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s2008m [1.1K]
2 years ago
13

You mix a 110.0 −mL sample of a solution that is 0.0133 M in NiCl2 with a 200.0 −mL sample of a solution that is 0.250 M in NH3.

After the solution reaches equilibrium, what concentration of Ni2+(aq) remains?
The value of Kf for Ni(NH3)62+ is 2.0×10^{8} .
Chemistry
1 answer:
love history [14]2 years ago
7 0

Based on the data provided, at equilibrium, the concentration of Ni2+ that remains is 4.268 ×10^-6 M

<h3>What is molar concentration of a solution?</h3>

The molar concentration of a solution is the amount in moles of solute dissolved in a given volume of solution in litres.

  • Molar concentration = moles/volume in Litres

Total volume of solution after mixing = 110 + 200 = 310 mL

Concentration of Ni2+ = 0.0133M/( 310ml/110ml) = 0.00472M

Concentration of NH3 = 0.250M/(310ml/200ml) = 0.1613 M

Assuming complete formation of Ni(NH3)6, the equation of formation is given as:

  • Ni2+(aq) + 6NH3(aq) -------> Ni(NH3)62+ (aq)

From equation of the reaction, 1 mole of Ni2+ reacts with 6 moles of NH3 to produce 1 mole of Ni[(NH3)6]2+

Then,

0.00472 M of Ni2+ react with 0.02832 M of NH3 to give 0.00472 M of Ni2+

Concentration of remaining NH3 = 0.1613 M - 0.02832M = 0.13298 M

The equation of dissociation at equilibrium of Ni(NH3)62+ is given as:

  • Ni[(NH3)6]2+(aq) <-------> Ni2+(aq) + 6NH3(aq)

Kd = [Ni2+][NH3]6/[Ni(NH3)6]

Kd = 1/Kf = 1/ 2.0 × 10^8

Kd = 5.0 ×10^-9

Using an ICE chart;

Initial concentration:

[Ni(NH3)62+] = 0.00472

[Ni2+] = 0

[NH3] = 0.

Change in concentration:

[Ni(NH3)62+] = - x

[Ni2+] = + x

[NH3] = + 6x

Equilibrium concentration:

[ Ni(NH3)62+] = 0.00472 - x

[Ni2+] = x

[NH3] = 0.13298 + 6x

From the dissociation constant equation;

x(0.1330 + 6x)^6 / 0.00472 - x) = 5.0 ×10^-9

Assuming x is very small;

  • 0.13298 + 6x = 0.13298
  • 0.00472 - x = 0.00472

x( 0.13298)^6/ 0.00472 = 5.0 ×10^-9

x × 0.00117= 5.0 ×10^-9

x = 4.268 ×10^-6 M

Therefore, at equilibrium, the concentration of Ni2+ that remains is 4.268 ×10^-6 M

Learn more about molar concentration at: brainly.com/question/26255204

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Which type of carbon fixation stores carbon dioxide in acid form? a. c3 b. c4 c. cam d. all of the above
Luba_88 [7]

The type of carbon fixation stores carbon dioxide in acid form is CAM i.e. crassulacean acid metabolism.

<h3>What are CAM?</h3>

CAM stands for crassulacean acid metabolism in this process photosynsthesis is occured at day time but the exchange of gases takes place at night itself only.

In this carbon fixation process, carbon dioxide is stored in the form of organic acid malic acid and losses carbon dioxide at the night time and by doing this it helps in the storage of water.

Hence option (C) is correct.

To know more about CAM, visit the below link:

brainly.com/question/4170802

8 0
2 years ago
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I need somebody to help me with my homework pls i dont get it .
zubka84 [21]
26. B
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7 0
3 years ago
What information do we need to determine the molecular formula of a compound from the empirical formula?
defon

Answer:

Molecular mass

Explanation:

Molecular formulas is the actual number of atoms of each element in the compound while empirical formulas is the simplest or reduced ratio of the elements in the compound.

Thus,  

Molecular mass = n × Empirical mass

Where, n is any positive number from 1, 2, 3...

Thus if the molecular mass is known, then we can find the value of n which results to molecular formula.

6 0
3 years ago
What does a chemical bond results from a rearrangement of?
Dmitriy789 [7]

Atoms

Explanation:

Chemical bonds results from the rearrangement of atoms in a chemical species.

It deals with the various attractive forces joining chemical species togethe.

  • When atoms are re-arranged, they form chemical bonds that leads to production of new compounds.
  • This is made possible by the exchange or sharing of electrons.
  • The driving force for most interatomic bonding is the tendency to have completely filled outer energy levels like the noble gases.
  • When atoms are re-arranged in compounds they lead to the production of chemical bonds.

learn more:

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5 0
3 years ago
How many grams of solid nickel will be plated if an aqueous nickel(II) sulfate solution is electroplated over 10.5 min with a co
Anna71 [15]

Answer:

613 mg

Explanation:

$Ni^{2+} + 2e \rightarrow Ni(s)$

Number of fargday's  $=\frac{It}{96500}$

Here, I = 9.20 A

        t = 10.5 min

          = 10.5 x 60 seconds

So, $\frac{It}{96500}$

  $=\frac{3.20 \times 10.5 \times 60}{96500}$

 = 0.0208 F

Here, 2e, 2F

2F = 1 mol of Ni

$0.0208 \ F = \frac{0.0208}{2} = 0.0104 \ mol \ Ni$

1 mol = 59 gm of Ni

0.0104 mol = 59 x0.0104 gm Ni

                    = 0.613 gm Ni

                    = (0.613 x 1000 ) mg of Ni

                    = 613 mg of Ni

3 0
2 years ago
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