/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 35 The \(\mathrm{pH}\) of solutions... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 7: Problem 35

The \(\mathrm{pH}\) of solutions \(\mathrm{A}, \mathrm{B}, \mathrm{C}\) and \(\mathrm{D}\) are \(9.5,2.5,3.5\) and \(5.5\), respectively. The most acidic solution is (1) \(\mathrm{A}\) (2) \(\mathrm{B}\) (3) \(\mathrm{C}\) (4) D

Short Answer

Expert verified
Solution \(\text{B}\) with a \(\mathrm{pH}\) of \(2.5\) is the most acidic.

Step by step solution

01

Understand \(\mathrm{pH}\)

To determine the acidity of a solution, use the \(\mathrm{pH}\) scale. The \(\mathrm{pH}\) scale ranges from 0 to 14. A \(\mathrm{pH}\) less than 7 is acidic, a \(\mathrm{pH}\) of 7 is neutral, and a \(\mathrm{pH}\) greater than 7 is basic.
02

Compare \(\mathrm{pH}\) values

Identify which of the given \(\mathrm{pH}\) values is the lowest. The given \(\mathrm{pH}\) values are: \(9.5\) for solution \(\text{A}\), \(2.5\) for solution \(\text{B}\), \(3.5\) for solution \(\text{C}\) and \(5.5\) for solution \(\text{D}\).
03

Determine the most acidic solution

The solution with the lowest \(\mathrm{pH}\) value is the most acidic. Among the given \(\mathrm{pH}\) values, \(\text{B}\) with a \(\mathrm{pH}\) of \(2.5\) is the lowest.

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.

Over 30 million students worldwide already upgrade their learning with 91影视!

Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Acidity Determination
Acidity in chemistry is all about the concentration of hydrogen ions \(\text{H}^+\) in a solution. The more hydrogen ions a solution has, the more acidic it is. We measure this acidity using the \(\text{pH}\) scale. The \(\text{pH}\) scale ranges from 0 to 14. Here's a critical aspect to remember:
  • A \(\text{pH}\) value less than 7 indicates an acidic solution.
  • A \(\text{pH}\) value of exactly 7 is considered neutral, like pure water.
  • If the \(\text{pH}\) value is more than 7, the solution is basic (or alkaline).
So, for our given solutions, we can determine their acidity by checking where they fall on the \(\text{pH}\) scale. Solution B has a \(\text{pH}\) of 2.5, solution C has a \(\text{pH}\) of 3.5, and solution D has a \(\text{pH}\) of 5.5. Therefore, solution B is the most acidic since it has the lowest \(\text{pH}\).
Solution Comparison
When we compare the acidity of different solutions, we primarily look at their \(\text{pH}\) values. The \(\text{pH}\) value tells us how acidic or basic a solution is. Here's a simple way to compare:
  • The lower the \(\text{pH}\) value, the more acidic the solution is.
  • Conversely, the higher the \(\text{pH}\), the more basic the solution is.
  • Notice that the difference in \(\text{pH}\) values is logarithmic. This means a small change in \(\text{pH}\) indicates a significant change in \(\text{H}^+\) concentration.
For instance, moving from a \(\text{pH}\) of 3 to 2 doesn't just double the acidity; it makes it 10 times more acidic! This is because the \(\text{pH}\) scale is logarithmic (base 10). Comparing solutions A (9.5), B (2.5), C (3.5), and D (5.5), we see Solution B is the most acidic, followed by C, D, and then A.
Chemistry Fundamentals
At the heart of understanding acidity is the basic chemistry concept of ions and molecules in a solution. Here are a few fundamentals:
  • Acids release hydrogen ions (\(\text{H}^+\)) when dissolved in water.
  • Bases release hydroxide ions (\(\text{OH}^-\)) when dissolved in water.
  • The \(\text{pH}\) scale measures the concentration of hydrogen ions in a solution. The formula is \(\text{pH} = -\text{log}[\text{H}^+]\).
Remember, a strong acid fully dissociates in water, releasing more \(\text{H}^+\) ions. This results in a lower \(\text{pH}\) and higher acidity. Understanding these concepts can help you interpret the behavior of various solutions. For example, picking the most acidic solution is straightforward when you understand the \(\text{pH}\) scale and its logarithmic nature.

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

The \(\mathrm{pH}\) of a \(1 \times 10^{8} \mathrm{M}\) aqueous solution of \(\mathrm{HCl}\) is slightly less than 7 because(1) the ionization of \(\mathrm{HCl}\) is incomplete (2) the ionization of water is negligible (3) the ionization of water at such a low concentration of \(\mathrm{HCl}\) is significant (4) the ionization of both \(\mathrm{HCl}\) and water are negligible

The \(10^{4} \mathrm{Ka}\) values for the acids acetic, hydrofluoric, formic and nitrous are \(6.7,4.5,1.8\) and \(0.18\) but not in the correct order. The correct acid strengths arc (1) \(\mathrm{HF}=0.18, \mathrm{HNO}_{2}=1.8, \mathrm{HCOOH}=4.5\), \(\mathrm{CH}_{3} \mathrm{COOH}=6.7\) (2) \(\mathrm{HF}=6.7, \mathrm{HNO}_{2}=4.5, \mathrm{HCOOH}=1.8, \mathrm{CH}_{3} \mathrm{COOH}\) \(=0.18\) (3) \(\mathrm{HF}=1.8, \mathrm{HNO}_{2}=0.18, \mathrm{HCOOH}=4.5\), \(\mathrm{CH}_{3} \mathrm{COOH}=6.7\) (4) \(\mathrm{HF}=6.7, \mathrm{HNO}_{2}=0.18, \mathrm{HCOOH}=4.5\) \(\mathrm{CH}_{3} \mathrm{COOH}=1.8\)

Which of the following is correct? 1) \(K_{\mathrm{a}}\) (weak acid) \(\times K_{\mathrm{b}}\) (conjugate weak base) \(=K_{\mathrm{v}}\) 2) \(K_{\mathrm{a}}\) (strong acid) \(\times K_{\mathrm{b}}\) (conjugate strong base) \(=K_{\mathrm{w}}\) 3) \(K_{\mathrm{a}}\) (weak acid) \(\times K_{\mathrm{b}}\) (weak base) \(=K_{\mathrm{T}}\) 4) \(K_{\mathrm{a}}\) (weak acid) \(\times K_{\mathrm{b}}\) (conjugate strong base) \(=K_{\mathrm{w}}\)

Which of the following statements is wrong? (1) for an acid buffer solution the \(\mathrm{pH}\) can be increased by inereasing the concentration of salt (2) for a basic buffer solution the pH can increased by decreasing the concentration of base(3) buffer capacity of a buffer solution is maximum when the ratio of salt/acid or base is 1 (4) the number of moles of acid or base required by one litre of buffer solution to alter its \(\mathrm{pH}\) by one unit is called buffer efficiency

The equilibrium constant for the formation of \(\mathrm{H}_{2} \mathrm{O}(\mathrm{g})\) from the elements is extremely large and that for the formation of \(\mathrm{NO}(\mathrm{g})\) from its elements is very small. This implies that (1) \(\mathrm{H}_{2} \mathrm{O}\) has a tendency to decompose into its elements. (2) NO has low tendency to decompose into its elements. (3) NO has appreciable tendency to decompose into its elements. (4) NO cannot be produced from direct reaction between nitrogen and oxygen.
See all solutions

Recommended explanations on Chemistry Textbooks

Organic Chemistry

Read Explanation

Inorganic Chemistry

Read Explanation

Making Measurements

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Nuclear Chemistry

Read Explanation

Chemical Analysis

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.