Problem- A buffer solution contains .20 moles of methanoic acid, HCOOH, and .30 moles of sodium methanoate, NaCOOH in 1.00 L of the buffer. The acid ionization constant, Ka of methanoic acid is 1.8 x 10^-4
1) Calculate the pH of the solution
2) Compare the capacity of this buffer to neutralize added acid to its capacity to neutralized added base. Explain your answer completely.
3) If .10 moles of HCL gas solution were bubbled through a liter of the buffer, what would happen to the pH? How would this addition affect the buffer's capacity to neutralized added acid and base in the fute? Answer the question fully, including equations and calculation where necessary.
Solve the above problem in detail no word count