Chemistry problem. Is alcohol soluble in water?
1 answer:
You might be interested in
Before addition of HCl,
conc. of CH3COOH = 0.450 M
conc. of CH3COONa = 0.550 M
After addition of 0.08 M HCl, following reaction occurs in system:
HCl + CH3COONa ↔ CH3COOH + NaCl
Thus, in reaction system conc. of CH3COOH will increase to 0.53 M (0.08M + 0.450M)
And, conc to CH3COONa will reduce to 0.47 M (0.550M - 0.08M)
Now, conc. of H+ ions = ka![\frac{[acid]}{[conjugated base]}](https://tex.z-dn.net/?f=%20%5Cfrac%7B%5Bacid%5D%7D%7B%5Bconjugated%20base%5D%7D)
where ka = dissociation constant for acid = 10^-5 for Ch3COOH
∴ conc. of H+ ions =
= 1.1277 x 10^-5
Now, pH = -log [H+] = -log (1.1227 x 10^-5) = 4.94
conc. of CH3COOH = 0.450 M
conc. of CH3COONa = 0.550 M
After addition of 0.08 M HCl, following reaction occurs in system:
HCl + CH3COONa ↔ CH3COOH + NaCl
Thus, in reaction system conc. of CH3COOH will increase to 0.53 M (0.08M + 0.450M)
And, conc to CH3COONa will reduce to 0.47 M (0.550M - 0.08M)
Now, conc. of H+ ions = ka
where ka = dissociation constant for acid = 10^-5 for Ch3COOH
∴ conc. of H+ ions =
= 1.1277 x 10^-5
Now, pH = -log [H+] = -log (1.1227 x 10^-5) = 4.94
Answer:
Distillation
Explanation:
Miscible solvents are separated from each other through a process called as Distillation. This technique works on the principle of difference in the boiling point of the solvents that are forming the miscible solution.
Example:
Water and Ethanol are two miscible solvents. They have different boiling points.
Ethanol = 78.37 °C
Water = 100 °C
In a experimental setup attached below, water and ethanol mixture is taken in a round bottom flask and heated on a hotplate. Ethanol having less boiling point than water boils first and evaporates. The Ethanol vapors are condensed as they passes through the condenser. In this way the ethanol is separated first and water having greater boiling point is left behind.
