q1.
The label on an antacid remedy states that each tablet contains 750 mg of aluminum hydroxide. Calculate the volume of stomach acid, 0.10 mol/L HCl(aq), which can be nuetralized by one antacid tablet.
Q2.
Compare equivalence point to endpoint
q1.
The label on an antacid remedy states that each tablet contains 750 mg of aluminum hydroxide. Calculate the volume of stomach acid, 0.10 mol/L HCl(aq), which can be nuetralized by one antacid tablet.
Al(OH)3 + 3HCl ==> AlCl3 + 3H2O
The remainder of the problem is worked just like the NaOH/H2SO4 problem. Don't forget to change 750 mg to grams. I assume you know mols Al(OH)3 = g/molar mass.
Q2.
Compare equivalence point to endpoint
The equivalence point is the pH (for an acid/base titration) at which what we are titrating equals exactly the material being titrated (best stated in terms of number of equivalents but that and normality are not being taught at many schools, much to my sorrow). The end point is the pH at which an indicator TELLS us we have reached that point where the number of equivalents of acid is the same as the number of equivalents of base. That is why it is called the end point. The indicator may or may not be a good one to use and this can lead to huge errors unless we pick the right indicator. That is, we would like for the end point and the equivalence point to the be same but they rarely are. With a judicious choice of indications, however, we can make them so close in most cases that the titration error is very small. There are equivalence points and end points in other titrations as well but the same principle holds as what I have said about the pH; the difference being that we aren't titrating acid/base systems.
I hope this helps.
q1. To calculate the volume of stomach acid that can be neutralized by one antacid tablet, you need to first determine the number of moles of aluminum hydroxide (Al(OH)3) in the tablet and then use the balanced chemical equation to determine the amount of hydrochloric acid (HCl) that can be neutralized.
1. Convert the mass of aluminum hydroxide from milligrams (mg) to grams (g). Since 1 g = 1000 mg, the mass of aluminum hydroxide in grams is 750 mg ÷ 1000 = 0.75 g.
2. Calculate the number of moles of aluminum hydroxide (Al(OH)3). To do this, divide the mass in grams by the molar mass of aluminum hydroxide. The molar mass of Al(OH)3 is calculated by summing the atomic masses of aluminum (Al), hydrogen (H), and oxygen (O) in one molecule of aluminum hydroxide. The atomic masses can be found on the periodic table.
Molar mass of Al: 26.98 g/mol
Molar mass of H: 1.01 g/mol
Molar mass of O: 16.00 g/mol
Molar mass of Al(OH)3 = (26.98 g/mol) + 3 × (1.01 g/mol) + 3 × (16.00 g/mol) = 78.00 g/mol
Number of moles of Al(OH)3 = Mass of Al(OH)3 / Molar mass of Al(OH)3 = 0.75 g / 78.00 g/mol
3. Use the balanced chemical equation for the reaction between aluminum hydroxide and hydrochloric acid to determine the stoichiometry. From the equation Al(OH)3 + 3HCl → AlCl3 + 3H2O, we can see that 1 mole of Al(OH)3 reacts with 3 moles of HCl.
Therefore, the number of moles of HCl that can be neutralized by 1 antacid tablet is 3 times the number of moles of Al(OH)3.
4. Finally, calculate the volume of stomach acid (HCl) that can be neutralized using the molarity of the HCl solution. The given concentration of HCl is 0.10 mol/L, which means that there are 0.10 moles of HCl in 1 liter of solution.
Volume of HCl = (Number of moles of HCl) / (Molarity of HCl)
Substitute the number of moles of HCl from step 3 and the molarity of HCl into the equation to calculate the volume in liters.
I hope this explanation helps! Let me know if you have any more questions.