A solution containing 18.25g of HCL and 500g of water. Find molality.
Solution and Explanation
Molality (m)=Mass of solvent in kg
No. of mass of solute
Molality =5000.5×1000=1m
Top Questions on Solutions
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[2mm] Order of \(\Delta T_b\) is: - 2 moles of liquid A and 3 moles of liquid B are mixed to from an ideal solution. The vapour pressure of ideal solution is 320 mm Hg. When 1 mole of A & 1 mole of B is further added then new vapour pressure of solution is 328.57 mm Hg. Find the vapour pressure of pure A ($P_A^\circ$) & pure B ($P_B^\circ$):
- If pure liquids A and B have vapour pressures of 55 kPa and 15 kPa respectively. If in a solution of A and B, mole fraction of A in vapour is 0.8, then find mole fraction of A in liquid phase.
- If percentage of N$_2$ above a liquid solution is 80% at a total pressure of 10 atm, then find the mole fraction of N$_2$ gas dissolved in solution.
[Given that Henry’s constant for N$_2$ is $7.6 \times 10^7$ mm Hg]
- Given below are two statements:
Statement-I: \( K_H \) is constant with change in concentration of gas till solution is dilute at a given temperature.
Statement-II: According to Henry’s Law, partial pressure of gas in vapor phase is inversely proportional to mole fraction of gas in solution.
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Which of the following are ambident nucleophiles?
[A.] CN$^{\,-}$
[B.] CH$_{3}$COO$^{\,-}$
[C.] NO$_{2}^{\,-}$
[D.] CH$_{3}$O$^{\,-}$
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Identify the anomers from the following.
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The standard Gibbs free energy change \( \Delta G^\circ \) of a cell reaction is \(-301 { kJ/mol}\). What is \( E^\circ \) in volts?
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Concepts Used:
Law of Chemical Equilibrium
Law of Chemical Equilibrium states that at a constant temperature, the rate of a chemical reaction is directly proportional to the product of the molar concentrations of the reactants each raised to a power equal to the corresponding stoichiometric coefficients as represented by the balanced chemical equation.
Let us consider a general reversible reaction;
A+B ↔ C+D
After some time, there is a reduction in reactants A and B and an accumulation of the products C and D. As a result, the rate of the forward reaction decreases and that of backward reaction increases.
Eventually, the two reactions occur at the same rate and a state of equilibrium is attained.
By applying the Law of Mass Action;
The rate of forward reaction;
Rf = Kf [A]a [B]b
The rate of backward reaction;
Rb = Kb [C]c [D]d
Where,
[A], [B], [C] and [D] are the concentrations of A, B, C and D at equilibrium respectively.
a, b, c, and d are the stoichiometric coefficients of A, B, C and D respectively.
Kf and Kb are the rate constants of forward and backward reactions.
However, at equilibrium,
Rate of forward reaction = Rate of backward reaction.
Kc is called the equilibrium constant expressed in terms of molar concentrations.
The above equation is known as the equation of Law of Chemical Equilibrium.