What is the pH of an aqueous solution that has 0.3 M potassium formate and 0.8 M formic acid? The pKa of formic acid is 3.8. Enter your answer to the nearest hundredth. Assume the temperature is 25 °C. Also, the value of R, the gas constant, is 1.987 cal/KLaTeX: \cdot⋅mol.

The pH of this aqueous solution is 3.37

Explanation:

Step 1: Data given

Concentration of potassium formate (HCOOK) = 0.3 M

Concentration of formic acid (HCOOH) = 0.8 M

pKa of formic acid = 3.8

Step 2: Calculate pH

pH = pKa = log ([conjugate base]/[acid])

pH = 3.8 + log (0.3 M / 0.8 M)

pH = 3.8 + log (0.375)

pH = 3.37

The pH of this aqueous solution is 3.37

thats how its supposed to be

answer: atomic mass was originally used to arrange elements on the periodic table, but is no longer used to organize the modern version.

explanation:

originally atomic mass was used to arrange elements on the periodic table from left to right in a row. each column then shows similar properties of elements of a group.

in modern periodic table, the atoms are arranged in increasing atomic number. as atomic number represents the number of protons in an atom which is unique for every atom.