Make a buffer solution with the following specification pH=5.5 Volume=2L total concentration=1M ...
a) Name the components?...
b) How many grams of each component would you use to make 2L of solution
To make a buffer solution with a pH of 5.5, a volume of 2L, and a total concentration of 1M, you need to consider two components: an acid and its conjugate base. The acid will provide the hydrogen ions (H+), while the conjugate base will help neutralize any added acid or base to maintain the desired pH.
a) Naming the Components:
Let's assume that the acid component is Acetic Acid (CH3COOH) and the conjugate base component is Sodium Acetate (CH3COONa). In this case, Acetic Acid acts as the weak acid, while Sodium Acetate acts as the weak base.
b) Calculating the Amount of Each Component:
To calculate the amount of each component required to make 2L of the solution, we need to use the total concentration and the volume.
1. Determine the moles of the acid:
The moles of the acid can be calculated using the equation: Moles = Concentration x Volume
Moles of Acetic Acid = 1M x 2L = 2 moles
2. Calculate the grams of the acid:
Using the molar mass of Acetic Acid (CH3COOH), which is approximately 60.05 g/mol, we can calculate the grams needed.
Grams of Acetic Acid = Moles x Molar Mass = 2 moles x 60.05 g/mol = 120.1 grams
3. Determine the moles of the conjugate base:
Since the buffer solution has a 1:1 ratio of acid to conjugate base, the moles of the conjugate base will be the same as the moles of the acid. Therefore, the moles of Sodium Acetate is also 2 moles.
4. Calculate the grams of the conjugate base:
Using the molar mass of Sodium Acetate (CH3COONa), which is approximately 82.03 g/mol, we can calculate the grams needed.
Grams of Sodium Acetate = Moles x Molar Mass = 2 moles x 82.03 g/mol = 164.06 grams
Therefore, to make 2L of buffer solution with a pH of 5.5, you would need approximately 120.1 grams of Acetic Acid (CH3COOH) and 164.06 grams of Sodium Acetate (CH3COONa).