:://:::: The acid form of an indicator is yellow and its anion is blue. The K₂ of this indicator is 10-5. Whatwill be the approximate pH range over which this indicator changes color?4 < pH < 66 < pH < 85 < pH <73 < pH < 5

Answered: Image /qna-images/answer/23b6e811-028e-42de-933f-8a78d904cf76.jpg

-5 What The acid form of an indicator is yellow and its anion is blue. The K₂ of this indicator is 10 will be the approximate pH range over which this indicator changes color? 4 < pH < 6 6 < pH < 8 5

-5 What The acid form of an indicator is yellow and its anion is blue. The K₂ of this indicator is 10 will be the approximate pH range over which this indicator changes color? 4 < pH < 6 6 < pH < 8 5

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 9RQ: What is an acidbase indicator? Define the equivalence (stoichiometric) point and the end point of a...

See similar textbooks

Related questions

Q: 6. If the temperature of the equilibrium system above is decreased and the concentrations of the…

A: 6. If the reaction is exothermic, heat can be considered as a product. If the reaction is…

Q: For the gas phase isomerization of isopropenyl allyl ether,…

Q: Phosgene (carbonyl chloride), 12, is an extremely loxic What is the equilibrium constant, Kp, of…

Q: Todd wondered what would happen if he could remove all the atoms in a metal spoon. He asked his…

A: The concept behind the answer is based on the fundamental principles of the structure of matter.…

Q: Draw the product of the reaction between a ketone and an alcohol. Include all hydrogen atoms in the…

Q: 42 Determine the molar mass for the following compounds: a. ethylene, a ripening hormone, C₂H4 b.…

A: The molar mass is the mass of one mole of a substance, expressed in grams per mole (g/mol). To…

Q: How would you draw the isomer structure(s) for [Fe(C2O4)2(H2O)2] 0

A: Since, Isomer are those whose molecular formula same but structural formula is different. Thus,

Q: O Macmillan Learning A 0.538 g sample of steam at 105.3 °C is condensed into a container with 5.77 g…

A: specific heat: The specific heat capacity, or the amount of heat needed to raise the temperature of…

Q: If 3 quarts of juice fill 15 glasses, how many glasses will 12 quarts of juice fill? [?] glasses

A: Explanation :- Above problem will be solved by unitary method . The unitary method is a…

Q: What is the empirical formula of a compound composed of 3.25% hydrogen (H), 19.36% carbon (C), and…

A: We have to calculate the empirical formula of the compound

Q: Some polyatomic ions name 0 0 chemical formula W CH,CO, NH. 4 BrO 3 CO3

A: Since, Naming the compound,first write name of cation then after anion. Thus,

Q: Write a K₂ expression for the reaction: H₂PO4 (ag) = 3H* 3- Pou (14) 3H+PO

A: Equilibrium constant (Kc) expression for the reaction:

Q: Identify the conjugate bases corresponding to the following acids: a) [Co(NH3)(OH₂)]³+ b) HSO4 c)…

A: Conjugate acid-base pair is the pair of compounds that differ by a proton. A proton is added to…

Q: What is the relationship between the following two compounds? H CH3 HC H OH Н and A) identical B)…

A: In this question, We will identifying the relationship between the two compounds which have two…

Q: a) (CH3)2CHCH(C₂H5)CH₂CH₂CH3 b) CH2=C(C₂H5)CH₂C(CH3)2CH3 c) (CH3)2C=CHC(C₂H5)=CH₂ d) CH3(CH₂)…

A: The following are suggested steps for drawing a line-angle structure Remove all hydrogens bonded to…

Q: Provide the intermediates, reagents, and product needed to complete this synthesis. Ignore inorganic…

Q: Consider the equilibrium system described by the chemical reaction below. At equilibrium, a sample…

A: This can be explained as :

Q: 9. Calculate the pH of a 0.20 M solution of iodic acid (HIO3 and K₂ = 0.17). [78] 10. Calculate the…

A: “Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: A Mass of empty evaporating dish + watch glass 65.362 g B Mass of dish + watch glass + initial solid…

Q: Problem 2: Calculate the formal charges to determine the most probable Lewis structure for the…

A: The formal charge of an atom in a molecule is defined as the charges acquire in the molecule. Formal…

Q: Give 3 examples of chemical equilibrium expressions that are important to day-to-day life/activities…

A: Chemical equilibrium is chemical equilibrium means that reaction which is in chemical equilibrium.…

Q: 2- Write the ROpo (RO)3P + PMC3 Co 03Pl O||!!.. H PMe3

A: A basic discussion of the complex to get the plausible mechanism.

