Say, for example, that you had prepared a buffer c, in which you mixed 8.203 g of sodium acetate, nac2h3o2, with 100.0 ml of 1.0 m acetic acid. what would be the initial ph of buffer c? if you add 5.0 ml of 0.5 m naoh solution to 20.0 ml each of buffer b and buffer c, which buffer's ph would change less? explain

pH regulatory solution 4.8

pH regulatory solution when adding base 4.86    

Explanation:

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To calculate the pH of a regulatory solution, the acid constant that relates the acid and the base must be identified in the table. In this case the constant that relates acetic acid and acetate anion has a value Ka = 1.75*10-5.

Assuming that the volume does not vary by aggravating sodium acetate we can calculate its concentration.

Knowing the acid constant and the acid and base concentrations, the pH of the solution is calculated.

By adding a base to the solution, the concentration of the acid species (acetic acid) is decreased by calculating the new concentration, the pH is calculated.

To calculate the concentration after adding the base it is necessary to calculate the dilution of each species, to avoid calculations it is convenient to work with mol or millimol (because they are contained in the same volume can be simplified).

The addition of an acid reduces the formation of the basic species of the solution.

The description of buffer b is missing to compare which pH varies more.

In a larger volume of regulatory solution, lower changes in pH are expected from the addition of acids or bases than in a small volume of solution.

In solutions with equal amounts of acid and base, lower changes in pH are expected than in solutions with different amounts due to the addition of acids or bases.

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adding or remove a gaseous reactant or product changes the concentrations. if the concentration of reactant or product is increased, the system will shift away from the side in which concentration was increased (i.e. if the concentration of reactants is increased, the system will shift toward the products. if more products are added, the system will shift to form more reactants). conversely, if the concentration of reactant or product is decreased, the system will shift toward the side in which concentration was decreased (i.e. if reactants are removed, the system will shift to form more reactants. if the concentration of products is decreased, the equilibrium will shift toward the products).

explanation: