Calculate the ph of a solution that is 0.065 m in potassium propionate (c2h5cook or kc3h5o2) and 0.090 m in propionic acid (c2h5cooh or hc3h5o2).

The pH of the solution with 0.065 m in potassium and 0.090 m in propionic acid is : 4.75

Given data :

Potassium propionate [ A⁻ ] : 0.065 m

Propionic acid [ HA ] : 0.090 m

Ka = 1.3 * 10⁻⁵

To determine the pH of the solution we will apply the H-H equation

pH = Pka + log [ A / HA ] ( 1 )

where : pKa = -log Ka = 4.89

Insert value into equation ( 1 )

pH = 4.89 + log [ 0.065 / 0.090 ]

     = 4.75

Therefore the pH of the solution is 4.75

Learn more about pH of solution : link

number of molecules / avogadro's number * molecule molecular = mass

explanation:

we define a gram-molecular weight as the mass of one mole of any element or compound. a mole contains avogadro's number of units (molecules) –  

6.022

x

10

23

. so, dividing the number of molecules by avogadro's number gives us the number of moles. multiplying that by the molecular weight gives us the mass. from the periodic table we find the gram-molecular weight of u to be238 and of f to be19. so,  

u

f

6

will have a gram-molecular weight of 352g.

c, liquids evaporate, creating a gas