At 298.K and 1.00 atm, assume that 22 mL of NO gas reacts with 18 mL of
oxygen gas and excess water to produce nitric acid according to the following
equation:
O (g) H O(l) 2 HNO (g)
2
3
2NO(g) + 2 + 2 ¾¾® 3 .
If all of the nitric acid produced by this reaction is collected and then dissolved
into 25 mL of water, what would be the pH of the resulting solution?
Your post is garbled because you tried to use spacing. The board ignores all spaces after the first one. Just write formulas like the rest of us do.
NO is NO. NO2 is NO2, N2O5 is N2O5.
To determine the pH of the resulting solution after dissolving the nitric acid, we first need to calculate the concentration of the acid in the solution.
Step 1: Calculate the number of moles of nitric acid produced
We start by finding the moles of nitric acid produced from the reaction. To do this, we need to convert the given volumes of NO gas and oxygen gas to moles using the ideal gas law equation: PV = nRT.
For NO gas:
P = 1.00 atm (given)
V = 22 mL (given)
T = 298 K (given)
R = 0.0821 L.atm/mol.K (ideal gas constant)
Using the ideal gas law equation:
n(NO) = (P x V) / (R x T)
n(NO) = (1.00 atm x 0.022 L) / (0.0821 L.atm/mol.K x 298 K)
n(NO) = 0.00091 mol
Since the stoichiometric coefficient of NO is 2, the number of moles of nitric acid produced is:
n(HNO3) = 2 x n(NO) = 2 x 0.00091 mol = 0.00182 mol
Step 2: Calculate the concentration of nitric acid in the solution
Next, we need to calculate the concentration of the nitric acid in the resulting solution. To do this, we use the formula:
Concentration (M) = moles of solute / volume of solution (in liters)
Given:
Volume of solution = 25 mL = 0.025 L (convert to liters)
Concentration (HNO3) = 0.00182 mol / 0.025 L
Concentration (HNO3) = 0.0728 M
Step 3: Calculate the pH of the resulting solution
The pH of a solution can be determined using the equation:
pH = -log[H+]
Since nitric acid is a strong acid, it dissociates completely in water to release H+ ions. Therefore, the concentration of H+ ions in the solution is equal to the concentration of HNO3:
[H+] = 0.0728 M
Using the equation, we can calculate the pH:
pH = -log(0.0728)
pH ≈ 1.14
Therefore, the pH of the resulting solution after dissolving the nitric acid is approximately 1.14.