Answer:
The answer to your question is [H₃O⁺] = 0.025 [OH⁻] = 3.98 x 10⁻¹³
Explanation:
Data
[H⁺] = ?
[OH⁻] = ?
pH = 1.6
Process
Use the pH formula to calculate the [H₃O⁺], then calculate the pOH and with this value, calculate the [OH⁻].
pH formula
pH = -log[H₃O⁺]
-Substitution
1.6 = -log[H₃O⁺]
-Simplification
[H₃O⁺] = antilog (-1,6)
-Result
[H₃O⁺] = 0.025
-Calculate the pOH
pOH = 14 - pH
-Substitution
pOH = 14 - 1.6
-Result
pOH = 12.4
-Calculate the [OH⁻]
12.4 = -log[OH⁻]
-Simplification
[OH⁻] = antilog(-12.4)
-Result
[OH⁻] = 3.98 x 10⁻¹³
Answer : The molar concentration of solution is 
Explanation :
Using Beer-Lambert's law :
where,
A = absorbance of solution = 0.614
C = molar concentration of solution = ?
l = path length = 1.0 cm
= molar absorptivity coefficient = 
(assume)
Now put all the given values in the above formula, we get:
Therefore, the molar concentration of solution is
Answer:
Argument: It is not Safe
Further support to the argument is given below.
Explanation:
Solution:
Argument: It is not Safe
First of all, we all know the ideal gas law:
PV = nRT
And the Boyle's Law states that , if the pressure is increased then, volume will decrease. and if the volume is increased then pressure will decrease.
V is inversely proportional to Pressure of the gas.
So, in this case, Let's suppose we have toxic solution of methyl alcohol in the bottle which is tightly closed. It means pressure in the bottle is high, hence the volume is less.
If in this scenario someone, leave the bottle open in the laboratory and as it is given that the level of solution will drastically decrease. It means it is volatile in nature and is converted into gaseous form and we know now that the open bottle has now less pressure. Hence the volume of the gas will be higher and now it can spread to every corner of the laboratory. And it is very dangerous.
<em>I think the answer to your question is increase.</em>
The vapor pressure of propanone is 56 degrees Celsius.
