Answer:
56.9 mmoles of acetate are required in this buffer
Explanation:
To solve this, we can think in the Henderson Hasselbach equation:
pH = pKa + log ([CH₃COO⁻] / [CH₃COOH])
To make the buffer we know:
CH₃COOH + H₂O ⇄ CH₃COO⁻ + H₃O⁺ Ka
We know that Ka from acetic acid is: 1.8×10⁻⁵
pKa = - log Ka
pKa = 4.74
We replace data:
5.5 = 4.74 + log ([acetate] / 10 mmol)
5.5 - 4.74 = log ([acetate] / 10 mmol)
0.755 = log ([acetate] / 10 mmol)
10⁰'⁷⁵⁵ = ([acetate] / 10 mmol)
5.69 = ([acetate] / 10 mmol)
5.69 . 10 = [acetate] → 56.9 mmoles
Answer:
0.1440M
Explanation:
Let''s bring out the parameters we were given;
Rate constant = 8.74 x 10^-4s^-1
Initial Concentration [A]o = 0.330M
Final concentration [A]= ?
Time = 800s
The reaction is a first order reaction, due to the unit of the rate constant. In first order reactions, the reaction rate is directly proportional to the reactant concentration and the units of first order rate constants are 1/sec.
Formular relating these parameters is given as;
ln[A] = ln[A]o − kt
Making [A] subject of interest, we have;
ln[A] = ln[A]o − kt
ln[A] = ln(0.330) - ( 8.74 x 10^-4 * 800)
In[A] = - 1.1086 - (6992 x 10^-4)
ln[A] = -1.8079
[A] = 0.1440M
Chlorine: The greenish-yellow, highly reactive and diatomic gas that is almost never found free in nature by itself. Most Chlorine is commercially produced and is most widely known for being used within compounds to purify water and create cleaning products.
Chloride: The negatively charged ionic form of Chlorine. Since Chlorine is found deep within the Earth's crust, and is extremely reactive, the only way it can be found in nature is when it reacts with other chemicals and creates compounds. Chloride is what is created when Chlorine gains an electron and combines with other elements. Chloride is found abundantly in nature and is most commonly known for forming neutral salts such as sodium chloride (table salt), potassium chloride, and calcium chloride.
By providing an alternative reaction<span>mechanism with a lower activation energy.</span>
