A 10.0-mL sample of pineapple juice was titrated with 0.100 M sodium hydroxide solution. the average volume of NaOH required to reach the endpoint was 12.8 mL
a.Calculate the number of moles of sodium hydroxide required to reach the endpoint
b.Using the mole ratio for the neutralization reaction shown in equation 1, determine the number of moles of citric acid in 10.0 mL of the of pineapple juice.
Volume of citric acid= 10.0mL
Concentration of NAOH= 0.1M
Volume of NaOH= 12.8mL
Moles of NaOH at end point= ?
Moles of citric acid/10.0mL= ?
C6H8O7 + 3NaOH è Na3C6H5O7
MOLES OF NaOH:
1000.0mL of NaOH contains 0.1 mol Of NaOH
12.8mL of NaOH contains (0.1*12.8)/1000
=1.28*10-3 mol of NaOH
MOLES OF CITRIC ACID:
3NaOH = 1 C6H8O7
1.28*10-3 = (1*1.28*10-3)/3
= 4.2666*10-4 mol of C6H8O7/10.0mL
Moles of NaOH at end point= 1.28*10-3 mol of NaOH
Moles of citric acid/10.0mL=4.2666*10-4 mol of C6H8O7
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