SOLVED: Suppose a student adds 25.00 mL of 0.989 M HCl to a 1.53 g antacid tablet. The student uses 20.9 mL of 0.555 M NaOH to titrate the solution. Calculate the moles of acid neutralized per gram of tablet.Suppose a student uses 1.024 M HCl to do a titration. However, they accidentally record the molarity as 1.004 M HCl. Will the moles of acid neutralized by the tablet appear too high, too low, or unchanged? Explain.More acid was added than thought, so the titration requires more NaOH than exp

SOLVED: Experiment Antacid AnalysisWeight of Antacid Tablet: Initial /3 = '304E J2i8g 3081g 0-1 MAg Concentration of HCLM: 0.1522 M Volume HCI ml added: [WUml of HCI was added to dissolve the tablet and diluted = to 250 ml Concentration of NaOH; M: 1607 M Volume NAOH required, ml: 4.4 47- 13.4ml /3-4A67ml For titration used only 25ml dissolved aliquots of trial Weight of Required NaOHml tablet, 3044 3218 1.30b|Using the results provided, do the following questions in your notebook: Using the tit

Antacid side effects

#longtermantacid #Antacid #antacidsideeffects #integrativemedicine #functionalmedicinedoctor #SideEffects #reminder | Robert Navalta

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