Question

Number of moles of H2O formed when 25ml of 0.1 M HNO3 solution is completely neutralised by NaOH is
(A)2.5×10^-4
(B)2.5×10^-3
(C)2.5×10^-2
(D)2.5×10^-1​

Answer 1

Answer:

(B)2.5×10^-3 is the correct answer

Explanation:

The equation of the reaction is :

$\mathbf {HNO_3 + NaOH \longrightarrow NaNO_3 + H_2O}$

So, for 1 mole HNO₃ with neutralization of 1 mole of NaOH,  we get 1 mole of H₂O

Given that 25ml of 0.1 M HNO₃ solution

We know that

$\boxed {Molarity = \dfrac{Number \ of \ moles \times 1000}{Volume \ in \ ml} }$

So, substituting the values, we get,

$0.1 = \dfrac{Number \ of\ moles \times 1000}{25}$

$: \longmapsto \text{Number of moles} = 2.5 \times 10^{-3}$

So, number of moles of HNO₃ used up are 2.5 × 10⁻³

As number of moles of HNO₃ spent and H₂O are same

2.5 × 10⁻³ moles of H₂O are formed

Hence, Option (B) is correct

Hope it helps!