62 5. To what volume must each of the following be diluted to give the concentra

Question

62 5. To what volume must each of the following be diluted to give the concentration called for a. 10.0ml of 6.00N HNOs to give 0.200N solution (300m) b. 9.00ml of concentrated H.So. (18.0M) to give a 0.300M solution (540ml) 6. 24.60ml of 0.185N HNO, is titrated with 27.35ml of KOH solution. What is the normality of the KOH? (0.166N) 7. The molar mass of phosphoric acid is 98.0 grams, the following reactions? What is its equivalent weight in each of (32.7g) (98.0g) (49.0g) (32.7g) (98.0g) b. HsPO4NaOH NaH2PO4+ H2O c. H3PO4 + 2NaOH Na2HPO+ 2H20 e. H3PO4 + Ca(OH)2 Ca(H2PO4)2 + 2H2O Exp. 8.2

Explanation / Answer

5.

a) V1N1 = V2N2

Volume (x) of the HNO3 required for 0.2 N solution:

10*6 = x*0.2

x= (10*6)/0.2

= 300 ml

b) Volume (y) of the H2SO4 required

9 * 18 = y * 0.3

y= 540 ml

6. Normality (X) of the KOH required for the titration is

24.6 * 0.185 = 27.35 * X

X = 0.116 N

7. The equivalent weight of H3PO4:

Equivalent weight of an acid= (Molecular Mass)/ Basicity

Basicity is the maximum no of H+ ions liberated on dissociation

a) Basicity in the reaction is 3

thus 98/3= 32.7 g

b) Basicity is 1 as one H+ is liberated in the dissociation

Thus, 98/1 = 98 g

c) Basicity is 2.

Thus, 98/2= 49 g

d) Basicity is 3

thus, 98/3= 32.7 g

2) Basicity is 1

Thus, 98/1= 98 g

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