1How would each of the following affect the accuracy of the calculated neutralizing power of antaid (too high, too low, no effect) explain
a)The actacid tablet was not cut exactly in half before weighing
b)The solution mixture of reacted antacid and excess HCL spattered out of the flask during boiling
2 Calculate the neutralizing powe of 1 gram of pure NaHCO3 (FW=84.02g/mol)
Answers depend on what you were doing.
1a) If the actacid tablet was not cut exactly in half before weighing, it would likely affect the accuracy of the calculated neutralizing power of antacid. The neutralizing power of an antacid is determined by the amount of active ingredient present in the tablet. By not cutting the tablet exactly in half, the amount of active ingredient in the measured portion may not be representative of the entire tablet. This could lead to an overestimation or underestimation of the neutralizing power, depending on whether the tablet was cut above or below the actual center.
b) If the solution mixture of reacted antacid and excess HCl spattered out of the flask during boiling, it would also likely affect the accuracy of the calculated neutralizing power. This is because some of the mixture would be lost, which means that less of the antacid would be available to neutralize the acid. Consequently, the measured neutralizing power would be lower than expected.
2 To calculate the neutralizing power of 1 gram of pure NaHCO3, we need to determine the number of moles of NaHCO3 first.
The formula weight (FW) of NaHCO3 is given as 84.02 g/mol. Since we have 1 gram of NaHCO3, we can convert this to moles by dividing the mass by the FW:
moles = mass / FW
moles = 1 g / 84.02 g/mol
Simplifying the equation gives us:
moles ≈ 0.011904 mol
The neutralizing power of an antacid is often defined as the number of moles of HCl that can be neutralized by 1 mole of the antacid. In this case, NaHCO3 can neutralize 1 mole of HCl.
Therefore, the neutralizing power of 1 gram of pure NaHCO3 would be approximately 0.011904 mol.