Can someone please explain how to determine the pH and solve for this question using the chart attached? AAD3.4 5 6Bromcresol Green3.8-5.4What is the pH of the solutions based your calculations? Show thecalculated pH in the box provided. pH Indicator ChartAcidicBasicIndicator12 3456 7891011121314pH RangeThymol Blue1.2-2.8 and 8.0-9.2Methyl Orange3.0-4.4Bromphenol Blue3.0-4.6Congo Red3.0-5.0Bromcresol Green3.8-5.4Methyl Red4.4-6.2Bromthymol Blue6.0-7.6Phenol Red6.8-8.4Phenolphthalein8.2-10.0Thymophthalein9.3-10.5© 2019 Flinn Scientic, Inc. All Rights Reserved.AP7291FLINNSCIENTIFICYour Safer Source for Science

Answered: Image /qna-images/answer/0cd35d24-713b-4b44-a30c-d083eab6fd87.jpg

Answered: how to determine the pH

Science

Chemistry

how to determine the pH

General, Organic, and Biological Chemistry

7th Edition

ISBN:9781285853918

Author:H. Stephen Stoker

Publisher:H. Stephen Stoker

Chapter10: Acids, Bases, And Salts

Section: Chapter Questions

Problem 10.71EP

See similar textbooks

Related questions

Q: A TESTING FOR AN ACID Acids turn blue litmus paper red. Does the red litmus paper change color with…

A: Litmus paper is a paper which is stained with litmus used to indicate acidity or alkalinity of…

Q: conjugate pair of acids and base:

A: Conjugate pair of acids and bases just differ by one H+

Q: calculate the

A: Ammonium chloride (NH4Cl) is salt of weak base-strong type. pKb of weak base = 4.74 Concentration of…

Q: How can you determine if an anion will act as a weak base?

A: An anion will act as a weak base can be determined as,

Q: What is the pH

A: The equilibrium between the weak acid and its conjugate base allows the solution to resist changes…

Q: Please answer the question below correctly after taking the time to read it carefully. Use a…

A: Given that: pH=5 To find: The [H+]?

Q: the acidity and basicity.

A: Explanation: The species that gives [C=O]+ more easily, will be more easily hydrolyzed. Such ability…

Q: what is the pH?

A: Given :- concentration of weak acid = 0.230 M concentration of conjugate base = 0.410 M ka = 4.0…

Q: Calculate the pH of solutions with the following hydroxide ionconcentrations: Remember to use the…

A: pH is measure of acidity of a solution whereas the pOH is a measure of basicity of a solution. To…

Q: Calculate the pH of a 0.20 mol L-' solution of KCN. Express the pH numerically to two decimal…

Q: ٤ Hydrochloric acid solution with 0.015 M, if you take 50 ml from it and diluted by water to 150 ml…

Q: Acid mine drainage can be very harmful to living things that depend on the water of nearby…

A: Acid drainage water is acidic water that comes from metal mines. This usually comes from rock mines…

Q: determine the pH of a 0.002 M HCl solution. your answer must be within _+ 0.1%

A: determine the pH of a 0.002 M HCl solution.

Q: the pH of a solution is determined to be 4.43. what is the hydronium ion concentration of this…

A: pH is a scale to measure the concentration of hydrogen ions. The negative logarithm of hydrogen ion…

Q: Summary of acid and bases

A: An acid is any substance that can donate a proton to another substance when it dissolves it into…

Q: Calculate the [H+] in each of the following solutions, and indicate whether the solution is acidic…

Q: For each of the following substances, predict the pH when each is dissolved in water. If more…

A: When a salt is allowed to dissolve in water, then the salt will dissociate and reacts to form a new…

Q: What is the concentration of the hydroxide ion?

A: Given :- concentration of hydronium ion = 0.0017 M To calculate :- concentration of hydroxide ion…

Q: What is an acid base solution in a ph

A: Answer - pH Scale - The pH of a solution indicates its acidity or basicity (alkalinity). The pH…

Q: Which of the following are weak acids? Mark all that apply.

