Assuming complete electrolytic dissociation of KBr, what is the molality of an a

Question

Assuming complete electrolytic dissociation of KBr, what is the molality of an aqueous solution of KBr which has the freezing point of -2.95 degree C? The molal freezing-point depression constant of water K_f = 1.86 (degree C kg)/mol. What is the normal boiling point (in degree C) of a solution prepared by dissolving 1-50gof aspirin (acetylsalicylic acid, C_5H_2O_4) in 75.000 g of chloroform (CHCI_4)? The normal boiling point for chloroform is 61.7 degree C and K_b = 3.63 (degree C kg)/mol. (Aspirin does not dissociate into ions in chloroform). Which of the following would be the most efficient in elevation of the boiling point of water? Show your calculations! 0.05 m NaBr; 0.10 m glucose; 0.02 m CuCl; 0.02 m FeCl_3; 0.075 KCI. A solution of a substance A in water at temperature 27 degree C produces an osmotic pressure of 3.85 atm. What is the molarity of A in this solution? What is the vapour pressure (in torr) of a solution prepared by dissolving 5.00 g of benzoic acid (C_7H_6O_2) in 100.0 g of ethanol (C_2H_5O) at 35 degree C?. The vapor pressure of pure ethanol at 35 degree C is 100.5 torr. (Assume that benzoic acid does not dissociate into ions in ethanol). For solid sodium, Na, the enthalpy of fusion delta_H = 2.64 kJ/mol. What is the enthalpy of freezing for liquid Na? How much energy, delta H (in kJ) is needed to heat 5.00g of ice from - 10.0 degree C to 30 degree C? Given enthalpy of fusion of water delta_H (water) = 6.01 kJ/mol; specific heat values for solid and liquid water are Cs(water, s) = 2.03 J/(g middot degree C) and C_s(water, I) = 4.18 J/(g degree C). How much energy, delta(in kJ) is released when 18.0 g of water steam at 115 degree C is converted into liquid water with temperature of 100 degree C? Given: enthalpy of vaporization of water delta H_vap (water) = 40.67 kJ/mol; specific heat for water vapor Cs(water, g) = 1.87 J/(g middot degree C). Assume that you place 50.0 ml, of 2.10 M HCI solution into a 250.0-mL volumetric flask and add water to the mark. What is the molarity of HCl after dilution? (Give the answer with correct number of significant figures).

Explanation / Answer

Normal freezing point of water = 0 C

Given freezing point = -2.95 C

So depression in freezing point = 2.95 C

Given K =1.86

We know that,

T = K*m

2.95 = 1.86 * m

Molality = 1.586 m

Only one question should be answered according to chegg rules.pls post questions. Separately

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