4. A student analyzed an antacid tablet from a bottle of 48 tablets purchased at

Question

4. A student analyzed an antacid tablet from a bottle of 48 tablets purchased at a discount store for $1.00. The mass of the tablet was 1.462 g. After adding 25.00 mL of 0.8000M HCI solution to the tablet, the student back-titrated the excess HCl with 3.52 mL of 1.019M NaOH solution. (a) Calculate the number of moles of HCI added to the tablet. (b) Calculate the number of moles of NaOH required for the back-titration. (c) Calculate the number of moles of HCl neutralized by the antacid tablet. (d) Calculate the mass effectiveness of the tablet. (e) Calculate the cost of one antacid tablet. (0 Calculate the cost effectiveness of the tablet.

Explanation / Answer

Q4

a)

moles of HCl = MV = (0.8*25*10^-3) = 0.02

b)

mol of NaOH = MbaseVbase = 1.019 * 3.52*10^-3 = 0.00358688

c)

mol of HCl used in antacid =0.02 -  0.00358688 = 0.01641

d)

effectiveness --> 0.01641 mol of HCl --> mol*MW = 0.01641*36.5 = 0.598965 g of Hcl can be neutralized

e)

cos ot 1 antacid --> 1 USD per 48 tablets -_> 1.00/48 = 0.0208 $ = 0.02 usd or 2 cents

f)

Cost effective tablet --> 2 cents / 0.598965 g = 3.33 cents per gram

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