Boston College CHEM CH111 Experiment 7 post Lab

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Boston College CHEM CH111 Experiment 7 post Lab 1. Calculate the average molarity of the NaOH solution from your three standardization trials. Trial 1: (final reading of buret: 18.86mL... ) - (Initial reading of buret : 0.56mL) = 18.30mL Litersof NaOH= 18.30mL(1L/10^3mL)= 0.0183L moles of KHPh=(0.374g)(1mol)/204.23 g= 0.001831mol KHPh M=0.001831moles of KHPh/0.0183 L= 0.100069M (1.0 x 10^(-1) M) Trial 2: (final reading of buret: 18.95mL) - (Initial reading of buret : 0.50mL) = 18.45mL Litersof NaOH= 18.45mL(1L/10^3mL)= 0.0185L moles of KHPh=(0.373g)(1mol)/204.23 g= 0.001826mol KHPh M=0.001826moles of KHPh/0.0185 L= 0.09872M (9.9 x 10^(-2) M) Trial 3: (final reading of buret: 19.70mL ) - (Initial reading of buret : 0.50mL) = 19.20mL Liters of NaOH= 19.20mL(1L/10^3mL)= 0.0192L moles of KHPh=(0.385g)(1mol)/204.23 g= 0.001885mol KHPh M=0.001885moles of KHPh/0.0192L= 0.09818M (9.8x10^(-2) M) 0.100069M+ 0.09872M+ 0.09818M/3= 0.0989896M Average of the three trials: 0.0989896M (9.9x10^(-2) M) 2. Calculations to determine the effectiveness of the antacid • Calculate the average number of moles of HCl neutralized per antacid tablet. • Calculate the number of moles of HCl neutralized per gram of antacid (weight effectiveness). • Calculate the average cost of the antacid tablet that would be needed to neutralize 1.00 mole of HCl. [Show More]

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