Answered: A diprotic indicator H2L has pK,1 of…

A diprotic indicator H2L has pK,1 of 3.5 and pK2 = 7.5. At pH = 6.0, what is the principal species in solution? H2L L1 O L2 O H2L*1 HL-1

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.85QE

See similar textbooks

Related questions

Q: The pH of a 0.5L HNO2-NO2 buffer solution was determined to be 4.23. The solution was mixed with 5g…

A: Given, pH of buffer solution = 4.23 pKa = 4.35 Volume of buffer solution = 0.5 L weight of HNO2 = 5…

Q: The indicator thymol pink has a Ka = 2 x 10-4. At pH =1 it is yellow and at pH=14 it is pink.…

A: This question belongs to strong acid and weak base titration using a thymol pink indicator. find the…

Q: 6. Calculate volume in ml of 0.200 M NAOH solution required to neutralize 1.858 g of primary…

Q: A bottled carbonated mineral water (i.e. closed system) has a pH of 4.9 and an alkalinity of 4×10-³…

Q: 1. (a) Using activities correctly and the short form of the Debye-Hückel model, calculate the pH of…

A: i) To Calculate the pH of the solution using activities.

Q: Two aliquot of a water sample is titrated against a strong acid using phenolphthalein and…

A: Alkalinity is the quantity of an aqueous solution that is needed to neutralize the acidity that…

Q: A mixture contains Na2CO3, NaOH and inert matter. A sample weighing 1.500 g requires 28.85 ml of…

A: Introduction: The given sample has a mixture of Na2CO3 and NaOH, here we use two indicators like…

Q: Approximately 6 mL of conc. perchloric acid ( 72% ) was transferred to a bottle and diluted with…

A: Molarity of a solution is defined as the number of moles of solute present in one litre of a…

Q: 3. The colour changes corresponding to the pH intervals for the three indicators are given in the…

A: So according to the given data and the indicator we have the following conclusion. :

Q: A mixture of pure BaCO3 and pure Na2CO3 weighs 1.000 g and has the total neutralizing power of…

Q: Determination of sodium carbonate by acidimetric titration involves: Direct titration by acid…

A: Process of determination of sodium carbonate by acidimetric titration: CO32- + H+ → HCO3- HCO3- + H+…

Q: Describe the preparation of 100 mL 0.050 M and 100 mL 0.0050 M phosphate buffer (both having pH =…

A: A buffer is a solution that can resist pH change upon the addition of acidic and basic components.…

Q: A diprotic acid, H2A, has values of Kai = 1.0 x 10° and K2 = 1.0 x 101º. In a 0.10 M solution of…

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

Q: Which of the following statement of neutralization titration experiment is correct? 1. OBromocresol…

A: Titration is a typical quantitative chemical analysis laboratory method for determining the…

Q: 6. Calculate volume in mL of 0.200 M NaOH solution required to neutralize 1.858 g of primary…

A: Given -> Molarity of NaOH = 0.200 M Weight of potassium hydrogen phthalate = 1.858 gm Molar mass…

Q: A biochemist working with bacteria requires a culture buffered at a pH of 3.6. Which of the…

A: Given that: pH = 3.6 Buffer solution is mixture of weak acid and its conjugate base . Buffer…

Q: A series of acid-base indicators were added to four separate samples of a solution with an unknown…

A: The data given is,

Q: | NaOH IN 25x10³ Q3: In a carbonate mixture containing HCO, CO², and NaOH, either alone or…

Q: What are the common acid-base indicators for acidimetry-alkalimetry? Indicate the pH range and color…

Q: Please give

A: Given,Molarity of NaOH = 0.248M.Volume of NaOH = 18.71mL = 0.01871L.Volume of H2SO4 = 10.00mL =…

Q: 4. The molar absorptivities of the indicator weak acid HIn (K_{a} = 1.42 * 10 ^ - 5) and its…

Q: A 110.00 mL solution of 0.00195 M A3B2 is added to a 160.00 mL solution of 0.00155 M C3D4. What is…

A: Given: Volume of A3B2 = 110.0 mL concentration of A3B2 = 0.00195 M Volume of C3D4 = 160.0 mL…

Q: What is the function of the vacuum aspirator? Predict the color shift of the indicator as a…

A: Aspirator is a tool which uses suction to remove or collect something specially in medicine for…

Q: Given the chemical equation for the anthocyanin extract of red cabbage as an indicator. HIn + H20 S…

A: Indicator is a compound that indicates the acidic and basic character of the solution. These are…

Q: An alkaline sample of sodium compounds weighing 1.196 g was dissolved in water, cooled at 15 deg C,…

A: Alkaline compounds of sodium may involve sodium hydroxide (NaOH), sodium bicarbonate (NaHCO3) and…

