An antacid tablet weighing 1.462 grams was dissolbed in 25mL of 0.8M HCl and diluted with water. The excess HCl was titrated with 3.5 mL of 1.019M NaOH solution.
1. Calculate the number of millimoles added to the tablet
2. Calculate the number of millimoles of NaOH required to neutralize the excess HCl left over
3. Calculate the number of millimoles of HCl that neutralized the tablet.
1. Calculate the number of millimoles added to the tablet
I assume this means mmoles of HCl added to the tablet.
mmoles = M acid x mL acid.
2. Calculate the number of millimoles of NaOH required to neutralize the excess HCl left over
mmoles NaOH = M NaOH x mL NaOH
3. Calculate the number of millimoles of HCl that neutralized the tablet.
mmoles tablet = mmoles HCl initially - mmoles HCl excess.
Post your work if you gets stuck.
16.4335
To solve these questions step-by-step, we'll use the given information and follow these calculations:
1. Calculate the number of millimoles added to the tablet:
- The molar mass of the antacid tablet is required to convert its mass to millimoles. However, the molar mass is not given, so this question cannot be answered with the given information.
2. Calculate the number of millimoles of NaOH required to neutralize the excess HCl left over:
- First, we need to find the number of millimoles of HCl in the excess solution.
- To do that, we'll use the concentration of HCl and the volume of HCl solution.
- Moles of HCl = concentration (in M) x volume (in L)
- Moles of HCl = 0.8 M x 0.025 L (as the volume was given in mL)
- Moles of HCl = 0.02 mol
- Since the balanced equation for the reaction between HCl and NaOH is 1:1, the number of millimoles of NaOH required is also 0.02 mmol.
3. Calculate the number of millimoles of HCl that neutralized the tablet:
- We can use the balanced equation between antacid and HCl to determine the number of millimoles of HCl required to neutralize the tablet.
- However, since the molar mass of the antacid tablet is not provided, we cannot calculate the number of millimoles of HCl neutralized by the tablet.
To solve these calculations, we need to follow a step-by-step approach. Let's break down each question and work through them one by one:
1. To calculate the number of millimoles added to the tablet, we first need to determine the number of moles of HCl solution used. We know that the concentration of the HCl solution is 0.8M and the volume used is 25 mL.
To convert the volume to liters, we divide by 1000: 25 mL / 1000 = 0.025 L.
Now, we can calculate the number of moles of HCl used by multiplying the concentration by the volume: 0.8 M * 0.025 L = 0.02 moles of HCl.
2. To calculate the number of millimoles of NaOH required to neutralize the excess HCl left over, we first need to determine the number of moles of NaOH used. We know the concentration of the NaOH solution is 1.019 M and the volume used is 3.5 mL.
Again, we convert the volume to liters: 3.5 mL / 1000 = 0.0035 L.
Now, we can calculate the number of moles of NaOH used by multiplying the concentration by the volume: 1.019 M * 0.0035 L = 0.0035625 moles of NaOH.
3. Finally, to calculate the number of millimoles of HCl that neutralized the tablet, we need to determine the difference between the moles of HCl used and the moles of NaOH used.
The moles of HCl used to neutralize the tablet is given by: 0.02 moles - 0.0035625 moles = 0.0164375 moles of HCl.
To convert this to millimoles, we multiply by 1000: 0.0164375 moles * 1000 = 16.4375 millimoles of HCl.
Therefore, the answers to the three questions are:
1. The number of millimoles added to the tablet is 20 millimoles.
2. The number of millimoles of NaOH required to neutralize the excess HCl left over is 3.5625 millimoles.
3. The number of millimoles of HCl that neutralized the tablet is 16.4375 millimoles.