Answer:
The answer to your question is [H₃O⁺] = 0.025 [OH⁻] = 3.98 x 10⁻¹³
Explanation:
Data
[H⁺] = ?
[OH⁻] = ?
pH = 1.6
Process
Use the pH formula to calculate the [H₃O⁺], then calculate the pOH and with this value, calculate the [OH⁻].
pH formula
pH = -log[H₃O⁺]
-Substitution
1.6 = -log[H₃O⁺]
-Simplification
[H₃O⁺] = antilog (-1,6)
-Result
[H₃O⁺] = 0.025
-Calculate the pOH
pOH = 14 - pH
-Substitution
pOH = 14 - 1.6
-Result
pOH = 12.4
-Calculate the [OH⁻]
12.4 = -log[OH⁻]
-Simplification
[OH⁻] = antilog(-12.4)
-Result
[OH⁻] = 3.98 x 10⁻¹³
Answer:
Option D 2220mmHg
Because there are three samples each with pressure as 740mmHg so in order to find the total pressure we multiply it by 3
Explanation:
I hope this will help you :)
it was earnest rutherford he did the gold foil experiment where he shot alpha particles at gold foil that was supposed to be about 1 atom thick. He expected all the atoms to pass straight through but some bounced back, so he proposed that there was something small dense and positive in atoms aka the nucleus
Use the Nernst equation which is:
E = E° - (RT/nF)*Ln Q
Where:
E the cell voltage in V,
R the gas constant 8.314 J/K•mol,
T the room temperature normally taken 298.15K, n=3 in this case,
F the Faraday constant 96485C,
Ln is the operation of natural logarithm, and: Q = [Cl-]^3*[Al3+]
Plugging in our values, will give us:
E = 1.88-(8.314*298.15/(3*96485))*Ln(0.010^3...)
= 2.01 (V)
