Answer:
6.7970 g
Explanation:
Considering the Henderson- Hasselbalch equation for the calculation of the pOH of the basic buffer solution as:
pOH = pK + log[acid] / [base]
Where K is the dissociation constant of the base.
Base dissociation constant of the ammonia = 1.8×10⁻⁵
pK = - log (Kb) = - log (1.8×10⁻⁵) = 4.75
Given concentration of base = [base] = 0.273 M
pH = 10.150
pOH = 14 - pH = 14 - 10.150 = 3.85
So,
3.85 = 4.75 + log[acid]/0.273
[Acid] = 0.0347 M
Given that Volume = 2 L
So, Moles = Molarity × Volume
Moles = 0.0347 × 2 = 0.0694 moles
Molar mass of ammonium bromide = 97.94 g/mol
Mass = Moles × Molar mass = (0.00775 × 97.94) g = 6.7970 g
Answer:
Sure I'll help you!
Explanation:
The head of the nail is flat and isn't sharp enough to cut anything, If you stab someone with a sword then hit them with a shield would it have the same effect? Of course not.
Explanation and answer:
The molar volume of a gas is 22.4 L at 0 deg. C.
So the molar mass of the gas is, by proportion,
0.16 g * (22400 mL)/(240 mL) = 14.93 g
The molar mass of (CH4)n = 12+4(1) = 16.
So n = 15.93/16 = 1, or the molecular formula is CH4.
Note: The temperature at which the volume was observed was not given. If 240 cm^3 was observed at 20 deg.C, then the volume at 0 deg.C would be
V=240*(273+0)/(273+20) = 223.6
The molar mass = 0.16*22400/(223.6) = 16.03
which gives n = 16/16.03 = 1 again, but more accurately.
Answer:
always repeats the same unit
made of smaller molecules
often made from repeating units