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loris [4]
3 years ago
7

15.0 mL of 0.050 M Ba(NO3)2 M and 100.0 mL of 0.10 M KIO3 are added together in a 250 mL erlenmeyer flask. In this problem, igno

re ionic strength effects and neglect the possible presence of any complex ions in solution. a. Will Ba(IO3)2 precipitate out of solution? Support your answer with appropriate calculations.
Chemistry
1 answer:
timama [110]3 years ago
5 0

Answer:

Yes, precipitation of barium iodate will occur.

Explanation:

Molarity of barium nitrate solution = 0.050 M

Volume of barium nitrate solution =15.0 mL = 0.0150 L

1 mL = 0.001 L

Moles of barium nitrate = n

n=0.050 M\times 0.0150L=0.00075 mol

Ba(NO_3)_2(aq)\rightarrow Ba^{2+}(aq)+2NO_3^{-}(aq)

Moles of barium ions: 1\times 0.00075 mol=0.00075 mol

Molarity of potassium iodate solution = 0.10 M

Volume of potassium iodate solution =100.0 mL = 0.1000 L

1 mL = 0.001 L

Moles of potassium iodate = n'

n'=0.10 M\times 0.1000 L=0.01 mol

KIO_3(aq)\rightarrow K^{+}(aq)+IO_3^{-}(aq)

Moles of iodate ions = 1\times 0.01 mol=0.01 mol

After mixing of both solution in 250 mL in erlenmeyer flask

Volume of the final solution = 250 mL = 0.250 L

Concentration of barium ions in 250 mL solution :

[Ba^{2+}]=\frac{0.00075 mol}{0.250 L}=0.003 M

Concentration of iodate ions:

[IO_3^{-}]=\frac{0.01 mol}{0.250 L}=0.04 M

Solubility product of barium iodate,K_{sp}=4.01\times 10^{-9}

Ionic product of the barium iodate in solution :K_i

Ba(IO_3)_2\rightleftahrpoons Ba^{2+}+2IO_3^{-}

K_i=[Ba^{2+}][IO_2^{-}]^2

K_i=0.003 M\times (0.04 M)^2=4.8\times 10^{-6}

K_{sp}  ( precipitation)

As we can see, the ionic product of the barium iodate is greater than the solubility product of the barium iodate precipitation of barium iodiate will occur in 250 mL of final solution.

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Calculate the boiling temperature of a 0.50 M solution of sucrose. Assume that the concentration is 0.50 m.
Ronch [10]
There is one missing point in the question.

The formula to find an increase in boiling Temperature is :

ΔT = kb x M

ΔT = is the increase in boiling Temperature
Kb = Boiling point constant of the Solvent
M = Molarity

You did not provide the Kb. If you have it, you just have to insert it to the formula to find the ΔT.


And assuming that the other solution is water, you just have to add it up with 100 Celcius


5 0
3 years ago
1 mole = 1000 millimoles (mmol); 1millimole = 1000 micromoles (µmol). if a solution contains 38231 µmol, what is that amount in
Mrrafil [7]
1 mmol --------------------- 1000 <span>µmol
( mmol ) -------------------- </span> 38231 µmol

mmol =  38231*1 / 1000

mmol = 38231/ 1000

=>  38.231 mmol
3 0
3 years ago
state the formula for potassium hydroxide and explain, in terms of charges, how you formed the formula
Ganezh [65]

Potassium oxide is an ionic compound. The potassium has a charge of <span>K+</span> and oxygen has a charge of <span>O<span>2−</span></span>. We need 2 potassium ions to balance one oxide ion making the formula <span><span>K2</span>O</span>.

Potassium hydroxide is an ionic compound. The potassium has a charge of <span>K+</span> and hydroxide has a charge of <span>OH−</span>. We need 1 potassium ion to balance one hydroxide ion making the formula KOH.

<span><span>K2</span>O+<span> H2</span>O→KOH</span>

To balance the equation we place a coefficient of 2 in front of the potassium hydroxide.

<span><span>K2</span>O+<span>H2</span>O→2KOH</span>

I hope this was helpful.

3 0
3 years ago
Chemist A burns 10.000 grams of C₂H₆ in a constant-volume container at 25ºC. Chemist B burns an unknown mass of C₂H₆ in a consta
alexandr1967 [171]

Answer:

10.000 grams

Explanation:

For the first law of thermodynamics, the energy must be conserved, that means that the energy in form of heat (Q) must be equal to the sum of work (W) and internal energy(ΔU) :

Q = W + ΔU

ΔU depends on the temperature and W in the variation of pressure and volume. Q depends on the temperature, but also the mass. So, there is the same temperature, ΔU is equal for both reaction, if there is no work done, the heat must be equal for both of them. So the mass such be the same.

5 0
3 years ago
The road map in the text shows that to convert from one unit to another, you must use the ____ as an intermediate step. ___ conv
jonny [76]

Answer:

Conversion factor;

Molar mass;

Avogadro's constant and molar mass

Explanation:

  • Firstly, an intermediate step is to define the conversion factor that will be then used in a conversion technique called dimensional analysis in order to convert from one unit to another. An example of a conversion factor would be, for example, 1 L = 1000 mL, which can be manipulated as a fraction, either \frac{1 L}{1000 mL} or \frac{1000 mL}{1 L};
  • Secondly, in order to convert mass to moles, we need to know the molar mass of a compound which has a units of g/mol (that is, it shows how many grams we have per 1 mole of substance.
  • Thirdly, Avogadro's constant, N_A = 6.022\cdot 10^{23} mol^{-1} tells us that there is N_A number of molecules or atoms in 1 mole of substance. We need two conversion factors to convert the number of molecules to a mass: firstly, we need to convert the number of molecules into the number of moles using Avogadro's constant and then we need to use the molar mass to convert the moles obtained into mass.
5 0
3 years ago
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