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Dovator [93]
3 years ago
6

Magnesium hydroxide is used in several antacid formulations. When it is added to water it dissociates into magnesium and hydroxi

de ions. Mg(OH)2(s) Mg2+(aq) + 2OH-(aq) The equilibrium constant at 25°C is 8.9 ´ 10-12. One hundred grams of magnesium hydroxide is added to 1.00 L of water and equilibrium is established. What happens to the solution if another 10 grams of Mg(OH)2 are now added to the mixture?
Chemistry
1 answer:
Sloan [31]3 years ago
5 0

Answer:

If you add 10 more grams of Mg(OH)₂, the solution will shift the equilibrium to the ions production to consume the excessive Mg(OH)₂.

Explanation:

Mg(OH)₂(s) → Mg²⁺(aq) + 2OH⁻(aq)

K = 8.9 x 10⁻¹²

K = [Mg²⁺][OH⁻]²

The concentration of Mg(OH)₂ does not enter the equation because it is in the solid state.

[Mg²⁺] = x

[OH⁻]²  = 2x

K = x.(2x)²

K = 4x³

4x³ =  8.9 x 10⁻¹²

x = 2.07 x 10⁻⁴ mol/L

At equilibrium:

[Mg²⁺] = x = 2.07 x 10⁻⁴ mol/L

[OH⁻]²  = 2x = 4.14 x 10⁻⁴ mol/L

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Which of the following acts as a catalyst in your body? A. Sweat B. Enzymes C. Blood cells D. Sugar
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3 years ago
Nitrogen gas reacts with hydrogen gas to produce ammonia. How many liters of hydrogen gas at 95kPa and 15∘C are required to prod
viktelen [127]

Answer:

222.30 L

Explanation:

We'll begin by calculating the number of mole in 100 g of ammonia (NH₃). This can be obtained as follow:

Mass of NH₃ = 100 g

Molar mass of NH₃ = 14 + (3×1)

= 14 + 3

= 17 g/mol

Mole of NH₃ =?

Mole = mass /molar mass

Mole of NH₃ = 100 / 17

Mole of NH₃ = 5.88 moles

Next, we shall determine the number of mole of Hydrogen needed to produce 5.88 moles of NH₃. This can be obtained as follow:

N₂ + 3H₂ —> 2NH₃

From the balanced equation above,

3 moles of H₂ reacted to produce 2 moles NH₃.

Therefore, Xmol of H₂ is required to p 5.88 moles of NH₃ i.e

Xmol of H₂ = (3 × 5.88)/2

Xmol of H₂ = 8.82 moles

Finally, we shall determine the volume (in litre) of Hydrogen needed to produce 100 g (i.e 5.88 moles) of NH₃. This can be obtained as follow:

Pressure (P) = 95 KPa

Temperature (T) = 15 °C = 15 + 273 = 288 K

Number of mole of H₂ (n) = 8.82 moles

Gas constant (R) = 8.314 KPa.L/Kmol

Volume (V) =?

PV = nRT

95 × V = 8.82 × 8.314 × 288

95 × V = 21118.89024

Divide both side by 95

V = 21118.89024 / 95

V = 222.30 L

Thus the volume of Hydrogen needed for the reaction is 222.30 L

8 0
3 years ago
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