Q: Exercise 15.3: The resistance of 0.1 M KCl solution in a conductance cell is 325 ohms and the…

A: The resistance of 0.1 M KCl solution in a conductance cell is 325 ohms and the specific conductance…

Q: Balance the following reaction: C₂H₂ + 0₂ → CO₂ The answer choices below list the coefficients for…

A: we have to balance the given equation and determine the coefficients

Q: Attached is the NMR data sheet for 4-cyclohexene-cis-dicarboxylic anhydride. How do I interpret it…

A: Integration is generally the number of one type of proton due to which signal arises (in the above…

Q: What decimal power does the abbreviation f represent? O 1 x 106 O 1 x 10³ O 1 x 10-1 O 1 x 10-15 O 1…

Q: Consider alkene 1. میشه ما تے ہیں H3C. H3C H₂C CH₂ CH H₂C Consider alkene 2. H Consider alkene 3. ΤΟ…

A: IUPAC nomenclature is a set of rules and conventions for naming organic compounds. The goal of IUPAC…

Q: Please provide only typed answer solution no handwritten solution needed allowed

A: Note: Since you have asked multiple questions, we will solve the first question for you. If you want…

Q: What is change in heat when vaporizing a 50.0 g of sample of Compound A that is already at its…

A: What is change in heat when vaporizing a 50.0 g of sample of Compound A that is already at its…

Q: A chemist is studying the following equilibirum, which has the given equilibrium constant at a…

A: Answer:- This question is answered by using the simple concept of calculation of equilibrium…

Q: student, lets call her cindy, was trying to carry out a grinard synthesis. The reaction simply would…

Q: Name the following ionic compounds: a. AlCl3 b. NH4C₂H₂O2 d. K3PO4 c. AgBr e. CsF f. MnO tole

Q: Please provide only typed answer solution no handwritten solution needed allowed

A: Given: The equilibrium concentration of CO is 0.0520M. The equilibrium concentration of H2 is…

Q: I neesd help with questions 1-8 in the above questions.

A: We have to answer the following questions NH4Cl compound is acidic, basic or neutral. Write the…

Q: Exercise 5.17: Justify that vibrational transitions in HCl are generally observed from v = = 0 to v…

A: Vibrational transition: Vibrational transitions are in actuality transitions between rotational…

Q: The following initial rate data are for the reaction of nitrogen dioxide with fluorine: 2NO+2H2 -->…

A: Recall the given reaction, 2 NO + 2 H2 → N2 + 2 H2OWe have to…

Q: For the general gas phase reaction 2 A + 3 B ↔ 2 C the equalibrium constant is 5.00. Calculate the…

A: The conditions for determining the direction of a chemical reaction in terms of the equilibrium…

Q: WS-3.7: How will you synthesize the compound below without rearrangements? Provide the mechanism for…

A: To synthesize the following compound without rearrangements and provide a mechanism:

Q: 3)Consider the following system, which is at equilibrium, CO(g) + 3H2(g) CH4(g) + H2O(g). Predict…

A: If we add product, equilibrium goes left, away from the product. If we remove…

Q: · 0 DZL Discussion 2 - Public Speaking Sec... = www-awu.aleks.com A ALEKS-Jacari Johnson - Learn…

A: We have been asked to draw the condensed structural formula of 2° alcohol having four carbon atums,…

Q: The conversion of methyl isonitrile to acetonitrile in the gas phase at 250 °C CH3NC(g) ---> CH3CN…

A: Given that, Rate constant=3.00 × 10-3 s-1 Initial concentration= 0.0358 M Time =442 s then,

Q: Classify each of the molecules below. OH O primary alcohol Osecondary alcohol C tertiary alcohol C…

A: There are three types of alcohol on the basis of carbon that is directly attached with oxygen :…

Q: solution A lead(II) nitrate zinc nitrate zinc chloride solution B potassium iodide potassium…

A: The explanation is given below-

Q: 4 The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an…

Q: A sample of 3.10 mol of helium is confined at low pressure in a volume at a temperature of 80 °C.…

A: Given , moles of helium in sample = 3.10 mol Temperature , T = 80°C

Q: How many moles of barium chloride (BaCl2) are in 81.5 g of the compound?

