The titration curve of a weak acid, HnA has 3 inflection points atpH = 3.5, 6.7 and 10.3. If 0.1 M of a buffer, pH 4.2 is to be preparedusing the weak acid and its conjugate base, what will be thecomponents of this buffer?A. H4A, H3AOB. H3A, H2A2OC. H3A, H2AO D. H2A", HA 2ОЕ. НА2, А3

Answered: Image /qna-images/answer/6bfef232-9db7-400f-8013-c8397b915bb3.jpg

The titration curve of a weak acid, HnA has 3 inflection points at pH = 3.5, 6.7 and 10.3. If 0.1 M of a buffer, pH 4.2 is to be prepared %3D using the weak acid and its conjugate base, what will be the components of this buffer? OA HA, H3A O B. H3A, H2A2 OC. H3A, H2A O D. H2A, HA 2 O E. HA2, A3

The titration curve of a weak acid, HnA has 3 inflection points at pH = 3.5, 6.7 and 10.3. If 0.1 M of a buffer, pH 4.2 is to be prepared %3D using the weak acid and its conjugate base, what will be the components of this buffer? OA HA, H3A O B. H3A, H2A2 OC. H3A, H2A O D. H2A, HA 2 O E. HA2, A3

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: <, (C,H;CO,H) = 6.5 x 105). • What is the initial pH before any base is added? The first digit is a…

Q: A 230.0 −mL buffer solution initially contains 3.0×10−2 M of HCHO2 and 3.0×10−2 M of NaCHO2. Part A…

A: Given Volume of buffer = 230 mLConcentration of HCHO2 = 3.0 × 10-2 MConcentration of NaCHO2 = 3.0 ×…

Q: A buffer solution contains 0.347 M C6H5NH3 Br and 0.336 M C6H5NH2 (aniline). Determine the pH change…

A: Pkb = -log(kb) = - log(7.4×10-10 ) Pkb = 9.13

Q: A buffer solution is 0.40 M in acetic acid and 0.38 M sodium acetate (Ka=1.75X10°). Calculate the…

A: Given, Molarity of CH3COOH = 0.40 M Volume of buffer = 200.0 mL = 0.200 L Molarity of CH3COONa =…

Q: In a reaction 45.0 mL of 0.3M of HC2H3O2 is titrated with 0.2M KOH solution. Ka= 1.8x10^-5 1) what…

A: Answers are explained below.

Q: A buffer consisting of 0.36 M HA and O.321 H of the solution once the NaOH is absort for HA =67x 10…

Q: For a certain chemical process, the addition of an acid and a base to a buffer must keep the pH in…

A: Answer:- This question is answered by using the simple concept of buffer solution. For the best…

Q: A 0.500 L buffer solution is made with 0.4 M NH3 and 0.15 M NH4Cl with a pK, = 4.75. What is the…

Q: 40.0 mL of 0.20 M benzoic acid and 60.0 mL of 0.10 M sodium benzoate are combined in a large flask…

Q: Use the given molar solubilities in pure water to calculate K for each compound. a. MX; molar…

A: a) The solubility reaction of MX is MX ------> M+ + X- Given : molar solubility = 3.27 X 10-11…

Q: A buffer is prepared by mixing 16 mL 1M CH3COONa and 4 mL 1M CH3COOH pKa = 4.74. Calculate the pH of…

Q: Volume transferred, mL Solution Buffer a Buffer b 0.100 М СН,СООН 40.0 40.0 0.100 M NaOH 20.0 30.0…

A: We have to use henderson hasselbalch equation to calculate the pH of buffer. We need to calculate…

Q: A buffer can be prepared from a weak acid, HA, and it's conjugate base, A. A 1L solution is prepared…

A: Given : Volume of buffer solution = 1 L [HA] i.e concentration of weak acid HA = 0.2 M [A- ] i.e the…

Q: Calculating the composition of a buffer of a given pH A chemistry graduate student Is given 100. mL…

A: A buffer is a solution which maintains its pH even after addition of a small amount if acid or base.…

