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kow [346]
3 years ago
10

A 0.100-l sample of an unknown hno3 solution required 32.9 ml of 0.200 m ba(oh)2 for complete neutralization. what was the conce

ntration of the hno3 solution?
Chemistry
2 answers:
ddd [48]3 years ago
7 0
The reaction between HNO3 and Ba(OH)2 is given by the equation below;
2HNO3 + Ba(OH)2 = Ba(NO3)2 + 2H2O
Moles of Barium hydroxide used;
 = 0.200 × 0.039 l
 = 0.0078 Moles
The mole ratio of HNO3 and Ba(OH)2 is 2: 1
Therefore; moles of nitric acid used will be;
= 0.0078 ×2 = 0.0156 moles
But; 0.0156 moles are equal to a volume of 0.10
The concentration of Nitric acid will be; 
 =  (0.0156 × 1)/0.1 
 = 0.156 M
jok3333 [9.3K]3 years ago
4 0

Answer: 0.132 M

Explanation:

According to the neutralization law,

n_1M_1V_1=n_2M_2V_2

where,

M_1 = molarity of HNO_3 solution = ?

V_1 = volume of HNO_3 solution = 0.100 L = 100 ml (1L=1000ml)

M_2 = molarity of Ba(OH)_2 solution = 0.200 M

V_2 = volume of Ba(OH)_2 solution = 32.9 ml

n_1 = valency of HNO_3 = 1

n_2 = valency of Ba(OH)_2 = 2

1\times M_1\times 100=2\times 0.200\times 32.9

M_1=0.132

Therefore, the concentration of HNO_3 solution is 0.132 M

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DedPeter [7]

Answer:

The solution would need 13.9 g of KCl

Explanation:

0.75 m, means molal concentration

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Let's think as an aqueous solution.

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250 g will have (0.75 . 250)/1000 = 0.1875 moles of KCl

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