For a theoretical yield of 1.98 g and percent yield of 92.1687%, calculate the actual yield for a chemical equation.
Answer in grams.

Actual yield  = 1.825 g

Explanation:

Given data:

Theoretical yield = 1.98 g

Percent yield = 92.1687%

Actual yield = ?

Solution:

Formula:

Percent yield = actual yield / theoretical yield × 100

Now we will put the values in formula:

92.1687 = actual yield /  1.98 g × 100

92.1687 / 100 = actual yield /  1.98 g

0.921687 =  actual yield /  1.98 g

0.921687 ×  1.98 g  = actual yield

Actual yield  = 1.825 g

when [oh-] is 10-5  m, and [h3o+] is 10-9  m, the poh is 5 and ph is 9. again in both cases the sum of ph and poh is 14. however, the hydrogen ion concentration is not always going to be equal to exactly 1 x 10 raised to a negative number. for example, we skipped over the value of 2.0 x 10-7.