A 17.4 L sample of oxygen gas (O2) was collected at a temperature of 23.0°C and a pressure of 2.18 atmospheres. What volume woul
1 answer:
The volume of the gas at STP = 35.01 L
<h3>Further explanation</h3>Conditions at T 0 ° C and P 1 atm are stated by STP (Standard Temperature and Pressure).
In general, the gas equation can be written
where
P = pressure, atm
V = volume, liter
n = number of moles
R = gas constant = 0.08206 L.atm / mol K
T = temperature, Kelvin
V=17.4 L
T = 23 + 273 = 296 K
P = 2.18 atm
The volume of the gas occupy at STP :
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Explanation:
(A) As we know that carbonic acid () and Sodium bicarbonate (
) forms an acidic buffer.
Therefore, pH of an acidic buffer is given by Hendeerson-Hasselbalch equation as follows.
pH = ........... (1)
So mathematically, if [Salt] = [Acid] then = 1
.
And, = 0
Therefore, equation (1) gives us the following.
pH = (when acid and salt are equal in concentration)
Hence, of
(carbonic acid) is 6.35.
And, with this we have following results.
In (A) and (D) we have the case \frac{[NaHCO_{3}]}{[H_{2}CO_{3}]}[/tex] i.e. [Salt] = [Acid].
Hence, for the cases pH = = 6.35.
(B) = 0.045 M and,
= 0.45 M
Hence, pH =
=
= 6.35 + (-1)
= 5.35
Therefore, it means that this buffer will be most suitable buffer as it has pH on acidic side and addition of slight excess base will not affect much of its pH value.
(C) = 0.45 M
= 0.045 M
So, pH =
=
= 6.35 + (+1)
= 7.35
This means that pH on Basic side makes it no more acidic buffer.