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Afina-wow [57]
3 years ago
14

Which statement best relates the strength and concentration of a base? At high enough concentrations, a weak base becomes strong

. Even at low concentrations, a strong base is strong. A weak base always has a low concentration. The stronger the base, the higher its concentration.
Chemistry
2 answers:
Lorico [155]3 years ago
6 0

Answer: Option (b) is the correct answer.

Explanation:

When there are more number of hydroxide ions in a solution then there will be high concentration of OH^{-} or hydroxide ions. As a result, more will be the strength of base in that particular solution.

A base is strong when it readily dissociate into its ions in the solution. When a base is strong, then it does not matter at what concentration it is dissolved in the solution because despite of its low concentration it will remain a strong base.

Thus, we can conclude that out of the given options, the statement even at low concentrations, a strong base is strong best relates the strength and concentration of a base.


Anna35 [415]3 years ago
4 0
I think that right annswer for this question is statement number two.
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Xenon (xe) of mass 5.08 g reacts with fluorine to form 9.49 g of a xenon fluoride compound. what is the empirical formula of thi
jenyasd209 [6]
We are already given with the mass of the Xe and it is 5.08 g. We can calculate for the mass of the fluorine in the compound by subtracting the mass of xenon from the mass of the compound.

  mass of Xenon (Xe) = 5.08 g
  mass of Fluorine (F) = 9.49 g - 5.08 g = 4.41 g

Determine the number of moles of each of the element in the compound. 
    moles of Xenon (Xe) = (5.08 g)(1 mol Xe / 131.29 g of Xe) = 0.0387 mols of Xe
   moles of Fluorine (F) = (4.41 g)(1 mol F/ 19 g of F) = 0.232 mols of F

The empirical formula is therefore,
      Xe(0.0387)F(0.232)
Dividing the numerical coefficient by the lesser number.
<em>     XeF₆</em>
8 0
3 years ago
How many mole of fe203 are in 233g og the compound
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The answer to this question
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3 0
3 years ago
How do you scale a recipe by changing the portion size
Elina [12.6K]

Answer:

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The ionization energy of silver is 731 kJ/mol. Is light with a wavelength of 415 nm sufficient to remove an electron from a silv
sineoko [7]

The energy of the light with a wavelength of 415 nm is not sufficient to remove an electron from a silver atom in the gaseous phase.

<h3>Energy and wavelength of light</h3>

The energy and wavelength of light are related by the formula given below:

  • Energy = hc/λ
  • where, E = energy
  • h = Planck's constant
  • c = velocity of light
  • λ = wavelength of light

<h3>Calculating the energy of the light</h3>

From the data provided:

  • h = 6.63 × 10^-34 Js
  • c = 3.0 × 10^8 m/s
  • λ = 415 nm = 4.15 × 10^-7 m

E = (6.63 × 10^-34 × 3.0 × 10^8 m/s)/4.15 × 10^-7 m

E = 4.79 × 10^-19 J

Energy of light is 4.79 × 10^-19 J

Compared with the ionization energy of silver, the energy of the light is far less.

Therefore, the energy of the light with a wavelength of 415 nm is not sufficient to remove an electron from a silver atom in the gaseous phase.

Learn more about about ionization energy and energy of light at: brainly.com/question/14596067

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