Solve for it?show all work for me as well please ASAP!!
1 answer:
Answer: The pressure will be 411 GH.
Explanation:
To calculate the final pressure of the system, we use the equation given by Gay Lussac Law. This law states that pressure of the gas is directly proportional to the temperature of the gas at constant volume
Mathematically,
where,
are the initial pressure and temperature of the gas.
are the final pressure and temperature of the gas.
We are given:
Putting values in above equation, we get:
Thus the pressure will be 411 GH.
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Answer:
You need to weight 6,005 g of acetic acid
Explanation:
Using Henderson-Hasselbalch formula you will obtain:
5,00 = 4,76 +log₁₀
<em>Where Ac⁻ is the salt of acetic acid (Acac).</em>
Solving:
1,738 = <em>(1)</em>
Also, yo know that:
0,200 M = [Ac⁻] + [Acac] <em>(2)</em>
Replacing (2) in (1):
[Acac] = 0,0730 M.
Thus:
[Ac⁻] = 0,127 M
The moles of each compound are:
Acac = 0,0730 M × 0,500 L = <em>0,0365 mol</em>
Ac⁻ = 0,127 M × 0,500 L = <em>0,0635 mol</em>
To prepare these moles it is necessary to use:
Acac + NaOH → AcNa + H₂O
The initial moles of Acac must be:
0,0365 moles + 0,0635 moles = 0,100 moles
<em>To obtain 0,0635 moles of Ac⁻ you need to take this quantity of NaOH moles.</em>
Thus, to obtain a acetate buffer of 5,00 you need to add 0,100 moles of acetic acid and 0,0635 moles of NaOH because This NaOH will react with acetic acid producing 0,0635 moles of Ac⁻ and surplus 0,0365 moles of acetic acid.
Now, to obtain 0,100 moles of acetic acid from pure acetic acid:
0,100 moles × = <em>6,005 g</em>
<em>You need to weight 6,005 g of acetic acid</em>
I hope it helps!