Q: A buffer is made up of 15.0 ml of 0.1 M HC,H,02 and 15.0 ml of 0.1 MNa CH,O, The solution is diluted…

Q: A chemistry graduate student is given 125. ml. of a 0.60M benzoic acid (HC,H,CO₂) solution. Benzoic…

A: Using Henderson hasselbalch equation we can figure out the moles of KC6H5CO2 required to reach…

Q: A buffer solution that is 0.458 M in HCN and 0.458 M in KCN has a pH of 9.40. The addition of 0.01…

A: The buffer solution consists of a weak acid (HCN) and the salt of weak acid and strong base (KCN).…

Q: A buffer is prepared by mixing 16 mL 1M CH3COONa and 4 mL 1M CH3COOH pKa = 4.74. Determine the pH…

A: Buffer capacity of buffer is a measure of magnitude of it`s resistance to change in the pH value on…

Q: 100.0 mL of the 1.0 M weak base solution is titrated with 2.0 M HCI. What volume of acid is required…

A: Given, Volume of the weak base = 100 mL Molarity of the weak base = 1.0 M Molarity of HCl = 2.0 M…

Q: which one has higher buffer capacity o.1 M C6 H8O7 , 0.01 M Na3C6 H5 O7 or 0.01M C6 H8O7, 0.01 0.01…

A: Buffer capacity refers to the amount of acid or base that the buffer can neutralize before the pH…

Q: Consider the titration of 50.0 mL of 0.319 M weak base B (Kb = 7.5 x 10⁻⁶) with 0.340 M HNO₃.…

Q: A chemistry graduate student is given 500. mL of a 1.10M acetic acid (HCH₂CO₂) solution. Acetic acid…

A: In the given question we know the concentration of acetic acid and Ka value, we need to find mass…

Q: What is the A-/HA ratio of these buffers at the given pH? NaF/HF pH = 4.00 (ii) CH3NH2/CH3NH3+Cl–…

A: The objective of this question is to calculate the ratio of the base (A-) to the acid (HA) in the…

Q: You want to make a 500.0 mL of 0.0500 M of phosphate buffer pH = 6.80 from solid Na2HPO4 compound…

A: The balanced chemical equation of formation of phosphate buffer can be shown as follows:

Q: Which of the following aqueous solutions are good buffer systems? . A 0.22 M perchloric acid + 0.18…

A: D. 0.12 M acetic acid + 0.12 M potassium acetate Buffer solutions can be made by mixing of aqueous…

Q: You want to make a 500.0 mL of 0.0500 M of phosphate buffer pH = 6.80 from solid Na,HPO, compound…

Q: Consider the titration of 30.0 mL of 0.255 M weak base B (Kb = 1.3 x 1010) with 0.150 M HI. a) What…

A: a.) We would write dissociation equation of base in water and use its Concentration and Kb values.…

Q: Enter your answer in the provided box. Find the pH of a buffer that consists of 0.83 M HBrO and 0.72…

Q: A buffer contains 0.175 moles C2H5NH3NO3 and 0.225 moles C2H5NH2 in 800.0 mL water. Kb (C2H5NH2) =…

A: The pOH of a basic buffer solution can be expressed as: pOH = pKb + logC2H5NH3NO3C2H5NH2pOH = pKb…

Q: 22. K, = 1.8 x 10s for acetic acid (HC2H3O2) Part 1. What molar ratio of acetic acid to sodium…

A: Part A. Formula of pH of buffer Solution of weak acid and its salt with strong base pH = pKa + log…

Q: A buffer is prepared by mixing 0.15 M NazHPO4 and 0.10 M NaH, PO4. K, for H3PO4 = 7.5 103 %3D Ka for…

A: The PH of buffer can be calculated as

Q: In the titration of Y(OH)3 with HX, which of the following equations should be used to calculate the…

Q: A 1.000L buffer is made of 0.7 M CH3COOH and 0.6 M CH3COONa.What is the pH of the buffer solution?…

