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Svetach [21]
3 years ago
11

Give the conjugate base for each compound below.? Acid --- Conjugate Base H2S _________ HPO4^-2 _________ NH4+ _________ Update:

Give the conjugate acid for each compound below? Base ---- Conjugate Acid HSO4- _______ SO4^-2 _______ NH3 _______
Chemistry
2 answers:
zhenek [66]3 years ago
8 0
 <span>take away one proton from the acid to give its conjugate base. So 

HS- 

PO4^3- 

NH3</span>
svetlana [45]3 years ago
6 0

According to  Bronsted-Lowry theory acid are donor of protons and bases are acceptors of protons (the hydrogen cation or H⁺).

When acid lost proton, it forms conjugate base and when base gain proton it form conjugate acid.

1) Answer is: HS⁻.

Chemical reaction (dissotiation) : H₂S(aq) → HS⁻(aq) + H⁺(aq).

2) Answer is: PO₄³⁻.

Chemical reaction (dissotiation) : HPO₄²⁻(aq) → PO₄³⁻(aq) + H⁺(aq).

3) Answer is: NH₃.

Chemical reaction (dissotiation) : NH₄⁺(aq) → NH₃(aq) + H⁺(aq).

4) Answer is: H₂SO₄.

Chemical reaction: HSO₄⁻(aq) + H⁺(aq) → H₂SO₄(aq).

5) Answer is: HSO₄⁻.

Chemical reaction: SO₄²⁻(aq) + H⁺(aq) → HSO₄⁻(aq).

6) Answer is: NH₄⁺.

Chemical reaction: NH₃(aq) + H⁺(aq) → NH₄⁺(aq).

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Explanation:

5 0
3 years ago
24 g of magnesium were burned in oxygen. The compound formed had a mass of 40 g. Explain why the mass had gone up.
DIA [1.3K]

Answer :

According to the law of conservation of mass, the mass of reactants must be equal to the mass of products.

The balanced chemical reaction is,

Mg+\frac{1}{2}O_2\rightarrow MgO

As we know that the molar mass of magnesium is 24 g/mole, the molar mass of O_2 is 32 g/mole and the molar mass of magnesium oxide is 40 g/mole.

From the given balanced reaction, we conclude that

As, 1 mole of magnesium react \frac{1}{2} mole of oxygen to give 1 mole of magnesium oxide.

So, the mass of Mg is 24 g, the mass of O_2=\frac{1}{2}\times 32=16g and the mass of MgO is 40 g.

That means 24 g of Mg react with 16 g O_2 to give 40 g of MgO.

8 0
3 years ago
Calculate the solubility of o2 in water at a partial pressure of o2 of 120 torr at 25 ̊c. the henry's law constant for o2 at 25
Vladimir79 [104]

Answer:

1) 2.054 x 10⁻⁴ mol/L.

2) Decreasing the temperature will increase the solubilty of O₂ gas in water.

Explanation:

1) The solubility of O₂ gas in water:

  • We cam calculate the solubility of O₂ in water using Henry's law: <em>Cgas = K P</em>,
  • where, Cgas is the solubility if gas,
  • K is henry's law constant (K for O₂ at 25 ̊C is 1.3 x 10⁻³ mol/l atm),
  • P is the partial pressure of O₂ (P = 120 torr / 760 = 0.158 atm).
  • Cgas = K P = (1.3 x 10⁻³ mol/l atm) (0.158 atm) = 2.054 x 10⁻⁴ mol/L.

2) The effect of decreasing temperature on the solubility O₂ gas in water:

  • Decreasing the temperature will increase the solubilty of O₂ gas in water.
  • When the temperature increases, the solubility of O₂ gas in water will decrease because the increase in T will increase the kinetic energy of gas particles and increase its motion that will break intermolecular bonds and escape from solution.
  • Decreasing the temperature will increase the solubility of O₂ gas in water will because the kinetic energy of gas particles will decrease and limit its motion that can not break the intermolecular bonds and increase the solubility of O₂ gas.


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