Chemical Equilibrium

A solution of two components containing n₁ moles of the 1st component and n₂ moles of the 2nd component is prepared. M₁ and M₂ are the molecular weights of component 1 and 2 respectively. If d is the density of the solution in gmL⁻¹, C₂ is the molarity and x₂ is the mole fraction of the 2nd component, then C₂ can be expressed as:

The stoichiometry and solubility product of a salt with the solubility curve given below is, respectively:

$3\mathrm{g}$ of acetic acid is added to $250\mathrm{m}\mathrm{L}$ of $0.1\mathrm{M}\mathrm{H}\mathrm{C}\mathrm{l}$ and the solution made up to $500\mathrm{m}\mathrm{L}$ . To $20\mathrm{m}\mathrm{L}$ of this solution $1/2\mathrm{m}\mathrm{L}$ of $5\mathrm{M}\mathrm{N}\mathrm{a}\mathrm{O}\mathrm{H}$ is added. The $\mathrm{p}\mathrm{H}$  of the solution is

[Given: ${\mathrm{p}\mathrm{K}}_{\mathrm{a}}$ of acetic acid $=4.75$ , molar mass of acetic acid $=60\mathrm{g}/\mathrm{m}\mathrm{o}\mathrm{l},\mathrm{l}\mathrm{o}\mathrm{g}?3=0.4771$  ] Neglect any changes in volume.

Assuming that Ba(OH)₂ is completely ionized in aqueous solution under the given conditions the concentration of H₃O⁺ ions in 0.005 M aqueous solution of Ba(OH)₂ at 298 K is __________ * 10⁻¹² mol L⁻¹. (nearest integer)

An homogeneous ideal gaseous reaction $A{B}_{2\left(g\right)}?A_{\left(g\right)}+2B_{\left(g\right)}$  is carried out in a 25 litre flask at 27°C. The initial amount of AB₂ was 1 mole and the equilibrium pressure was 1.9atm. The value of K_p is x * 10^-2. The value of x is-----------. (Integer answer).

[R = 0.08206 dm³ atm K^-1 mol^-1]

At 1990K and 1 atm pressure, there are equal number of Cl₂ molecules and Cl atoms in the reaction mixture. The value of K_P for the reaction $?$ Cl_2(g)  2Cl_(g) under the above conditions is x * 10^-1. The value of x is______ (Rounded off to the nearest integer)