A: The pH of the buffer solution can be determined as follows: pH = pKa + logSaltAcidpH = 4.74 +…

Q: 6. A buffer solution contains 0.1OM benzoic acid (C,H5COOH, Ka = 6.3 x 10) and 0.10M potassium…

A: pH can be calculated by using henderson equation pH = pka + log (salt/ acid) Pka = - log 6.3 x10-5…

Q: A chemistry graduate student is given 450. mL of a 0.70.M pyridine (C5H5N) solution. Pyridine is a…

Q: A buffer solution is formed by adding 0.200 moles of solid potassium nitrite, KNO₂, to 500.0 ml of…

A: A buffer is a solution which resist any change in pH on adding a small amount of acid or base . It…

Q: -10 What A chemistry graduate student is given 125. mL of a 1.70 M hydrocyanic acid (HCN) solution.…

A: when weak acid HCN ionises in water

Q: i. A 1.000L buffer is made of 0.7 M CH3COOH and 0.6 M CH3COONa .What is the pH of the buffer…

A: (i) We have volume of solution =1 L Molarity of CH3COOH=0.7 M⇒moles =0.7 mol/L ×1L=0.7 molMolarity…

Q: Be sure to answer all parts. A buffer consists of 0.17 M KHCO3 and 0.65 M K2CO3. Carbonic acid is a…

Q: Determine the pH change when 0.071 mol NaOH is added to 1.00 L of a buffer solution that is 0.346 M…

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

Q: 13. Which of the following buffer solutions has the highest buffer capacity? A. 0.10 M NH3 and 0.10…

A: An acidic solution contain more Hydronium ion than hydroxide ion while a basic solution have more…

Q: An acetate buffer is prepared with equal volumes of 0.10 M acetic acid and 0.10 M sodium acetate…

A: Given equal volumes of 0.10 M cetic acid and 0.10 M sodium acetate.The concentration of NaOH = 0.10…

Q: A buffer is made with 200.0 mL of 0.30 M propanoic acid (HC3H50₂) and 300.0 mL of 0.267 M NaC3H5O2.…

A: Buffer solution is the solution which have capacity to resist the change of its pH value even with…

Q: The pK, value for H2S is 7.00. What mole ratio of KHS to H2S is needed to prepare a buffer with a pH…

A: The henderson hasselbalch equation for weak acid, pH = pKa + log [conjugate base][acid]

Q: Consider a buffer made by adding 52.3 g of (CH3),NH2I to 250.0mL of 1.42 M (CH3)¿NH (Kb = 5.4 x…

A: The concentration or Molarity of salt is calculated by - M = w×1000/m×V Here, M = Molarity of Salt,…

Q: True or False: NaBr can never be the salt of a buffer. http://www.sciencegeek.net/tables/ka.shtml O…

A: As per bartleby guidelines I answered only first question so please don't mind.Thanks in advance.

Question

The titration curve of a weak acid, HnA has 3 inflection points at
pH = 3.5, 6.7 and 10.3. If 0.1 M of a buffer, pH 4.2 is to be prepared
using the weak acid and its conjugate base, what will be the
components of this buffer?
A. H4A, H3A
OB. H3A, H2A2
OC. H3A, H2A
O D. H2A", HA 2
ОЕ. НА2, А3

