delco714 Posted October 26, 2008 Share Posted October 26, 2008 (edited) Lemon juice has a pH of about 2.5. Assuming that the acidity of lemon juice is due solely to citric acid, that citric acid is a monoprotic acid, and that the density of lemon juice is 1.0 g/mL, then the citric acid concentration calculates to 0.5% by mass. Estimate the volume of 0.0100 M NaOH required to neutralize a 3.71-g sample of lemon juice. The molar mass of citric acid is 190.12 g/mol. ANSWER IN ml of 0.0100 M NaOH. i did: 3.71g X 0.005 = 0.0186 g citric acid 0.0186g / (190.12g/mole) = 0.0000977 mole 0.0000977 mole X 39.997 g/mole NaOH = 0.00391g NaOH V = 0.00391 / 0.0100 M = .39008 L NaOH = 390.08 mL NaOH says it's wrong.. Edited October 26, 2008 by delco714 Link to comment Share on other sites More sharing options...
John Cuthber Posted October 26, 2008 Share Posted October 26, 2008 I think you have multiplied by the molar mass of NaOH twice. .0000977 moles of acid takes the same number of moles of NaOH and you can calculate the volume of that without needing the molar mass of NaOH. 0.0000997mol/0.0100 mol/litre =x mol Link to comment Share on other sites More sharing options...
delco714 Posted October 26, 2008 Author Share Posted October 26, 2008 but... MOLE / (MOLE/L) = x Liters...which is 0.00997 L.. which does = 9.97 mL... did you mean Liters and mistakenly put mole? Link to comment Share on other sites More sharing options...
John Cuthber Posted October 26, 2008 Share Posted October 26, 2008 Oops! that last unit should be litres. 10 ml is a perfectly reasonable answer for a titration. Link to comment Share on other sites More sharing options...
Recommended Posts
Create an account or sign in to comment
You need to be a member in order to leave a comment
Create an account
Sign up for a new account in our community. It's easy!
Register a new accountSign in
Already have an account? Sign in here.
Sign In Now