37th question plzz
Dear Student,
As given in the question;
a.) 100 mL (cm3) of 0.1 M oxalic acid (O.A) solution
(considering the oxalic acid to be anhydrous)
I. Molecular weight of O.A = 90.02 g/mol
When oxalic acid is hydrated
II. Molecular weight of O.A = 126 g/mol
0.1 moles = 1000 mL (from molarity given)
1 mL = 0.1/1000 moles
100 mL will have = (0.1/1000) x 100 = 0.01 moles
Case I. Amount of O.A = 0.01 x 90 = 0.9 g
Case II. Amount of O.A = 0.01 x 126 = 1.26 g
b.) Molecular weight of anhydrous sodium carbonate = 106 g/mol
Volume of solution = 500 cm3 or mL
molarity = 0.12 M
Hence 0.12 moles = 1000 mL
So 500 mL = (0.12/1000) x 500 = 0.06 moles
Amount present = 0.06 x 106 = 6.36 grams
Please let me know, if you have any doubts.
Regards
As given in the question;
a.) 100 mL (cm3) of 0.1 M oxalic acid (O.A) solution
(considering the oxalic acid to be anhydrous)
I. Molecular weight of O.A = 90.02 g/mol
When oxalic acid is hydrated
II. Molecular weight of O.A = 126 g/mol
0.1 moles = 1000 mL (from molarity given)
1 mL = 0.1/1000 moles
100 mL will have = (0.1/1000) x 100 = 0.01 moles
Case I. Amount of O.A = 0.01 x 90 = 0.9 g
Case II. Amount of O.A = 0.01 x 126 = 1.26 g
b.) Molecular weight of anhydrous sodium carbonate = 106 g/mol
Volume of solution = 500 cm3 or mL
molarity = 0.12 M
Hence 0.12 moles = 1000 mL
So 500 mL = (0.12/1000) x 500 = 0.06 moles
Amount present = 0.06 x 106 = 6.36 grams
Please let me know, if you have any doubts.
Regards