Q: Indicator Measurement Colour of Indicator phenol red pOH = 6.8 Indicator Measurement Colour of…

Q: 3. Complete neutralization of 10 mL of phosphoric acid solution by NaOH 0.1 N in the presence of…

A: During titration of phosphoric acid we can use either methyl orange and detect first end point…

Q: v. What is pH? Calculate the pH for 0.0001N NH4OH solution of 100mL volume. The pKb value for NH4OH…

A: Ammonium hydroxide is a weak base. The dissociation of the weak base is given by: NH4OH ↔ NH4+ + OH-…

Q: which is tribasic(H3Y). 25cm^3 of lemon juice was diluted to 250cm^3. 25cm^3 of the solution was…

A: The question is based on the concept of solutions. we have to quantitatively estimate the citric…

Q: 200 ml of a water sample required 20 ml 0.025M Hydrochloric acid using methyl orange as indicator…

A: Alkalinity in water comes from sodium carbonate and sodium bicarbonate present in water. When…

Q: The Ka values for nitrous acid (HNO2) and hypochlorous (HClO) acid are 4.5 x10-4and 3.0 x10-8,…

A: The pKa values of HNO2 and HClO is calculated below. The pKa of HClO is closer to the required pH…

Q: How much amount (in grams) do you need to prepare the following solutions 500.0 mL 0.1000 M stock…

A: Concept: The molarity of a solution can be calculated as the number of moles of solute divided by…

Q: Use acid-base titration to determine the concentration of: – A strong acid: HCl -0.100 M HCl…

A: pH = -log[H+]

Q: If the absorbance of one of the buffer solutions (pH = 4.604) was 0.314 and the absorbance of the…

Q: Determine the pH of a solution containing 0.030 M NaOH and 0.025 M KI neglecting activities.

A: The answer to the following question is-

Q: Calculate the volume in liters of 0.545 M KOH necessary to titrate 0.0113 moles of hydrochloric…

Q: What will the pH of the mixture that contains: 250 mL of 0.12 M of H2SO4 and 150 mL of 0.04 M of…

A: Let's first consider the neutralization reaction between H2SO4 and NaOH.

Q: Consider the following indicators: dinitrophenol (pKin = 3.5), bromothymol blue (pKın = 7),…

A: Indicators are the chemical components used in titrations (acid-base). They are added in a small…

Q: Methyl orange is an indicator used for detecting the pH of acidic solutions. The red, protonated…

Q: In a lab, dissociation constant, K, of an acid-base indicator is measured. A 1.00 x 104 M solution…

A: Concentration (C) of the indicator = 1.00 x 10-4 M path length (l) of cuvette = 1.00 cm Molar…

Q: What Volume of the titrant is needed to reach the End Point having 5g of sample and 1N H2SO4 as a…

A: According to law of equivalence, an acid exactly neutralizes the same number of equivalents of base…

Q: A sample of material contains the components NaOH, Na2CO3, NaHCO3 , or possible mixtures of these.…

A: Weight of sample = 1 g normality of acid = 1.038 N

Q: Given that the Ka value of Thymolphthalein, weak acid and acid-base indicator, is equal to 1 x…

A: 1- In this question, we want to determine the pH of the solution in which indicator change the color…

Q: When adding 25 ml of a pulverizer containing a solution of M (NaOH 0.2) to a beaker containing 50 ml…

A: The acidic function is measure of the acidity of the solution and the most commonly used acidity…

Q: A weak acid (HA) with a pKa of 4.0 has a distribution constant of 5.2 between an organic and aqueous…

A: The fraction of HA acid in the organic phase at pH 2 and 6 is calculated:

Q: A solution contains Na2CO3 and NaHCO3. 10 mL of the solution required 2.5 mL of 0.1 M H2SO4 for…

Q: The acid-base indicator "Thymol Blue" has two transition ranges as listed below (with the…

A: The pKa values of the forms of thymol blue can be calculated as: pKa=-log Ka

Q: Mr. Clean recently bought a laboratory-grade sodium carbonate from a chemical company known as Brand…

Question

100%

A diprotic indicator H2L has pK,1 of 3.5 and pK2 = 7.5. At pH = 6.0, what is the principal species in solution?
H2L
L-1
O L2
O H2L*1
HL-1

