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Calculate the freezing point what solutions assuming complete dissociation?
Wiki User
∙ 13y ago
The problem with this question is that you did not provide any solutions, as stated, to calculate the freezing point for.
Wiki User
∙ 13y ago
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Assuming no change in temperature and pressure calculate the volume of O2 in liters required for the complete combustion of 14.9 L of butane C4H10?
Assuming no change in temperature and pressure, calculate the volume of O2 (in liters) required for the complete combustion of 14.9 L of butane (C4H10):
Why degree of dissociation of electrolyte increase with dilution?
these electrolytes will dissociate a lot less compared to the dissociation of strong electrolytes. This is due to the fact that they don't completely ionize in a moderately solution.
What is the concentration of K plus ions in a 0.025 M K2CO3 solution assuming complete dissociation?
K2CO3 ==> 2K^+ + CO3^2-0.025 M K2CO3 = 2 x 0.025 M K^+ = 0.05 M concentration of K+ ions.
Calculate the freezing point depression of an aqueous solution of 0.22 m FeCl3 Assume complete dissociation?
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
What is the molar concentration of Br- ions in a 0.225 M aqueous solution of FeBr3 assuming complete dissociation?
There are 0.225 mol dm-3 FeBr3 molecules. For each FeBr3 that fully dissociates, we get 3 Br- (and one F3+). It is fully dissociated. So 0.225 x 3 = 0.675 mol dm-3.
What describes a weak base in solution?
The dissociation is not complete.
Assuming no change in temperature and pressure calculate the volume of O2 in liters required for the complete combustion of 14.9 L of butane C4H10?
Assuming no change in temperature and pressure, calculate the volume of O2 (in liters) required for the complete combustion of 14.9 L of butane (C4H10):
Why degree of dissociation of electrolyte increase with dilution?
these electrolytes will dissociate a lot less compared to the dissociation of strong electrolytes. This is due to the fact that they don't completely ionize in a moderately solution.
What is the concentration of K plus ions in a 0.025 M K2CO3 solution assuming complete dissociation?
K2CO3 ==> 2K^+ + CO3^2-0.025 M K2CO3 = 2 x 0.025 M K^+ = 0.05 M concentration of K+ ions.
Calculate the freezing point depression of an aqueous solution of 0.22 m FeCl3 Assume complete dissociation?
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
How about that of inch2 to cm2?
Complete solutions from 0.02Nm to 10MNm
Would a strong electrolyte contain mostly ions mostly molecules or a combination of both?
Mostly ions, because the dissociation is near complete.
The pH in aqueous solution of hcl at 25c is 4 hcl0.003 moles was added to 1l of this solution calculate the new pH in the solution assume complete dissociation of hcl?
if its complete dissociation, then the products would be a salt and water, which means the pH is 7 or neutral. OMG, if the pH is currently 4 then [H+] = 1.0 e-4 M (pH = -log[H+]) if you add 0.003 moles then 1.0e-4 M +.003 M = .0031 M (Since the strong acid HCL completely dissociates in aq solution) pH = -log [.0031M] = 2.51
What is the molar concentration of Br- ions in a 0.225 M aqueous solution of FeBr3 assuming complete dissociation?
There are 0.225 mol dm-3 FeBr3 molecules. For each FeBr3 that fully dissociates, we get 3 Br- (and one F3+). It is fully dissociated. So 0.225 x 3 = 0.675 mol dm-3.
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Atrioventricular Dissociation (or commonly known as Complete Heart Block).
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