Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 15: Problem 51

What is the \(\mathrm{pH}\) of aqueous solutions of the strong acid \(\mathrm{HNO}_{3},\) nitric acid, if the concentrations of the solutions are as follows: (a) \(0.005 \mathrm{M},(\mathrm{b}) 0.05 \mathrm{M},(\mathrm{c}) 0.5 \mathrm{M},(\mathrm{d}) 5 \mathrm{M} ?\)

Short Answer

Expert verified
The pH values for the HNO3 solutions of concentrations 0.005 M, 0.05 M, 0.5 M and 5.0 M respectively are approximately 2.3, 1.3, 0.3 and -0.7.

Step by step solution

01

Calculate pH for a 0.005M HNO3 solution

Using the formula for calculating pH, which is \(pH = -\log[H^+] \), replace the [H+] with the concentration of the HNO3 solution given. In this case, pH equals -log(0.005). Calculate the value using a calculator.
02

Calculate pH for a 0.05M HNO3 solution

Again use the formula \(pH = -\log[H^+] \), and replace the [H+] with the concentration of the HNO3 solution given, which is now 0.05. The calculation will now be pH = -log(0.05). Calculate the value using a calculator.
03

Calculate pH for a 0.5M HNO3 solution

With the same formula \(pH = -\log[H^+] \), replace the [H+] with the concentration of the HNO3 solution, which is now 0.5. The calculation will now be pH = -log(0.5). Calculate the value using a calculator.
04

Calculate pH for a 5M HNO3 solution

Lastly use the formula \(pH = -\log[H^+] \), and replace the [H+] with the concentration of the given HNO3 solution, which is 5 this time. So, pH = -log(5). Calculate the value using a calculator.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

If 25 \(\mathrm{mL}\) of 1.00 \(\mathrm{M} \mathrm{HCl}\) is mixed with 75 \(\mathrm{mL}\) of \(1.00 \mathrm{M} \mathrm{NaOH},\) what are the final amounts and concentrations of all ions present?

If 18.5 \(\mathrm{mL}\) of a 0.0350 \(\mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}\) solution neutralizes 12.5 \(\mathrm{mL}\) of aqueous LiOH, what mass of LiOH was used to make 1.00 \(\mathrm{L}\) of the LiOH solution?

Find \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) in a solution of \(\mathrm{pH} 4\).

What product do all neutralization reactions have in common?

Why is it important to slow down the drop rate of the buret near the end of a titration?
See all solutions

Recommended explanations on Chemistry Textbooks

Organic Chemistry

Read Explanation

Kinetics

Read Explanation

The Earths Atmosphere

Read Explanation

Making Measurements

Read Explanation

Chemical Analysis

Read Explanation

Nuclear Chemistry

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free