)\rightleftharpoons CaO(s)+{ CO }_{ 2 }(g)\) is 1.15 a/m at 1073 K.

Calculate the pH of the following solutions.
0.3 g of Ca(OH)₂ dissolved in water to give 500 mL solution.

What is the pH of 0.001M aniline solution? The ionization constant of aniline can be taken from Table . Calculate the degree of ionization of aniline in the solution. Also calculate the ionization constant of the conjugate acid of aniline.

Dihydrogen gas is obtained from natural gas by partial oxidation with steam as per following endothermic reaction.
\({ CH }_{ 4 }\left( g \right) +{ H }_{ 2 }O\left( g \right) \rightleftharpoons { CO }\left( g \right) +3{ H }_{ 2 }\left( g \right) \)
How will the value of K_p and composition of equilibrium mixture be affected by
(a) increasing the pressure
(b) increasing the temperature
(c) using a catalyst?