what is the normality of a 2.0M phosphoric acid, H3PO4, solution?

Question

a. 0.67N
b. 2.0N
c. 4.0N
d. 6.0N

Answer 1

Normality is equal to the gram equivalent weight of a solute per liter of solution. A gram equivalent weight or equivalent is a measure of the reactive capcity of a given molecule. Normality is the only concentration unit that is reaction dependent.

Example:
1 M sulfuric acid (H2SO4) is 2 N for acid-base reactions because each mole of surfuric acid provides 2 moles of H+ ions. On the other hand, 1 M sulfuric acid is 1 N for sulfate precipitation, since 1 mole of sulfuric acid provides 1 mole of sulfate ions.


So for you, 1M phosphoric acid would be 3 N, so 2M of phosphoric acid would be d. 6.0 N

Answer: d. 6.0 N

Answer 2

answer is (d) 6N Solute: A N = eq/L eq= mass A (g)/ eqw A (g/eq) So, N= mass A(g)/ (eqw A * L) eqw = Molecular weight / n (n is # of eq. in compound) H3PO4 MW = ninety seven.9952 n = 3 eqw=ninety seven.9952/3 = 32.665 Mass H3PO4 (g) = 2M = mol/L 2 moles consistent with a million L convert to g by ability of MW of H3PO4: 2mol *ninety seven.9952 g/mol=195.9904 g of solute N = 195.9904/(32.665 * 1L) N = 6

Answer 3

H3PO4 has 3 valence ( PO4 3-)
molar is weight/ atomic weight
normal is weight/ equivalent atomic weight

equivalent ---> atomic weight divide by valence.
normal = molar x valence

2M H3PO4 ----> 2 x 3 = 6 N

Answer 4

2.0molH3PO4/1LS x 3eqwtH3PO4/1molH3PO4 = 6 eqwt/L = 6.0N d. is correct.