Chapter 5, Problem 5.112PAE

Interpretation Introduction

Interpretation:

Nitric acid can be prepared by bubbling dinitrogen pentoxide into water.

${\text{N}}_{\text{2}}{\text{O}}_{\text{5}}\left(\text{g}\right){\text{+H}}_{\text{2}}\text{O}\left(\text{l}\right)\to {\text{2H}}^{\text{+}}\left(\text{aq}\right){\text{+2NO}}_3^{-}\left(\text{aq}\right)$

1. When 1.50 L of ${\text{N}}_{\text{2}}{\text{O}}_{\text{5}}$ at $25{}^{\circ }\text{C}$ a and 1.00 atm pressure is bubbled into water, number of moles of ${\text{H}}^{+}$ needs to be determined.
2. The solution obtained in part (a) after reaction is complete has a volume of 437 mL. The molarity of the nitric acid should be calculated.

Concept introduction:

An ideal gas which is known as the perfect gas is a gas whose volume V, Pressure P and temperature T are related through the ideal gas

$\text{PV = nRT}$

Here,

n = number of moles of the gas

R = ideal gas constant

T = Temperature

P = Pressure

Also, molarity is defined as number of moles of solute present in 1 L volume of solution.

$\text{M}=\frac{\text{n}}{\text{V}}$

Here, n is number of moles of solute and V is volume of solution.

Given:

${\text{N}}_{\text{2}}{\text{O}}_{\text{5}}\left(\text{g}\right){\text{+H}}_{\text{2}}\text{O}\left(\text{l}\right)\to {\text{2H}}^{\text{+}}\left(\text{aq}\right){\text{+2NO}}_3^{-}\left(\text{aq}\right)$

a) $1.50\text{ L}$ of $N_2{O}_5$ at $25\text{ °C and 1atm}$

b) Volume= $437\text{ mL}$