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

Similar questions

A 75.0 mL sample of 0.100M NH3 is titrated with 0.100 M HCI. What is the most likely pH of the resulting solution after the addition of 100.0 mL of HCl to the NH3? Kp, NH3 = 1.8x10-5 O the pH would be exactly 1 O the pH is = 7.545 O the pH = 5.277 O pH = 1.845
A buffer solution contains 0.442 M CH3NH3Cl and 0.294 M CH3NH₂ (methylamine). Determine the pH change when 0.062 mol NaOH is added to 1.00 L of the buffer. pH after addition - pH before addition = pH change = C Submit Answer 54 $ 998 R F F4 V % 5 [References] Use the References to access important values if needed for this question. Retry Entire Group 9 more group attempts remaining T Cengage Learning Cengage Technical Support G 6 B MacBook Air S Y H & 7 ◄◄ N F7 U J * 8 ►ll F8 I M -0 9 K ►► F9 O -0 L F10 P 4) F11 Previous + Next> = Save and Exit 4))) F12 ( delete
One of the most common buffers used in protein chemistry is a weak base called TRIS (the nitrogen atom of the amino group is the basic portion of the molecule): Но. -NH2 (HOCH2);CNH, = TRIS %3D A biochemist prepares a buffer solution by adding enough TRIS and 12 M HCI to give 1.0 L of a buffer solution that has concentrations [TRIS] = 0.39 M and [TRISH*] = 0.56 M. (pK, of TRIS is 5.91.) (a) Calculate the pH of the buffer solution. pH = i (b) Suppose that 3.3 mL of 12 M HCI is added to 12 L of the buffer solution; calculate the new pH of the solution. pH = i
A chemistry graduate student is given 500. mL of a 0.30 M benzoic acid (HC6H5CO2) solution. Benzoic acid is a weak acid with K= 6.3x 10-5 . What mass of NaC6H5CO2 should the student dissolve in the HC6H5CO2 solution to turn it into a buffer with pH = 4.25? You may assume that the volume of the solution doesn't change when the NaC6H5CO2 is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.
A buffer solution is prepared that is 0.28 M NH3 and 0.14 M NH4CI. What is the pH of this buffer? Kp for NH3 is 1.8x 10 OA8 95 B. 4,44 OC5.05 O D.9.26 0E. 9.56
Please don't provide handwritten solution ...
12 a b U Consider a buffer made by adding 132.8 g of NaC,H,O₂ to 300.0 mL of 1.83 M HC,H,O₂ (Ka = 6.3 x 10-5) X L L What is the pH of this buffer? What is the pH of the buffer after 0.750 mol of H+ have been added? What is the pH of the buffer after 0.250 mol of OH- have been added? >
A buffer solution contains 1.250 mol of phenol, C6H5OH, and 0.950 mol of sodium phenoxide, C6H5ONa, in 1.00 L of solution. Ka = 1.30 x 10-10. a. What is the pH of this buffer? b. What is the pH of this buffer after the addition of 0.525 mol of NaOH? (assume no volume change upon the addition of the NaOH) c. To the buffer produced in part a, what is the pH of the buffer after the addition of 0.225 mol of HCI? (assume no volume change up the addition of the HCI)
What is the least volume of 3.10 M HCl(aq) that will exceed the buffer capacity of 1.00 L of a buffer that is composed of 0.40 M acetic acid and 0.72 M sodium acetate?(Ka for acetic acid = 1.8 × 10−5.) a. 0.55 L b. 5.5 L c. 0.14 L d. 1.6 L e. 0.20 L
A buffer is prepared by mixing 25 mL of 0.10 M nitrous acid (HNO2) and 25 mL of 0.15 M sodium nitrite (NaNO2). The Ka for nitrous acid is 5.6 x 10-4. a.) What is the pH of the buffer solution? b.) What is the pH change when 5 mL of 0.10 M HCl is added to the solution?
A chemistry graduate student is given 250. mL of a 0.40M pyridine (C₂H₂N) solution. Pyridine is a weak base with K=1.7 x 10. What mass of C H₂NHBr should the student dissolve in the C,H-N solution to turn it into a buffer with pH =4.75? You may assume that the volume of the solution doesn't change when the C₂H₂NHBr is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.
A buffer solution is prepared in such a way that the concentration of propanoic acid is 3.9 x 10-1 power M and the concentration of sodium propanoate is 1.8 x 10 0 power M. The buffer equilibrium is described by C2H5cooH + H20 both arrows H3O+ c2h5COO- with Ka= 1.34 x 10 - 5 power . if the concentration of the sodium propanoate were double propanotate were doubled while the acide concentration remained the same, calculate the pH of the resulting solution pH = _______