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Asked on 11/12/2021 Learn Equilibrium

CaC03(s) → CaO(s) + C02(g),∆fH° = -635.1 kJ mol--1,∆fH° = -393.5 kJ mol--1,∆fH° = -1206.9 kJ mol--1... read more
CaC03(s) → CaO(s) + C02(g),∆fH° [CaO(s)] = -635.1 kJ mol–1,∆fH° [COz(g)] = -393.5 kJ mol–1,∆fH° [CaC03(s)] = -1206.9 kJ mol–1 Predict the effect of temperature on the equilibrium constant of the above reaction. read less

Asked on 11/12/2021 Learn Equilibrium

A reaction between ammonia and boron trifluoride is given below: :NH3 + BF3 →H3N : BF3. Identify the... read more
A reaction between ammonia and boron trifluoride is given below: :NH3 + BF3 →H3N : BF3. Identify the acid and base in this reaction. Which theory explains it? What is the hybridization of B and N in the reactants? read less

Asked on 11/12/2021 Learn Equilibrium

Calculate the volume of water required to dissolve 0.1 g lead (II) chloride to get a saturated solution.... read more
Calculate the volume of water required to dissolve 0.1 g lead (II) chloride to get a saturated solution. (Ksp of PbCl2 = 3.2 x 10-8, atomic mass of Pb = 207 u). read less

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Asked on 11/12/2021 Learn Equilibrium

The solubility product of Al(OH)3 is 2.7 x 10-11. Calculate its solubility in g--L and also find out... read more
The solubility product of Al(OH)3 is 2.7 x 10-11. Calculate its solubility in g–L and also find out pH of this solution. (Atomic mass of A1 = 27 u). read less

Asked on 11/12/2021 Learn Equilibrium

Calculate the pH of a solution formed by mixing equal volumes of two solutions A and B of a strong acid... read more
Calculate the pH of a solution formed by mixing equal volumes of two solutions A and B of a strong acid having pH = 6 and pH = 4 respectively. read less

Asked on 11/12/2021 Learn Equilibrium

pH of 0.08 mol dm–3HOC1 solution is 2.85. Calculate its ionization constant.

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Asked on 11/12/2021 Learn Equilibrium

A sparingly soluble salt gets precipitated only when the product of concentration of its ions in the... read more
A sparingly soluble salt gets precipitated only when the product of concentration of its ions in the solution (Qsp) becomes greater than its solubility product. If the solubility of BaS04 in water is 8 x 10-4 mol dm-3, calculate its solubility in 0.01 mol dm-3 of H2S04. read less

Asked on 11/12/2021 Learn Equilibrium

pH of a solution of a strong acid is 5.0. What will be the pH of the solution obtained after diluting... read more
pH of a solution of a strong acid is 5.0. What will be the pH of the solution obtained after diluting the given solution a 100 times? read less

Asked on 11/12/2021 Learn Equilibrium

On the basis of the equation pH = -log , the pH of 10-8 mol dm-3 solution of HC1 should be 8. However,... read more
On the basis of the equation pH = -log [H+], the pH of 10-8 mol dm-3 solution of HC1 should be 8. However, it is observed to be less than 7.0. Explain the reason. read less

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Asked on 11/12/2021 Learn Equilibrium

The value of Kc for the reaction 2HI(g) ⇌H2(g) + I2(g) is 1 x 10-4. At a given time, the composition... read more
The value of Kc for the reaction 2HI(g) ⇌H2(g) + I2(g) is 1 x 10-4. At a given time, the composition of reaction mixture is [HI] = 2 x 10-5 mol, [H2] = 1 x 10-5 mol and [I2] = 1 x 10-5 mol. In which direction will the reaction proceed? read less

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