Q: What are the approximate pKa values for the groups marked with arrows? 3² 1 ОН NH₂ 2 3 OH SH 4 ОН 5

A: pKa is an index to express the acidity of acids. pKa = -logKa , where Ka is dissociation constant.…

Q: A 1.440 M solution of CH3OH Express the molarity as an integer. B. 0.21 MM solution of…

A: We are given the molarity of solution as 1.440 M and we need to write this value as an integer. And,…

Q: ed a 7 (d) Word Equation: 8 Blue → no change 9 (d) Word Equation: White, Cloudy Sodium Carbonate +…

A: As per the student's request I'm solving only question number 7,8 & 9. We have to write the…

Q: 5. Again, regarding the experiment completed in lab, draw a separatory funnel and identify all…

A: As you have asked for Q.6. hence providing you the solution for the same. Introduction Salicylic…

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%

:://::::

The acid form of an indicator is yellow and its anion is blue. The K₂ of this indicator is 10-5. What
will be the approximate pH range over which this indicator changes color?
4 < pH < 6
6 < pH < 8
5 < pH <7
3 < pH < 5

Expert Solution

This question has been solved!

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

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

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

Sketch the titration curve for a weak acid titrated by a strong base. When performing calculations concerning weak acidstrong base titrations, the general two-slep procedure is to solve a stoichiometry problem first, then to solve an equilibrium problem to determine the pH. What reaction takes place in the stoichiometry part of the problem? What is assumed about this reaction? At the various points in your titration curve, list the major species present after the strong base (NaOH, for example) reacts to completion with the weak acid, HA. What equilibrium problem would you solve at the various points in your titration curve to calculate the pH? Why is pH 7.0 at the equivalence point of a weak acid-strong base titration? Does the pH at the halfway point to equivalence have to be less than 7.0? What does the pH at the halfway point equal? Compare and contrast the titration curves for a strong acidstrong base titration and a weak acidstrong base titration.
Metacresol purple is an indicator that changes from yellow to purple at pH 8.2. (a) What is Ka for this indicator? (b) What is its pH range? (c) What is the color of a solution with pH 9.0 and a few drops of metacresol purple?
Amino acids are an important group of compounds. At low pH, both the carboxylic acid group (CO2H) and the amine group (NHR) are protonated. However, as the pH of the solution increases (say, by adding base), the carboxylic acid proton is removed, usually at a pH between 2 and 3. In a middle range of pHs, therefore, the amine group is protonated, but the carboxylic acid group has lost the proton. (This is called a zwitterion.) At more basic pH values, the amine proton is dissociated. What is the pH of a 0.20 M solution of alanine hydrochloride, [NH3CHCH3CO2H]Cl?
Sketch a titration curve for the titration of potassium hydroxide with HCl, both 0.100 M. Identify three regions in which a particular chemical species or system dominates the acid-base equilibria.
A diprotic acid, H2B(MM=126g/moL), is determined to be a hydrate, H2B xH2O. A 10.00-g sample of this hydrate is dissolved in enough water to make 150.0 mL of solution. Twenty-five milliliters of this solution requires 48.5 mL of 0.425 M NaOH to reach the equivalence point. What is x?
8-71 Explain why you do not need to know the chemical formula of a buffer compound to use it.
A friend asks the following: Consider a buffered solution made up of the weak acid HA and its salt NaA. If a strong base like NaOH is added, the HA reacts with the OH to form A. Thus the amount of acid (HA) is decreased, and the amount of base (A) is increased. Analogously, adding HCI to the buffered solution forms more of the acid (HA) by reacting with the base (A). Thus how can we claim that a buffered solution resists changes in the pH of the solution? How would you explain buffering to this friend?
Using the diagrams shown in Problem 10-117, which of the solutions would have the greatest buffer capacity, that is, greatest protection against pH change, when the following occurs? a. A strong acid is added to the solution. b. A strong base is added to the solution.
Determine the dominant acid-base equilibrium that results when each of the following pairs of solutions is mixed. Indicate the equilibrium by writing 1 for a strong acid, 3 for a weak acid, 4 for an acidic buffer, 7 for a neutral solution, 10 for a basic buffer, 11 for a weak base, and 13 for a strong base. (a) 10.0 mL of 0.15 M NaOH + 15.0 mL of 0.10 M HNO3 (b) 25.0 mL of 0.10 M HCl + 10.0 mL of 0.25 M NH3 (c) 50.0 mL of 0.050 M NaOH + 50.0 mL of 0.10 M NH3 (d) 50.0 mL of 0.10 M NH3 + 50.0 mL of 0.05 M HCl
8-55 We commonly refer to a buffer as consisting of approximately equal molar amounts of a weak acid and its conjugate base—for example, CH3COOH and CH3COO-. Is it also possible to have a buffer consisting of approximately equal molar amounts of a weak base and its conjugate acid? Explain.
You have a solution of the weak acid HA and add some of the salt NaA to it. What are the major species in the solution? What do you need to know to calculate the pH of the solution, and how would you use this information? How does the pH of the solution of just the HA compare with that of the final mixture? Explain.
. How is the strength of an acid related to the fact that a competition for protons exists in aqueous solution between water molecules and the anion of the acid?