The answer is: 231.25 ppm.
To solve this, compute first the percentage of hydrogen in the 3.2 g air sample. % = (0.00074g/3.2g)*100 = 0.023125%
1% = 10,000ppm <--- use this as conversion factor.
0.023125%(10,000ppm/1%) = 231.25 ppm
Answer:
pH = 8.18
Explanation:
The weak base, X, reacts with HCl as follows:
X + HCl → HX⁺ + Cl⁻
<em>Where 1 mole of X with 1 mole of HCl produce 1 mole of HX⁺ (The conjugate acid of the weak base).</em>
Now, using H-H equation for bases:
pOH = pKb + log [XH⁺] / [X]
<em>Where pOH is the pOH of the buffer (pH = 14 -pOH)</em>
<em>pKb is -log Kb = 5.824</em>
<em>And [X] [HX⁺] are the molar concentrations of each specie</em>
Now, at the neutralization of the half of HX⁺, the other half is as X, that means:
[X] = [HX⁺]
And:
pOH = pKb + log [HX⁺] / [X]
pOH = 5.824 + log 1
pOH = 5.824
pH = 14-pOH
<h3>pH = 8.18</h3>
Answer:
its true i just looked on quizlet
Explanation: