Determine the empirical formula for a compound that is 70.79% carbon

CH₅

Explanation:

This question may be lacking some information and in order to solve it, I will assume that the compound is a hydrocarbon, and therefore the percentages of carbon and hydrogen are:

C = 70.79 %                        H = 100 - 70.79 = 29.21 %

In 100 grams of compound wil have

70.79 g C

20.21 g H

Dividing by the atomic weights to get the mol of atoms:

C= 70.71 g/ 12 g/mol = 5.90 mol

H= 29.21 g/1 g/mol = 29.21 mol

Dividing by the 5.90 to get the proportions ,

C = 5.90/5.90 = 1

H= 29.21/5.90 = 4.95 rounding to 5,

the empirical formula is 1 atom of carbon per 5 of hydrogen

CH₅

the ratio of the conjugate base to the acid required to attain the desired ph.