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alukav5142 [94]
3 years ago
12

Give the formula of the conjugate base of each of the following. (Type your answer using the format CO2 for CO2, (NH4)2CO3 for (

NH4)2CO3, [NH4]+ for NH4+, and [Ni(CN)4]2- for Ni(CN)42-.) (a) NH3
Chemistry
1 answer:
MissTica3 years ago
7 0

Answer:

a) [NH2]-,

b) [O]2-

c) [Cl]-

Explanation:

The conjugate base is the base member (X⁻) of a weak acid (HX). In other words, the conjugate base is the remaining substance due to the proton loss in the acid HX.

a) For NH₃, (HX; X: NH₂⁻), conjugate base is NH₂⁻. In the format, <em>[NH2]-</em>.

b) For OH⁻, (HX; X: O²⁻), conjugate base is O²⁻. In the format,<em> [O]2-</em>.

c) For HCl, (HX; X: Cl⁻), conjugate base is Cl⁻. In the format, <em>[Cl]-</em>.

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Consider two equal size rooms connected by an open door. One room is maintained at a higher temperature then the other one. Whic
patriot [66]

Answer:

  • The room mantained at a lower temperature will contain more air molecules.

Explanation:

1) Since the two rooms are <em>connected by an open door</em>, you assume pressure equilibrium: the pressure on the two rooms is the same.

2) Since you consider <em>two equal size rooms</em>, both volumes are equal.

3) Assuming ideal gas behavior, pressure (P), temperature (T), volume (V) and number of moles (n) are related by the equation PV = nRT

4) Naming T₁ the lower temperature, T₂ the higher temperature, n₁ the number of moles of air in the room at lower temperature, and n₂ the number of moles of air in the room at higher temperature, you get:

  • n₁ T₁  = n₂ T₂, or n₁ / n₂ = T₂ / T₁

5) That means that the amount of molecules (number of moles) is inversely related to the temperature: the higher the temperature the lower the number of moles, and the lower the temperature the greater the number of moles.

Hence, the answer is that <em>the room that contains more air molecules is the room mantained at a lower temperature.</em>

5 0
3 years ago
How much mercury and oxygen could be obtained from 21.7g of mercury (II) oxide
Musya8 [376]

20.06 g of Hg  and 1.6 g of O₂

<u>Explanation:</u>

To Find:

Number of Mercury and oxygen that can be obtained from 21.7 g of HgO

First we have to write the balanced equation for the decomposition reaction of Mercury(II) oxide as,

2 HgO (s) → 2Hg(l) + O₂ (g)

21.7 g of HgO  = \frac{21.7 g}{216.59  g / mol}  

                         = 0.1 mol of HgO.

As per the above equation, we can find the mole ratio between HgO and Hg is 1: 1 and that of HgO and oxygen is 2:1 .

So amount of Hg produced = 0.1 mol × 200.59 g / mol ( molar mass of Hg)

                                                 = 20.06 g of Hg

Amount of oxygen produced = 0.05  mol × 32 g/ mol = 1.6 g of O₂

Thus it is clear that 20.06 g of Hg  and 1.6 g of O₂  is obtained from 21.7 g of HgO

7 0
3 years ago
During a reaction in an aqueous solution, the concentration of bactants
STALIN [3.7K]

Answer:

my define it will be turst me is c

5 0
3 years ago
In a solution of pure water, the dissociation of water can be expressed by the following: H2O(l) + H2O(l) ⇌ H3O+(aq) + OH−(aq) T
kakasveta [241]

Answer:

  • [H₃O⁺] = 2.90 × 10⁻¹⁰ M

Explanation:

1)<u><em> Ionization equilibrium equation: given</em></u>

  • H₂O(l) + H₂O(l) ⇌ H₃O⁺(aq) + OH⁻(aq)

2) <em><u>Ionization equilibrium constant, at 25°C, Kw: given</u></em>

  • Kw = 1.0 × 10⁻¹⁴

<u>3) Stoichiometric mole ratio:</u>

As from the ionization equilibrium equation, as from the fact it is stated, the concentration of both ions, at 25°C, are equal:

  • [H₃O⁺(aq)] = [OH⁻(aq)] = 1.0 × 10⁻⁷ M

  • ⇒ Kw = [H3O⁺] [OH⁻] = 1.0 × 10⁻⁷  × 1.0 × 10⁻⁷  = 1.0 × 10⁻¹⁴ M

<u><em>4) A solution has a [OH⁻] = 3.4 × 10⁻⁵ M at 25 °C </em></u><em><u>and you need to calculate what the [H₃O⁺(aq)] is.</u></em>

Since the temperature is 25°, yet the value of Kw is the same, andy you can use these conditions:

  • Kw = 1.0 × 10⁻¹⁴ M², and

  • Kw = [H3O⁺] [OH⁻]

Then you can substitute the known values and solve for the unknown:

  • 1.0 × 10⁻¹⁴ M² = [H₃O⁺] × 3.4 × 10⁻⁵ M

  • ⇒ [H₃O⁺]  = 1.0 × 10⁻¹⁴ M² / ( 3.4 × 10⁻⁵ M ) = 2.9⁻¹⁰ M

As you see, the increase in the molar concentration of the ion [OH⁻] has caused the decrease in the molar concentration of the ion [H₃O⁺], to keep the equilibrium law valid.

6 0
3 years ago
Read 2 more answers
ASAP MULTIPLE CHOICE
OleMash [197]
The mass of electrons , i just did the same test and got it right
7 0
3 years ago
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