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

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

Given three acid-base indicatorsâ€”methyl orange (end point at pH 4), bromthymol blue (end point at pH 7), and phenolphthalein (end point at pH 9)â€”which would you select for the following acid-base titrations? (a) perchloric acid with an aqueous solution of ammonia (b) nitrous acid with lithium hydroxide (c) hydrobromic acid with strontium hydroxide (d) sodium fluoride with nitric acid
Phenolphthalein is a commonly used indicator that is colorless in the acidic form (pH 8.3) and pink in the base form (pH 10.0). It is a weak acid with a pKa of 8.7. What fraction is in the acid form when the acid color is apparent? What fraction is in the base form when the base color is apparent?
3. Complete neutralization of 10 ml of phosphoric acid solution by NaOH 0.I N in the presence of phenol phthalein until the appearance of purple color (pH, = 9) 11 ml. of NaOH is consumed. (a) What is the concentration of phosphoric acid? (b) Calculate the indicator error. pk2.1 pK. - 7.2 pK - 124
A solution contains KHCO3, K2CO3 and KOH either alone or in permissible combination. A 50.0 mL aliquot requires 25.0 mL of 0.100 M HCI to reach the phenolphthalein end point. Another 50.0 mL aliquot requires 45.0 mL of the same acid to reach the bromocresol green end point. Which of the following statements BEST describes the composition of the sample solution? O The solution contains more KOH than K2CO3. O The solution contains K2CO3 only. O The solution contains more KHCO3 than K2CO3. O The solution contains a mixture of KHCO3 and KOH. O The solution contains KOH only. O The solution contains more K2CO3 than KOH.
Consider the spectrophotometric pH measurement of seawater with the indicator thymol blue illustrated at the opening of this chapter. The blue form of the indicator In22 on page 202 has maximum absorbance at a wavelength of 596 nm (nanometers). The yellow form HIn2 has maximum absorbance at 435 nm. Measurements of absorbance at the two wavelengths allows us to find the ratio [In22]/[HIn2]. How would you use this measurement to find the pH?
You are asked to prepare a 200.0 mL buffer solution of pH 8.52 from the following hypohalous acids: Hypobromous acid, HBro Hypochlorous acid, HCIO Hypoiodous acid, HIO (Ka = 2.0 x 10) (K, = 3.0 x 10) (Ka = 2.0 x 10-11) The available reagents are 5.0 M each of the acids and solids NaCIO (74.44 g/mol), NaBro (118.9 g/mol) and Nalo (165.9 g/mol). a. What would be the concentration of the salt if the required concentration of the acid component is 1.00 M? b. How much of the acid will you use? c. How much of the salt is needed?
From the following choose the most appropriate weak base (when added to its conjugate acid) for making a buffer with pH = 4.50 O (CH3)3N (K, = 6.4 x 105) %3D O CgH5NH2 (K = 3.9 x 1010) O C2H5NH2 (Kg = 5.6 x 104) O HONH2 (K, = 1.1x 108) %3D O NH3 (K5 - 1.8 x 10 5)
Given the following hydrolysis constants, which of the salts has the weakest parent ACID? K₂ or K, for salt 3.3 x 10-7 5.6 x 10-10 5.6 x 10-10 5.0 x 10-6 (A) (B) (C) (D) SALT NaClO2 NH4NO3 C₂H302 C₂H5NHBr NaCN A E B 2.5 x 10-5.
A certain indicator, HA, has a Ka value of 6.3 x 10-7. The protonated form of the indicator is yellow and the ionized form is red. What is the pKa of the indicator? pK₂ = What is the color of this indicator in a solution with pH = 4? yellow red orange
If the pka of the indicator is approximately 6, to which of the following equivalence point will it be most suitable? (A) pH 4 B pH 5 С) рH 13 (D) рH 10
A student used 9.925 x 10-2 mol/L hydrobromic acid to standardize an aqueous solution of potassium hydroxide and obtained the following titration data using phenolphthalein as an indicator: Concentration of HBr used: 9.925 x 10-2 mol/L Volume of HBr used: 25.00 mL Indicator: phenolphthalein Endpoint colour change: colorless to pale pink Table 1: Volume of Potassium Hydroxide Required Burette reading (mL) Trial 1 Trial 2 Trial 3 Final reading 29.28 36.62 43.98 Initial reading 1.78 9.28 16.62 Volume of KOH used (mL) Average of 2 closest values to within 0.10 mL: Questions Complete Inclosed table Write the molecular equation for the reaction that occurs between potassium hydroxide and hydrobromic acid. Calculate the molar concentration, in mol/L, of the aqueous potassium hydroxide.
The titration of Na₂CO3 (H₂CO3 has a pka1 = 6.37 and pka2 = 10.32) against HCl(aq) is depicted below: pH B V₁ V₂ mL HC1 E F a) Identify the major species in solution at points A - F. b) For the titration of 25.00 mL of 0.100 M Na₂CO3 against a 0.100 M HCl solution: i) calculate V₁ and V₂ ii) calculate the pH at points A - E. Note: points B and D are halfway points to equivalence.