The pH of the solution in which one normal adult dose aspirin is dissolved is : 2.7
Given data :
mass of aspirin = 640 mg = 0.640 g
volume of water = 10 ounces = 0.295735 L
molar mass of aspirin = 180.16 g/mol
moles of aspirin = mass / molar mass = 0.00355 mol
<h3>Determine the pH of the solution </h3>
First step : <u>calculate the concentration of aspirin</u>
= moles of Aspirin / volume of water
= 0.00355 / 0.295735
= 0.012 M
Given that pKa of Aspirin = 3.5
pKa = -logKa
therefore ; Ka =
= 
From the Ice table
=
=
given that the value of Ka is small we will ignore -x
x² =
x =
Therefore
[ H⁺ ] =
given that
pH = - Log [ H⁺ ]
= - ( -3 + log 1.948 )
= 2.71 ≈ 2.7
Hence we can conclude that The pH of the solution in which one normal adult dose aspirin is dissolved is : 2.7
Learn more about Aspirin : brainly.com/question/2070753
this is beta decay as the mass number stays the same but proton number changes, this is specifically beta minus as a neuron changes into a proton
Answer: I think that you have to find it in your lesson
Explanation:
Yes because obviously some other organism lives off eating that organism so if they die off the other organisms will be affected heavily
Answer:
P = 0.6815 atm
Explanation:
Pressure = 754 torr
The conversion of P(torr) to P(atm) is shown below:
So,
Pressure = 754 / 760 atm = 0.9921 atm
Temperature = 294 K
Volume = 3.1 L
Using ideal gas equation as:
PV=nRT
where,
P is the pressure
V is the volume
n is the number of moles
T is the temperature
R is Gas constant having value = 0.0821 L.atm/K.mol
Applying the equation as:
0.9921 atm × 3.1 L = n × 0.0821 L.atm/K.mol × 294 K
⇒n of helium gas= 0.1274 moles
Surface are = 1257 cm²
For a sphere, Surface area = 4 × π × r² = 1257 cm²
r² = 1257 / 4 × π ≅ 100 cm²
r = 10 cm
The volume of the sphere is :
Where, V is the volume
r is the radius
V = 4190.4762 cm³
1 cm³ = 0.001 L
So, V (max) = 4.19 L
T = 273 K
n = 0.1274 moles
Using ideal gas equation as:
PV=nRT
Applying the equation as:
P × 4.19 L = 0.1274 × 0.0821 L.atm/K.mol × 273 K
<u>P = 0.6815 atm</u>
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