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13 Dec 2019
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?
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?
Nelly StrackeLv2
17 Dec 2019
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