A: Weak acids are those which partially dissociate in electrolytic solution. and strong acids…

Q: Calculate the pH

Q: Use the rules for logarithms and exponents to solve for pH in terms of [H*]. NOTE: Capitalization…

A: The pH is then calculated using the expression: pH = - log [H+].

Q: nistry: Fundamentals and Principles presented by Ma ne compounds as acids, bases, or salts. Acid…

Q: For each molecular picture shown in the figure, determine the chemical formula, and the formula of…

Q: Predict whether the following NH4CN solution will be acidic, basic, or essentially neutral. Explain…

A: In case of salt hydrolysis one acid and one base are generated. If acid is stronger than base then…

Q: Can you solve for the pH given that you know the pOH? Why or why not?

A: Answer : Yes ,you can solve for the pH given that you know the pOH You can slove the pH if we know…

Q: Use the concentrations given to determine whether each of the following is acidic, neutral, or…

A: If the pH of a solution is less than 7, then it is acidic. When it is greater than 7, it is basic…

Q: What is ph how and how to use the formula?

A: The pH is the measure of the acidity or basicity a substance. The pH scale ranges from 0 to 14.A pH…

Q: veak acid. What is the pH of a solution that is

A: [H+] = √( Kw • C / Kb ) This above equation for salt Hydrolysis of NH4Cl [H+] = √( 10^-14 • 0.046…

Q: All the compounds having hydrogen atoms are not acids. Justify based on at least two acid base…

A: All the compounds having hydrogen atoms are not acids. This can be explained using the following…

Q: How would I the conjugate acid and the base including ions pair and electron

A: Conjugate acid is a species able to donate proton and formed by accepting a proton of a acid.…

Q: e CONJUGATE ACID for t

Q: 1.) Using your data from Part C including your initial pH and molarity, calculate the percent…

Q: 2. A solution with a pH of would be considered an acid. Оз 8 10

A: Answer - The correct option is (a) = 3 Explanation - The scale has values ranging from zero (the…

Q: strong or weak? acid

Q: Compare and contrast basic solutions with acidic solutions. In your answer, include the way the…

A: In the given question, Acids and bases are to be compared. The comparison of acid and bases…

Q: If the following salt was dissolved in water, select whether the cation and anion would be acidic,…

A: Salts that on dissolving make the solution acidic are called acidic salts. On the other hand, we…

Q: Calculate the pH

A: pH is used to determine the concentration of hydronium ion.

Q: ) Using your data from Part E including your initial pH and Kb, calculate the percent ionization for…

A: We have to find percentage ionization of ammonia Given pH = 10.18

Q: Draw the pH scale (with correct numerical reference). Label where acids, bases, neutral substances…

A: PH is defined as the negative logarithm of the H+ ion concentration. It was introduced by Sorensen.…

Q: calculate the pH

Q: Classify each salt as acidic, basic, or neutral. Drag the appropriate items to their respective…

A: Acidic salt: Produces strong acid and weak base after hydrolysis Basic salt: Produces weak acid and…

Q: A solution has a pOH =13, What is the of this solution?

A: pH of a solution is the measure of H+ ions. If pH is less than 7 then solution is acidic.If pH is…

Q: The concentration H* of a substance is 1010. Calculate the pH value and classify it as an acid or a…

Q: How can you increase the pH of a solution when The pH of its equal 7 ? O (a) By adding a small…

A: The negative logarithm of hydrogen ion concentration is defined as the pH of the solution. It is…

Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

100%

Can someone please explain how to determine the pH and solve for this question using the chart attached?

A
A
D
3.
4 5 6
Bromcresol Green
3.8-5.4
What is the pH of the solutions based your calculations? Show the
calculated pH in the box provided.

pH Indicator Chart
Acidic
Basic
Indicator
1
2 3
4
5
6 7
8
9
10
11
12
13
14
pH Range
Thymol Blue
1.2-2.8 and 8.0-9.2
Methyl Orange
3.0-4.4
Bromphenol Blue
3.0-4.6
Congo Red
3.0-5.0
Bromcresol Green
3.8-5.4
Methyl Red
4.4-6.2
Bromthymol Blue
6.0-7.6
Phenol Red
6.8-8.4
Phenolphthalein
8.2-10.0
Thymophthalein
9.3-10.5
© 2019 Flinn Scientic, Inc. All Rights Reserved.
AP7291
FLINN
SCIENTIFIC
Your Safer Source for Science

