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

Chemistry
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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

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