Grapefruit juice contains approximately 0.75g/oz of citric acid (H3C6H5O7(aq)), a triprotic acid. If one tablet of Tums contains 500mg of CaCO3, would one tablet be able to neutralize the acid in one glass of grapefruit juice (8.0oz)? Show your calculations.
Therefore I found the relavant variables would be:
- 0.75g/oz of citric acid
- the fact that it's a triprotic acid
- the volume of one glass of grapefruit juice (8.0oz)
- the grams of tums (0.5g CaCO3)
- Balancing the equation, which I had no idea how to do. I attempted to use the products H2O + CO2 + CaO, but I found I couldn't balance it.
- Dimensional analysis of the citric acid and CaCO3 from grams to moles
The Attempt at a Solution
1) Multiplied 0.75g/oz of Citric acid with the volume of citric acid (8.0oz) to get the grams of citric acid in grapefruit juice
2) I converted it to the moles of citric acid by dividing by the molar weight
So: 6.0g citric acid/193.1241g citric acid
3) I converted the amount of CaCO3 to moles as well
Not entirely sure where to go from here.