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27 Nov 2019

A student back-titrates an antacid tablet. S/he adds 25.00 mL of 1.0530 M HCl to the tablet. Titrating the resulting solution to the endpoint requires 22.0 mL of 0.5040 M NaOH. How many moles of HCl were neutralized by the tablet

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Nestor Rutherford
Nestor RutherfordLv2
26 Apr 2019

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Related questions

Suppose a student adds 25.00 mL of 1.041 M HCl to a 1.50 g antacid tablet. The student boils and then titrates the resulting solution to the endpoint with 0.4989 M NaOH. The titration requires 21.1 mL NaOH to reach the endpoint. How many moles of HCl were neutralized by the NaOH?How many moles of HCl were neutralized by the tablet?

Please Help! A particular brand of antacid contains 500 mg CaCO3 per 2.0 g tablet according to label. 1. How many moles of CaCo3 are in one tablet? 2. The reaction by which the antacid neutralizes HCl is: 2HCl + CaCO3 > CaCl2 + CO2 + H20. How many moles of HCl can be neutralized by one tablet? 3. 50.0 ml of .300 M HCL are used to dissolve a 2.00 g tablet. How many moles of acid are used to dissolve the tablet? 4.The excess acid then requires 53.13 ml of .100 M NaOH for the back titration. How many moles of excess acid were there in the 50 ml? 5. How many moles of HCl were neutralized by the tablet?

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)?

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