I've been stuck on this problem for 4 hours and i don't know what to do.
H3PO4+3NaOH----> Na3PO4+3H2O
if 30.00ml of 0.1000N NaOH was required to neutralize 15.00ml of an H3PO4 solution, what is the normality of the acid? How many grams of H3PO4 are in the 15ml solution?
thank you for your help
H3PO4+3NaOH----> Na3PO4+3H2O
if 30.00ml of 0.1000N NaOH was required to neutralize 15.00ml of an H3PO4 solution, what is the normality of the acid? How many grams of H3PO4 are in the 15ml solution?
thank you for your help
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WEll its not tht difficult .......
milliequivalents of NaOH = Milli equivalents of H3PO4
Normality of NaOH x Volume of NaoH = N X volume of H3PO4
.1 X 30 = 15N
=> N = .2
Molarity = N / basicity = .2 /3 = 0.067
Also , Molarity = number of moles / Volume
0.067 = n / .15
n = .15 X 0.067 = .01
w / M = .01 M = molar mass = 98 gm/mole
=> w = 0.01 X 98 = 0.98 gms
hope tht helps !! Gud luck !!!:D
milliequivalents of NaOH = Milli equivalents of H3PO4
Normality of NaOH x Volume of NaoH = N X volume of H3PO4
.1 X 30 = 15N
=> N = .2
Molarity = N / basicity = .2 /3 = 0.067
Also , Molarity = number of moles / Volume
0.067 = n / .15
n = .15 X 0.067 = .01
w / M = .01 M = molar mass = 98 gm/mole
=> w = 0.01 X 98 = 0.98 gms
hope tht helps !! Gud luck !!!:D