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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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GrogVix [38]

Answer:

0.200 m K3PO3

Explanation:

Let us remember that the freezing point depression is obtained from the formula;

ΔTf = Kf m i

Where;

Kf = freezing point constant

m = molality

i = Van't Hoff factor

The  Van't Hoff factor has to do with the number of particles in solution. Let us consider the  Van't Hoff factor for each specie.

0.200 m HOCH2CH2OH - 1

0.200 m Ba(NO3)2 - 3

0.200 m K3PO3 - 4

0.200 m Ca(CIO4)2 - 3

Hence, 0.200 m K3PO3 has the greatest van't Hoff factor and consequently the greatest freezing point depression.

8 0
3 years ago
Charle's Law
Setler [38]

Convert temperature to Kelvin

  • 225°C=498K
  • 127°C=400K

Convert vol to L

  • 400mL=0.4L

Apply Charles law

  • V1T_2=V2T_1
  • 0.4(400)=498V_2
  • 160=498V_2
  • V_2=0.32L=320mL
8 0
2 years ago
Read 2 more answers
What is the number of oxygen atoms in 32grams of the gas​
Lady bird [3.3K]

One mole of oxygen gas, which has the formula O2, has a mass of 32 g and contains 6.02 X 1023 molecules of oxygen but 12.04 X 1023 (2 X 6.02 X 1023) atoms, because each molecule of oxygen contains two oxygen atoms.

7 0
2 years ago
13. What is the total pressure inside the container​
nasty-shy [4]

<u>Answer:</u> The total pressure inside the container is 77.9 kPa

<u>Explanation:</u>

Dalton's law of partial pressure states that the total pressure of the system is equal to the sum of partial pressure of each component present in it.

To calculate the total pressure inside the container, we use the law given by Dalton, which is:

P_T=p_{N_2}+p_{O_2}+p_{Ar}

We are given:

Vapor pressure of oxygen gas, p_{O_2} = 40.9 kPa

Vapor pressure of nitrogen gas, p_{N_2} = 23.3 kPa

Vapor pressure of argon, p_{Ar} = 13.7 kPa

Putting values in above equation, we get:

p_T=23.3+40.9+13.7\\\\p_{T}=77.9kPa

Hence, the total pressure inside the container is 77.9 kPa

7 0
3 years ago
Help?
Ahat [919]

Answer:

KClO_3

Explanation:

Hello!

In this case, as we know the mass of the total sample, we can first compute the mass of oxygen:

m_O=22.9g-7.33g-6.65g=8.92g

Next, we compute the moles of each element:

n_K=\frac{7.33g}{39.9g/mol}= 0.184mol\\\\n_{Cl}=\frac{6.65g}{35.45g/mol}=0.188mol \\\\n_O=\frac{8.92g}{16.00g/mol} =0.5575mol

Now, we divide the moles by 0.184 moles, the fewest ones, to obtain:

K=\frac{0.184}{0.184}=1.0 \\\\Cl=\frac{0.187}{0.184}=1.0\\\\O=\frac{0.5575}{0.184}  =3.0

Therefore, the empirical formula is:

KClO_3

Regards!

3 0
2 years ago
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