In experiment 1, you study a neutralization reaction involving an acid and a base.
Oxalosuccinic acid (H3C6H3O7) is a tricarboxylic acid.
It reacts with NaHCO3 (sodium bicarbonate or "baking soda") to yield carbon dioxide, water and sodium oxalosuccinate (Na3C6H3O7).
Balance the following reaction:
H3C6H3O7(aq) + 3NaHCO3(s) = 3CO2(g) + 3H2O(l) + Na3C6H3O7(aq)
A student measures 11.41 g of baking soda and adds this to 24. mL of 3.0 M oxalosuccinic acid (in an alcoholic solution).
Identify the limiting reagent and calculate the number of moles of CO2 produced.
The limiting reagent is:
1.358×10-1 mol of CO2 are produced.
QUESTION: Hypothetically, if the temperature of the solution goes from 25.0°C to 8.0°C the reaction is considered
Calculate the temperature change per mole of H+ which reacted.
ΔT/(mol H+ reacted) = K/mol
*11.41 g NaHCO3/84.007 g/mol = 0.1358 mol NaHCO3.
3 M * 0.24 L = 0.72 mol H3C6H3O7
I determined that baking soda was the limiting reagent through some calculations and verifIcations.
For the question I am stuck on, I know that Delta T is -17 from 8-25.
I am not quite sure how to get the moles of H+.
Please any help is appreciated.