Question

A solution containing 1.5 g of barium nitrate, Ba(NO3)2 in 0.1 Kg of water freezes at -0.43 degrees Celsius. Calculate the apparent degree of dissociation of the salt. (Kb of water = 1.86 degrees Celsius

Answer #1

Barium nitrate dissociates in ions,which increases the depression in freezing point of the solution.

A solution containing 0.11 kg of Ba(NO3)2 in 0.1 kg of water
boils at 100.46C calculate the degree of ionization of the salt
(kb-0.5 kg.C/mol)?

40g Ba(NO3)2 is dissolved in 1Kg of water
ate 313.15K.
a) Compute the equilibrium vapor pressure above the solution if
none of the Ba(NO3)2 ionizes. Assume the
solution behaves ideally in the Roult's law regime. The equilibrium
vapor pressure above pure water at 313.15K is 55.324 torr.
b) What would the vapor pressure be if barium nitrate ionizes
completely?
c) The actual vapor pressure is found to be 54.909 torr.
Calculate the percent ionization for barium nitrate.
d) Calculate Gmixing...

Barium sulfate is made by the following reaction:
Ba(NO3)2 (aq) +
Na2SO4 (aq) ? BaSO4 (s) +
2NaNO3 (aq)
An experiment was begun with 75.00 g of barium nitrate and
72.00g of sodium sulfate. After collecting and drying 64.45 g of
barium sulfate was obtained.
Calculate the theoretical yield,_________________
Calculate the percentage yield._________________

A solution is made by dissolving 15.1 g of
barium hydroxide,
Ba(OH)2, in enough water to make
exactly 100. mL of solution. Calculate the
molarity of each species:
Ba(OH)2 _______ mol/L
Ba2+ _________ mol/L
OH- _________ mol/L

When 100 mL of Ba(NO3)2 solution at 25 degrees Celsius is
mixed with 100 mL solution CaSO4 solution at 25 degrees Celsius in
calorimeter, the white solid BaSO4 forms and the temperature of the
mixture increases to 28.1 degrees Celsius. Assuming that the
calorimeter absorbs only a negligible quantity of heat and the
specific heat capacity of the solution is 4.184 J/g.degrees
Celsius, and that the density of the final solution is 1.0 g/mL,
calculate the enthalpy change of this...

Following the general procedure described in this experiment , a
student synthesized 6.895 g of barium idoate monhydrate, Ba(IO3)2 .
H2), by adding 30.00 mL of 5.912x10^(-1) M barium nitrate,
Ba(NO3)2, to 50.00 mL of 9.004x10^(-1) M sodium idoate, NaIO3.
When reviewing the procedure and calculations, the student
discovered that a 4.912x10^(-1) M barium nitrate solution had been
used instead of a 5.912x10^(-1) M solution.
Calculate the precent yield of barium iodate monhydrate using
30.00 mL of 4.912x10^(-1) M barium...

A coffee-cup calorimeter initially contains 125 g water at 24.2
degrees celsius. Ammonium Nitrate (10.5 g), also at 24.2 degree
celsius, is added to the water, and after the ammonium nitrate
dissolves, the final temperature is 18.3 degrees celsius.What is
the heat of solution of ammonium nitrate in kj/mol? Assume that the
specific heat capacity of the solution is 4.18 J/Cg and that no
heat is transferred to the surrounds or to the calorimeter.

The vapor pressure of water at 25 degrees Celsius is
23.76 mm of Hg; Kf for water is 1.86 (degree Celsius kg/mol). The
normal boiling point of chloroform is 61.0 degrees Celsius and Kb
is 3.63 (degree Celsius kg/mol) R=0.08206 (L atm/mol.k).
1. What is the vapor pressure of a solution on 10.0g of NaNO3 in
25.0g of water?
2. What is the freezing point of a 0.20 m
aqueous solution of sucrose at 1 atm pressure?
3. What is...

A solution is made by dissolving 23.2g of Chromium (II) nitrate,
CR(NO3)2, in enough water to make 250. ml of solution. Calculate
the molartity of each species:
Cr(NO3)2= mol/L
Cr^2+= mol/L
NO3- = mol/L

If 500 mL of a solution containing 5.01 x 10-3 moles of
magnesium nitrate, (Mg(NO3)2, is combined with 500 mL of a solution
containing 7.04 x 10-3 moles of sodium carbonate, (Na2CO3), will
there be a precipitate? (Magnesium carbonate has a Ksp value of
6.82 x10^6)
a. There will be no precipitate.
b. Magnesium nitrate will precipitate.
c. Magnesium carbonate will precipitate.
d. It is impossible to tell.
e. Sodium nitrate will precipitate.

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