Post by: kat148 on August 21, 2009, 06:02:13 am
Q) Gastric juice consists essentially of a solution of hydrochloric acid and the enzyme pepsin. It is normally at a pH in the range of 0.3 to 1.2 with the lower figure leading to hyperacidity. The commonly available antacids provide relief from hyperacidity. Aluminium hydroxide is sometimes used for this purpose.
What mass of aluminium hydroxide must be used in an antacid tablet if it is designed to increase the pH of 500 ml of gastric juice from 0.3 to 0.12?
..now would the first step be to calculate the
Thanks in advance!
Post by: chem-nerd on August 21, 2009, 03:28:06 pm
n(H3O+) to be neutralised = (10-0.3 - 10-1.2)/2 = 0.219 mol
n(Al(OH)3) = 1/3 x 0.219 mol
the use m = n x Mr
Post by: kat148 on August 21, 2009, 05:16:48 pm
Post by: kat148 on August 25, 2009, 09:20:19 pm
A commonly used primary standard acid in analytical chemistry is potassium hydrogen phthalate (
In a titration exercise it is found that a sample of 1.305g of potassium hydrogen pthalate requires 17.28 ml of sodium hydroxide solution to neutralise it.
What is the molarity of the NaOH solution.
Can anybody lead me in the right direction? Thanks
Post by: Edmund on August 25, 2009, 09:37:37 pm
n(potassium hydrogen phthalate) = n(NaOH)
Now we have n(NaOH), V(NaOH), we can calculate C.
Post by: kat148 on August 25, 2009, 10:25:36 pm
Post by: kat148 on September 01, 2009, 12:07:37 am
What volume of 0.100M
Again, how would I apporach this?
Thanks for any advice