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Freezing point of the solution will increase. Mercuric Iodide will react with Potassium Iodide to form dipotassium tetraiodomercury. The reaction is given below :2KI + HgI2 = K2[HgI4]This association will decrease the number of ions in the solution as a result of which Van't Hoff Factor (i) will decrease as n decreases from 4 to 3.Now, Freezing point depression when a solute is added to a solvent is given by ΔT = i Kf mClearly now i has decreased from when it was an aqueous KI solution to when HgI is added so ΔT is less now, hence less depression in freezing point which means a higher freezing point.Hence the freezing point of solution will increase.Note: Van't Hoff factor (i) =1+alpha(n-1) where alpha=dissociation degree and n is the no of ions dissociatedHope you understand the reasoning behind it now.
Theritical MM/ Observed MM = 1 + a (2-1) 58.5/30 = 1+a a = .95 or 95%
An *aqueous* solution is formed when a substance is dissolved in water. The term "aqueous" stands for the latin word "aqua" which means water.
F.p.'s and B.p.'s are independent (intensive) properties, you can NOT calculate them.
Haemocyanins are a group of proteins.
-0.37 C
look at Calculate_the_boiling_point_elevation_of_an_aqueous_solution_of_0.0500_m_CaCl2_Assume_complete_dissociationvery similar questionanswer is 1.64 lower than the originial freezing pointif the freezing point is 0 for example the freezing point depression is -1.64
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Higher boiling point and a lower freezing point. These are called colligative properties. When a solute is put into solution with the solvent, there is a change in the vapor pressure, osmotic pressure, elevation of the boiling point, and depression of the freezing point.
-14.8
Freezing point of the solution will increase. Mercuric Iodide will react with Potassium Iodide to form dipotassium tetraiodomercury. The reaction is given below :2KI + HgI2 = K2[HgI4]This association will decrease the number of ions in the solution as a result of which Van't Hoff Factor (i) will decrease as n decreases from 4 to 3.Now, Freezing point depression when a solute is added to a solvent is given by ΔT = i Kf mClearly now i has decreased from when it was an aqueous KI solution to when HgI is added so ΔT is less now, hence less depression in freezing point which means a higher freezing point.Hence the freezing point of solution will increase.Note: Van't Hoff factor (i) =1+alpha(n-1) where alpha=dissociation degree and n is the no of ions dissociatedHope you understand the reasoning behind it now.
-10.6 c
This solution is called water solution or aqueous solution.
'An Aqueous' solution. NB The word 'aqueous' comes from Latin ; 'aqua' meaning 'water'.
dT = (i)(Kf)(m) is the equation that can be used to model the freezing point depression. dT represents the change change in temperature. i represents the amount of ions formed from the dissolution of the solute. Kf represents the constant of the freezing point depression of water. m is the molality of the solute in solution. dT = (3)(1.86 degC/m)(2.65m) dT = 14.8 degC 0-14.8 degC = -14.8 degC So the freezing point is -14.8 degrees C. The reason why this value was subtracted from zero is because the presence of a solute lowers the freezing point.
Theritical MM/ Observed MM = 1 + a (2-1) 58.5/30 = 1+a a = .95 or 95%
-10.6 Celsius