Rutgers University Titration of an Antacid Lab Report Watch my introductory video by Clicking Here. Click and watch each of the following videos. 1. Expe | Course Hero

Rutgers University Titration of an Antacid Lab Report Watch my introductory video by Clicking Here.

Click and watch each of the following videos.

1. Experimental Video: Click Here

Document attached below.

Using the data provided, perform the calculations need to fill in the missing values on the report sheet. Do not use the data given in the videos.
Submit the lab as an attachment to this assignment (Word document only).

Professor’s Instructions^ CH 111 – Introduction to Inorganic and Organic Chemistry
Lab 7 – Exp. 478 – Titration of an Antacid
In this lab we are going to determine the amount of HCl one antacid tablet can
neutralize. We are going to utilize a titration to perform this analysis, however we cannot do
the standard titrations we have done the previous 2 labs. Instead we will be performing
something called a back titration.
A back titration involves adding an excess of one of the reactants in the neutralization
reaction, and then titrating back the excess amount added. This is necessary because the
antacid tablet is insoluble in water, so in order to get the ions in solution we must first react the
antacid (Calcium Carbonate (CaCO3)) with excess HCl, according to reaction 1 below. Some of
the HCl will be neutralized by the CaCO3, but the excess will remain in the flask. The excess HCl
will then be titrated with NaOH, just as we did in Exp. 5 according to reaction 2 below. Since we
will know the exact amount of HCl added, we can determine the amount of HCl that that was
not neutralized by the antacid. We can then determine the amount of HCl that was neutralized
by the antacid.
1.
2 HCl (aq) + CaCO3 (s)
CaCl2 (aq) + H2O (aq) + CO2 (g)
Antacid
2.
HCl (aq) + NaOH (aq)
NaCl (aq) + H2O (aq)
Excess HCl
Supplementary Questions
1. What was the mass of the tablet in the video?
2. What was the concentration of the NaOH in the video? (Normal is the same as Molar in
this example.)
3. How many mL of distilled water did he add?
4. How many drops of phenolphthalein were added?
5. Why does HCl need to be added to the tablet in the beginning of the experiment?
Data Sheet
Mass of Antacid Tablet (g)
Trial 1
Trial 2
0.6274
0.6111
Molarity HCl (M)
0.600
Volume HCl Added to Tablet (mL)
25.0
Molarity NaOH (M)
1.00
Volume NaOH initial (mL)
1.2
0.4
Volume NaOH final (mL)
10.8
10.6
Volume NaOH Used in Titration (mL)
Moles HCl Added to Tablet (mol)
Moles NaOH req. (mol)
# moles HCl neutralized per tablet (mol)
Avg. # moles HCl neut. per tablet (mol)
# moles HCl neutralized per gram of tablet (mol)
Avg. # moles HCl neut. per gram of tablet (mol)
Calculations
Volume NaOH used in titration = Volume NaOH final – Volume NaOH initial
Moles HCl = volume HCl used in Liters (convert!) x Molarity HCl
Moles NaOH req. = volume NaOH used in Liters (convert!) x Molarity NaOH
# moles HCl neutralized per tablet = moles HCl added – moles NaOH req.
# moles HCl neutralized per gram of tablet =
??????.# ?????????? ?????? ????????.?????? ????????????
???????? ???? ????????????

Purchase answer to see full
attachment