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Explain why an acid-base indicator changes color over a range of pH values rather than at a specific pH.
Two students were asked to determine the Kb of an unknown base. They were given a bottle with a solution in it. The bottle was labeled aqueous solution of a monoprotic strong acid. They were also given a pH meter, a buret, and an appropriate indicator. They reported the following data: volume of acid required for neutralization = 21.0 mL pH after 7.00 mL of strong acid added = 8.95 Use the students' data to determme the Kb of the unknown base.
A solution is made by dissolving 15.0 g sodium hydroxide in approximately 450 mL water. The solution becomes quite warm, but after it is allowed to return to room temperature, water is added to bring the volume to 500.0 mL of solution. (a) Calculate the pH and pOH in the final solution. (b) Why would we wait for it to return to room temperature? (c) If the mass of the water used to initially dissolve the sodium hydroxide were exactly 450 g and the temperature of the water increased by 8.865 C, how much heat was given off by the dissolution of 15.0 g of solute? Assume the specific heat of the solution is 4.184 J/g. K. What is the molar heat change for the dissolution of sodium hydroxide (known as the enthalpy of solution, Hsol)?
A drop of thymol blue gave a yellow color with a solution of aspirin. A sample of the same aspirin solution gave a yellow color with bromphenol blue. What was the pH of the solution? Was the solution acidic, neutral, or basic? (See Figure 15.10.)
Consider the following six beakers. All have 100 mL of aqueous 0.1 M solutions of the following compounds: beaker A has HI beaker B has HNO2 beaker C has NaOH beaker D has Ba(OH)2 beaker E has NH4Cl beaker F has C2H5NH2 Answer the questions below, using LT (for is less than), GT (for is greater than), EQ (for is equal to), or MI (for more Information required). (a) The pH in beaker A the pH in beaker B. (b) The pH in beaker C the pH in beaker D. (c) The % ionization in beaker A the % ionization in beaker C. (d) The pH in beaker B the pH in beaker E. (e) The pH in beaker E the pH in beaker F. (f) The pH in beaker C the pH in beaker F.
A solution has a pH of 4.5. What would be the color of the solution if each of the following indicators were added? (See Fig. 14-8.) a. methyl orange b. alizarin c. bromcresol green d. phenolphthalein
. The “Chemistry in Focus” segment Garden-Variety Acid— Base Indicators discusses acid-base indicators found in nature. What colors are exhibited by red cabbage juice under acid conditions? Under basic conditions?
Calculate the pH of each of the following solutions. (a) 10.0 mL of 0.300 M hydrofluoric acid plus 30.0 mL of 0.100 M sodium hydroxide (b) 100.0 mL of 0.250 M ammonia plus 50.0 mL of 0.100 M hydrochloric acid (c) 25.0 mL of 0.200 M sulfuric acid plus 50.0 mL of 0.400 M sodium hydroxide
Which of the following statements is(are) true? Correct the false statements. a. When a base is dissolved in water, the lowest possible pH of the solution is 7.0. b. When an acid is dissolved in water, the lowest possible pH is 0. c. A strong acid solution will have a lower pH than a weak acid solution. d. A 0.0010-M Ba(OH)2 solution has a pOH that is twice the pOH value of a 0.0010-M KOH solution.
Consider the process H2O H+(aq)+OH(aq)H=55.8kJ (a) Will the pH of pure water at body temperature (37C) be 7.0? (b) If not, calculate the pH of pure water at 37C.
. Choose the answer that best completes the following statement and defend your answer. When 100.0 mL of water is added to 100.0 mI of 1.00 M HCI. a. the pH decreases because the solution is diluted. b. the pH does not change because water is neutral. c. the pH is doubled because the volume is now doubled. d the pH increases because the concentration of H decreases e. the solution is completely neutralized.
A substance that functions to prevent rapid, drastic changes in the pH of a body fluid by changing strong acids and bases into weak acids and bases is called an: a.salt. b.buffer. c.enzyme. d.coenzyme.