A box contains equal amounts of helium, argon, and krypton (all gases) at 25 ∘c. part a consider the temperatures, masses, avera
2 answers:
The common things in all gases are temperature, average kinetic energy, and average velocities. The different thing about the gases is their masses.
Further explanation:
The given gases are helium, argon, and krypton. It is also given in the question that all gases are in equal amount. The temperature of the box containing all gases is 25 oC.
Common in all gases:
Temperature: Since all gases are in the box at temperature 25 oC, therefore, the temperature is the same for all gases.
Average kinetic energy: The average kinetic energy of the gas is given as,
Here, <em>K</em> is average kinetic energy, <em>R</em> is a gas constant, is an Avogadro’s number, and <em>T</em> is temperature (in Kelvin)
Since the average kinetic energy is only related to temperature and temperature of all gases is the same, and therefore, average kinetic energy is also the same for all gases.
Average velocities: Average velocity of gases is directly related to the kinetic energy and temperature of gases thus the average velocity is also the same for all gases.
Different in all gases:
Mass: The given quantity of gases is the same. This means the number of particle of each gas present in the box is same. But the mass of each gas is different because the molar mass of each gas is different.
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Answer details:
Grade: Senior School
Subject: Chemistry
Chapter: Ideal gas equation
Keywords: Ideal gas, helium, argon, krypton, temperature, masses, average velocities, average kinetic energy, gas in the mixture.
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Answer :
The correct answer for Mass of Na₂HPO₄ = 4.457 g and mass of NaH₂PO₄ = 8.23 g
Given : pH = 6.86
Total concentration of Phosphate buffer = 0.1 M
Asked : Mass of Sodium phosphate monobasic (NaH₂PO₄) = ?
Mass of Sodium phosphate dibasic(Na₂HPO₄)= ?
Following steps can be done to find the masses of NaH₂PO₄ and Na₂HPO₄ :
(In phosphate buffer , Na+ ion from NaH₂PO₄ and Na₂HPO₄ acts as spectator ion , so only H₂PO₄⁻ and HPO₄²⁻ will be considered )
<u>Step 1 : To find pka </u>
H₂PO₄⁻ <=> HPO₄²⁻
The above reaction has pka = 7.2 ( from image shown )
<u>Step 2 : Plug values in Hasselbalch- Henderson equation </u>.
Hasselbalch -Henderson equation is to find pH for buffer solution which is as follows :
pH = 6.86 pKa = 7.2
Subtracting both side by 7.2
Removing log
---------------- equation (1)
<u>Step 3 : To find molarity of H₂PO₄⁻ and HPO₄²⁻</u>
Total concentration of buffer = [H₂PO₄⁻] + [HPO₄²⁻] = 0.1 M
Hence, [H₂PO₄⁻ ] + [ HPO₄²⁻ ] = 0.1 M
Assume [H₂PO₄⁻ ] = x
So , [x ] + [ HPO₄²⁻ ] = 0.1 M
[ HPO₄²⁻ ] = 0.1 - x
Step 4 : Plugging value of [H₂PO₄⁻ ] and [ HPO₄²⁻ ]
[H₂PO₄⁻ ] = x
[ HPO₄²⁻ ] = 0.1 - x
Equation (1) = >
Plug value of [H₂PO₄⁻ ] and [ HPO₄²⁻ ] ( from step 3 ) into equation (1) as :
Cross multiplying
Adding x on both side
Dividing both side by 1.457
x = 0.0686 M
Hence , [H₂PO₄⁻ ] = x = 0.0686 M
[ HPO₄²⁻ ] = 0.1 - x
[ HPO₄²⁻ ] = 0.1 - 0.0686
[ HPO₄²⁻ ] = 0.0314 M
Step 5 : To find moles of H₂PO₄⁻ ( NaH₂PO₄) and HPO₄²⁻ (Na₂HPO₄ ) .
Molarity is defined as mole of solute per 1 L volume of solution .
Molarity of NaH₂PO₄ = 0.0686 M or 0.0686 mole per 1 L
Molarity of Na₂HPO₄ = 0.0314 M or 0.0314 mole per 1 L
Since that volume of buffer solution is 1 L , so Molarity = mole
Hence Mole of NaH₂PO₄ = 0.0686 mol
Mole of Na₂HPO₄ = 0.0314 mol
<u>Step 6 : To find mass of Na₂HPO₄ and NaH₂PO₄ </u>
Moles of Na₂HPO₄ and NaH₂PO₄ can be converted to their masses using molar mass as follows :
Molar mass of Na₂HPO₄ =
Molar mass of NaH₂PO₄ =
Mass of Na₂HPO₄ = 4.457 g
Mass of NaH₂PO₄ = 8.23 g
Answer : The solubility of in water is,
Explanation :
The solubility equilibrium reaction will be:
Let the molar solubility be 's'.
The expression for solubility constant for this reaction will be,
Given:
=
Now put all the given values in the above expression, we get:
Therefore, the solubility of in water is,