Question

1. What is the boiling point of a 3.0 m Ca(NO3)2 solution in water?

Where:

the change in boiling point (ΔTb) = mKb

m is the molality of the solution

Kb (the boiling point constant) for water is 0.512

2. The freezing point of ethanol (C₂H₅OH) is -114.6 °C.  What is the freezing point (°C) of a solution prepared by dissolving 50.0 g of glycerin a nonelectrolyte) in 200.0 g of ethanol?

(C3H803,

Where:

ΔT_f = mK_f

The molal freezing point depression constant (K_f) ( for ethanol is 2.00 °C/m.

3. The osmotic pressure of blood is 7.65 atm at 37°C. If blood were considered a solution of NaCl, what is the molar concentration of NaCl in blood? Assume an ideal van’t Hoff factor.

Where:

Π = iMRT

R is the ideal gas law constant ( $LaTeX: 0.08205\:\frac{L\cdot atm}{mol\cdot K}$ 0.08205 L ⋅ a t m m o l ⋅ K)

and T is the absolute temperature

4. Why do ice cubes get smaller when left in the freezer for a long time?

  

Neither The ice cubes melt during the brief warming cycles of auto-defrost and freezer access, thus leaving the ice cubes smaller and making them stick together in clumps nor The water molecules of the ice sublime from the solid to gaseous phase without ever entering a liquid phase accurately explain why ice cubes get smaller in the freezer over time.

   

The ice cubes melt during the brief warming cycles of auto-defrost and freezer access, thus leaving the ice cubes smaller and making them stick together in clumps.

   

The water molecules of the ice sublime from the solid to gaseous phase without ever entering a liquid phase.

   

Both The ice cubes melt during the brief warming cycles of auto-defrost and freezer access, thus leaving the ice cubes smaller and making them stick together in clumps and The water molecules of the ice sublime from the solid to gaseous phase without ever entering a liquid phase occur.

5. What volume of 18.0 M sulfuric acid is required to prepare 26.20 L of 0.126 M H₂SO₄?

  

3.30 L

  

207.94 mL

  

0.183 L

  

471.60 mL

  

5.45 mL

Answer 1

1. The change in boiling point Atb = mkz The boiling point constant ky=0.512 elm for coater m= molal concentration of the solution. Ath-380-5+2je The boiling point elevation is given by a To= ix koxm is van't Hoff factor vant Hoff factor i tor Ca(NO3)2 is 3 because one male of it gives 3 ions (I caht and 2 N02-) so oTo= (3x 0.512 x3) C = 4.608°C & DTy = To - To To = DIG + To [ For water Tyo = 100° e] :. To = 1000 e + 4.608° 0 = 104.608°C T = 104.61°C

epression 2. Att = mkg = The molal doreezing point constant - 2.00°clm 50 g glyarn (C₂ H2O₂) is dissolved in 200g of ethanol. La converting the giren mass of glycerin to moles using its molar mass: nog glycern (1 mol glycerin ) 0.543 mo 192.00 g glycerin me m mal glycerin 0.543 - - 2.715 molalily - 0.2 ky et to the o Off = i xm x kq = 1 x 2.715 x 2 = 5.43 The freezing point of ethanol = - 114.6° 0 a t ATG = TG - If - T = 454 + tjº T = – ATJ - TJ o = 109.17 6 J = 46 (-5.43 + 114.6) C a solution is log. 17°C. so, the freezing point of

3. Osmotic poressure in expressed by the formula: T = iMRT where I = Osmotic pressure in alm i = van't Hoff factor of the = 7.65 atm solue. R = 0.08205 Lafm/mal. K M = molar concentration in mollL T = (37+273) K = 310k 7.65 .: M = 1 RT = 0.301 mol/L 1X0.8205x310 of rach in blood is 0.301 mol/L The molar concentration