Answer:
The resonance structure for the cyclopentadienyl anion is shown in the drawing below.
Explanation:
The resonance representation of the cyclopentadienyl anion shows that it is a stable ion. On the other hand it is important to note that it has 6 π electrons and is aromatic.
Element Symbol Atomic Mass
Barium Ba 137.327
Hydrogen H 1.00794
Oxygen O 15.9994
Hope this helps, good luck
Answer:
a. H₂S(aq) + H₂O(l) ⇄ HS⁻(aq) + H₃O⁺(aq)
b. NH₄⁺(aq) + H₂O(l) ⇄ NH₃(aq) + H₃O⁺(aq)
Explanation:
According to Bronsted-Lowry acid-base theory,
- An acid is a substance that donates a H⁺.
- A base is a substance that accepts a H⁺.
a. When dissolved in water, H₂S behaves as an acid according to the following equation.
H₂S(aq) + H₂O(l) ⇄ HS⁻(aq) + H₃O⁺(aq)
b. When dissolved in water, NH₄⁺ behaves as an acid according to the following equation.
NH₄⁺(aq) + H₂O(l) ⇄ NH₃(aq) + H₃O⁺(aq)
The mass of salt dissolved in 1.0 L of 0.010 M SO₄²⁻ is 0.67 g/l
<h3>How can we Calculate the mass of the salt dissolve in 1.0 L of 0.010 M SO₄²⁻ ?</h3>
To calculate the mass of the salt dissolved, we multiply by the mass of 1 mole to molar solubilty and lets assume we are using the anhydrous salt CaSO₄ for which the Molar Mass (M) = 136.1
Mass of the salt dissolved = Molar solubility x Molar mass
Molar Mass (M) = 136.1
Molar solubility = ?
Formula to find molar solubilty ;
Molar solubility = Square root of Solubity product (Given)
S = 
(Value of Solubity product is given in the question)
= 4.9 × 10⁻³
Mass of the salt dissolved = Molar solubility x Molar mass
= 4.9 × 10⁻³ x 136.1
= 0.67 g/l
Learn more about Solubility here ;
brainly.com/question/8591226
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Answer:
1.2 M
1.2 m
Explanation:
There is some info missing. I think this is the original question.
<em>A student dissolves 5.1g of ammonia (NH₃) in 250 mL of a solvent with a density of 1.02 g/mL. The student notices that the volume of the solvent does not change when the ammonia dissolves in it. Calculate the molarity and molality of the student's solution. Round both of your answers to 2 significant digits.</em>
<em />
Molarity
The molar mass of ammonia is 17.03 g/mol. The moles corresponding to 5.1 grams is:
5.1 g × (1 mol/17.03 g) = 0.30 mol
The volume of the solution is equal to the volume of the solvent, 250 mL or 0,250 L.
The molarity of ammonia is:
M = moles of solute / liters of solution
M = 0.30 mol / 0.250 L
M = 1.2 M
Molality
The density of the solvent is 1.02 g/mL. The mass corresponding to 250 mL is:
250 mL × 1.02 g/mL = 255 g = 0.255 kg
The molality of ammonia is:
m = moles of solute / kilograms of solvent
m = 0.30 mol / 0.255 kg
m = 1.17 m ≈ 1.2 m
