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12 Dec 2019

1.Suppose an antacid is dissolved in 25.00 mL of 1.00 M HCl solution. The solution is titrated with 1.00 M NaOH solution. The endpoint of the titration is reached when 14.45 mL of NaOH solution have been added. How many moles of acid were neutralized by the antacid?

2.The volume added from a buret can typically be determined to the 0.05 or even 0.01 mL.

a)True

b)False

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Beverley Smith
Beverley SmithLv2
13 Dec 2019

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Related questions


4. A 0.201 g sample of antacid is dissolved in water, and then 50.0 mL of 0.100 M HCl is added so that the solution is acidic. The excess HCl is then titrated with 0.0883 M NaOH to the equivalence point. The back titration requires 20.33 mL to reach the endpoint.

b. How many moles of HCl was added initially?

c. How much excess HCl was titrated with NaOH(in mol HCl)?

d. How many moles of HCl were neutralized by the antacid?

e. What is the effectiveness of the antacid (in mol HCl neutralized/g antacid)?

Please show all work!! Thank you!! :)

A 0.6841 gram sample of an antacid is weighed out and then 50.00 mL of 0.098 M HCL is added to the antacid.

A. Calculate the moles of acid added to the antacid.

B. The solution is titrated to its endpoint. What color is the solution at the endpoint this week?

c. To reach the endpoint, 22.83 mL of 0.1032 M NaOH are required. How many moles of base are used for the back titration?

d. How many moles of acid were neutralized by the antacid?

e. Based on this data, what is the acid consuming capacity (ACC) of the antacid (moles/g)?

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