An unknown weak acid with a concentration of 0.086 M has a pH of 1.80. What is the Ka of the weak acid?

2.90 × 10⁻³

Explanation:

Step 1: Given data

pH: 1.80

Concentration of the weak acid (Ca): 0.086 M

Step 2: Calculate the concentration of H⁺

We will use the following expression.

pH = -log [H⁺]

[H⁺] = antilog -pH = antilog -1.80

[H⁺] = 0.0158 M

Step 3: Calculate the acid dissociation constant (Ka)

We will use the following expression.

Ka = [H⁺]² / Ca

Ka = 0.0158² / 0.086

Ka = 2.90 × 10⁻³

the formula mass of a molecule or a compound is the sum of the atomic weights of the atoms in its empirical formula

(that's what i know about formula mass)

you need to have a picture of the atom that way we can answer it