A 50.0mL volume of 0.15 M HBr is titrated with 0.25 M KOH. Calculate the pH after the addition of 12.0 mL of KOH.

A buffer is made using 100.0 mL of 0.100 M CH3 CH2 COOH (propanoic acid) and 100.0 mL of 0.100 M NACH3 CH2 COO (sodium propanoate). A) Explain in your own words what will occur (at the molecular level) when an nitric acid is added to the buffer? What would be the effect on the pH? B) Explain in your own words what will occur when LIOH is added tot he buffer? What would be the effect on the [H+]?

Determine the pH at the equivalence point of a titration between 50.0 mL of 0.157 M (CH3)2NH solution with 0.157 M HCIO4. Remember that only the decimals in a pH count as significant figures. Please enter your answer with three decimal places.

A 25.0 mL sample of 0.86 M HCOOH is titrated with 0.20 M KOH. What is that pH of the solution at equivalence point ? Ka= 1.77 x 10^-14