Time remaining:
if an antacid tablet is olied with 50mL of 0.10M HCL, and the resulting solution requires 8.9 mL of

Chemistry
Tutor: None Selected Time limit: 1 Day

if an antacid tablet is bolied with 50mL of 0.10M HCL, and the resulting solution requires 8.9 mL of 0.095 M NaOH in a back titration, whatr mass of NaHCO3 did the tablet contain ?

Apr 7th, 2015

Step 1:

Determine the number of moles of HCl added.

50 mL * 1L/ 1000mL * 0.1 mol /  1 L = 0.005 mol HCl

Step 2:

Determine the number of moles of NaOH added.

8.9 mL *1L/1000mL * 0.095 mol / 1 L = 0.0008455 mol NaOH

Step 3:

Determine the number of moles of HCl that reacted with the antacid.

HCl + NaOH ======> NaCl + H2O

0.0008455 mol NaOH * 1mol HCl/1mol NaOH = 0.0008455 mol HCl

0.005 mol - 0.0008455 mol = 0.0041545 mol HCl reacted with antacid

Step 4:

Determine the mass of NaHCO3 in the antacid.

NaHCO3 + HCl =====> H2CO3 + NaCl

0.0041545 mol HCl * 1 mol NaHCO3 / 1 mol HCl * 84.007 g / 1 mol NaHCO3 = 0.349 g NaHCO3 in the antacid.


Apr 7th, 2015

thank you 

Apr 7th, 2015

thank you 

Apr 7th, 2015

Studypool's Notebank makes it easy to buy and sell old notes, study guides, reviews, etc.
Click to visit
The Notebank
...
Apr 7th, 2015
...
Apr 7th, 2015
Mar 25th, 2017
check_circle
Mark as Final Answer
check_circle
Unmark as Final Answer
check_circle
Final Answer

Secure Information

Content will be erased after question is completed.

check_circle
Final Answer