The following data was obtained by Odar Sverk when he completed this investigation:
a) 220 mL of acid (0,1 M HCl) was added to two tablets of Divol , a brand of antacid. The total mass of the two tablets was 2.50 g. 15 mL of base was used to complete the analysis. Find the A.C.C. per tablet of Divol.
b) What is the significance of the A.C.C. number?
c) Complete the following statement: Divol neutralizes __________ times its mass in excess stomach acid.
ACC: acid consuming capability
The base used to complete analysis: what strength was that?
molesHCL-molesBase*(Heq)=moles acid consumed
ACC= massacidconsumed/mass Divol tabs
What base? What strength?
What does A.C.C stand for?
To calculate the A.C.C. (Active Compound Content) per tablet of Divol, we need to determine the amount of acid neutralized by the tablet in the given experiment. Here's how you can find the answer:
a) First, we need to determine the moles of acid used in the reaction:
Moles of acid = volume of acid (in liters) x concentration of acid
Given that the volume of acid is 220 mL and the concentration is 0.1 M (Molar), we convert the volume to liters:
Volume of acid = 220 mL = 0.22 L
Now we can calculate the moles of acid used:
Moles of acid = 0.22 L x 0.1 M = 0.022 moles
Next, we need to calculate the moles of base used in the titration. Since it is not specified which base was used, we'll assume it is sodium hydroxide (NaOH) since it's commonly used in neutralization reactions:
Moles of base = volume of base (in liters) x concentration of base
Given that the volume of base used is 15 mL and the concentration of NaOH is typically around 0.1 M, we convert the volume to liters:
Volume of base = 15 mL = 0.015 L
Now we can calculate the moles of base used:
Moles of base = 0.015 L x 0.1 M = 0.0015 moles
Since the reaction between the acid and base is 1:1 according to the balanced equation, the moles of acid neutralized is equal to the moles of base used.
Therefore, the moles of acid neutralized = 0.0015 moles.
To find the A.C.C. per tablet, we divide the moles of acid neutralized by the total mass of the two tablets:
A.C.C. per tablet = moles of acid neutralized / total mass of tablets
Given that the total mass of the two tablets is 2.50 g:
A.C.C. per tablet = 0.0015 moles / 2.50 g = 0.0006 moles/g or 0.6 mmol/g
Therefore, the A.C.C. per tablet of Divol is 0.6 mmol/g.
b) The A.C.C. (Active Compound Content) number is significant because it indicates the amount of active compound present in a particular sample or dosage form. It helps in determining the effectiveness and potency of a medication or therapeutic agent. By knowing the A.C.C., healthcare professionals and researchers can ensure consistent dosing and compare different products or formulations.
c) Divol neutralizes __________ times its mass in excess stomach acid.
To complete the statement, we can use the A.C.C. per tablet obtained in part a) and the concept of stoichiometry from the balanced equation:
The balanced equation for neutralization of hydrochloric acid (HCl) with sodium hydroxide (NaOH) is:
HCl + NaOH -> NaCl + H2O
From the equation, we know that 1 mole of HCl reacts with 1 mole of NaOH to produce 1 mole of water. Additionally, we found in part a) that 0.0015 moles of HCl were neutralized.
Now, we can determine the mass of excess stomach acid neutralized:
Mass of excess stomach acid neutralized = moles of acid neutralized x molar mass of HCl
The molar mass of HCl is given as 36.46 g/mol.
Mass of excess stomach acid neutralized = 0.0015 moles x 36.46 g/mol = 0.055 g
Therefore, we can complete the statement as follows:
Divol neutralizes 0.055 g (or 55 mg) of excess stomach acid per tablet.