Question #209442
When a solution prepared by dissolving 4.00 g of an unknown monoprotic acid in 1.00 L of water is titrated with 0.600 M , 37.0 mL of the solution is needed to neutralize the acid.
a
Determine the molarity of the acid solution.
Expert's answer
1. Find the number of moles of 37ml (0.6M) solution used to neutralize the acid. To do this, use the following formula: n=V(l)*CM
n=V*CM=0.037L *0.6M=0.0222mol
2. 1 mole of alkali is used to neutralize 1 mole of monoprotic acid. that is, the monoprotic acid was also 0.0222mol
3. We use the following formula to find the molarity of an acid: CM=n/V
CM=0.0222mol/1L= 0.0222mol/L
Answer: 0.0222mol/L
