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Chapter 15: Problem 186

If \(100 \mathrm{~mL}\) of an aqueous solution of nitric acid contains \(0.030\) mole of \(\mathrm{HNO}_{3}\), what is the \(\mathrm{pH}\) of the solution?

Short Answer

Expert verified
The pH of the aqueous solution of nitric acid containing 0.030 moles of HNO3 in 100 mL of solution is approximately 0.52.

Step by step solution

01

Calculate the concentration of HNO3 in the solution

Given that the aqueous solution has a volume of 100 mL and contains 0.030 moles of HNO3, we can calculate the molarity (concentration in moles per liter) of HNO3 in the solution using the formula: Molarity (M) = moles of solute / liters of solution First, convert the volume to liters: 100 mL = 0.100 L Now, plug the values into the molarity formula: Molarity (M) = 0.030 moles / 0.100 L Molarity (M) = 0.30 M
02

Calculate the concentration of hydrogen ions (H+) in the solution

Since nitric acid (HNO3) is a strong acid and it completely dissociates in water, the concentration of H+ ions is equal to the concentration of HNO3 in the solution. Therefore, the concentration of H+ ions in the solution is 0.30 M.
03

Calculate the pH of the solution

Now that we have the concentration of hydrogen ions (H+), we can find the pH using the formula: pH = -log10[H+] Where [H+] is the concentration of hydrogen ions in the solution. Plug the [H+] value into the pH formula: pH = -log10(0.30) pH ≈ 0.52 So, the pH of the aqueous solution of nitric acid containing 0.030 moles of HNO3 in 100 mL of solution is approximately 0.52.

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Most popular questions from this chapter

When water undergoes autoionization, is it serving as an acid, a base, or neither? Explain.

What is the general recipe for making a buffer? Explain the function of each ingredient.

Perchloric acid, \(\mathrm{HClO}_{4}\), is a strong acid. (a) Write the chemical equation for the reaction between perchloric acid and water. (b) List all species present in an aqueous solution of perchloric acid in order of concentration, highest to lowest. (c) Calculate the concentration of all species (except \(\mathrm{H}_{2} \mathrm{O}\) ) present in a \(0.100 \mathrm{M} \mathrm{HClO}_{4}\) solution. (d) What is the \(\mathrm{pH}\) of this solution?

Aniline, \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{2}\), is a weak base, with a lone pair of electrons on the nitrogen atom. (a) According to Bronsted and Lowry, what must aniline do to act as a base? (b) Why can aniline act as a base? (c) What are the molecular formula and charge of the conjugate acid of aniline?

If you dissolve \(0.250 \mathrm{~g}\) of \(\mathrm{Ba}(\mathrm{OH})_{2}\) in \(3.00 \mathrm{~L}\) of water, what is the \(\mathrm{pH}\) of the solution?
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