Which of the following equations are predominant incalculations of pH for the buffer solution of NaH2PO4?I. H3PO4 + H20 2 H30* + H2PO4II. H2PO4 + H20 2 H30* + HPO,2-II. HPO,2 + H20 H30* + PO43-Select one:O a. Only IIO b. I and IIO c. I, Il and IIO d. Il and IIIO e. I and III

Answered: Image /qna-images/answer/80462413-7613-4351-9795-04626c6fb6ad.jpg

Which of the following equations are predominant in calculations of pH for the buffer solution of NaH,PO4? I. H3PO4 + H20 2 H30* + H2PO4 II. H2PO4 + H202 H30* + HPO,2 II. HPO,2 + H20 2 H30* + PO,3- Select one: a. Only II O b. I and II O c. I, Il and II d. Il and III O e. I and III

Which of the following equations are predominant in calculations of pH for the buffer solution of NaH,PO4? I. H3PO4 + H20 2 H30* + H2PO4 II. H2PO4 + H202 H30* + HPO,2 II. HPO,2 + H20 2 H30* + PO,3- Select one: a. Only II O b. I and II O c. I, