You have 250.0 mL of 4.00 M sugar solution. You added 216.1 mL of water to this solution. Determine the concentration of the sug
1 answer:
Answer:
Explanation:
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In this case, since the dilution processes are characterized by the addition of extra solvent, in this case water, to an initial solution in order to decrease the concentration of the solute, in this case sugar; as water is added, the moles of sugar remain unchanged, so the following equation can be written:
Whereas 1 accounts for the initial 250.0 mL of 4.00 M sugar and 2 for the concentration at the new volume which is:
Thus, the final concentration is:
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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>
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