Choose the species that is incorrectly matched with its electronic geometry.
1 answer:
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Answer:
15.9 g
Explanation:
(Take the atomic mass of C=12.0, H=1.0, O=16.0)
no. of moles = mass / molar mass
no. of moles of octane used = 11.2 / (12.0x8 + 1x18)
= 0.0982456 mol
Since oxygen is in excess and octane is the limiting reagent, the no. of moles of H2O depends on the no. of moles of octane used.
From the balanced equation, the mole ratio of octane : water = 2:18 = 1: 9,
so this means, one mole of octane produced 9 moles of water.
Using this ratio, we can deduce that (y is the no. of moles of water produced):
y = 0.0982456x9
y= 0.88421 mol
Since mass = no. of moles x molar mass,
mass of water produced = 0.88421 x (1.0x2+16.0)
=15.9 g
Answer:
A) pH of the buffer is 3.44
B) pH of the buffer solution is 3.37
Explanation:
Relation between K_{a} and pK_{a} is as follows.
.
The relation between pH and pK_{a} is as follows.
pH of the buffer is 3.44.
b)
mol of HCl added = 11.6M *0.001 L = 0.0116 mol
In the given reaction, will react with
to form
No. of moles of
And, no. of moles of
= 0.12 mol
after the reaction :
No. of moles of = moles present initially - moles added
= (0.15 - 0.0116) mol
= 0.1384 mol
Moles of = moles present initially + moles added
= (0.12 + 0.0116)
= 0.1316 mol
As,
Since, volume is both in numerator and denominator, we can use mol instead of concentration.
= 3.347+ log {0.1384/0.1316}
= 3.369
≅ 3.37
pH after the addition of 1.00 mL of 11.6 M HCl to 1.00 L of the buffer solution is 3.37