A SOLUTION OF 0.05METER ACID PKA 6.10 IS MIXED WITH AN EQUAL VALUE 0.1 SODIUM SOLUTION OF SODIUM SALT WHAT IS THE PH OF THE FINAL MIXTURE.
1.3
Surely you don't mean "meter" acid. Surely you mean molar.
Use the Henderson-Hasselbalch equation.
pH = pKa + log (base/acid).
To calculate the pH of the final mixture, we need to understand the reaction that takes place when the acid and its sodium salt are mixed.
In this case, the acid is dissociating in water, while the sodium salt is the conjugate base of the acid. The acid's pKa value of 6.10 indicates its degree of ionization in water. A lower pKa value means a stronger acid, and a higher pKa value means a weaker acid.
When the acid and its conjugate base are mixed, they react through a process known as a buffer solution. A buffer solution helps maintain a relatively stable pH even when small amounts of acid or base are added.
To find the pH of the final mixture, we'll use the Henderson-Hasselbalch equation:
pH = pKa + log([A-]/[HA])
In this equation, [A-] represents the concentration of the conjugate base (sodium salt), and [HA] represents the concentration of the acid.
Given that the acid solution is 0.05 M and the sodium solution is 0.1 M (which is equal to the [A-]), we can substitute these values into the equation:
pH = 6.10 + log(0.1/0.05)
Calculating this using logarithms:
pH = 6.10 + log(2)
Finally, solving for the pH:
pH ≈ 6.10 + 0.301
pH ≈ 6.40
Therefore, the pH of the final mixture is approximately 6.40.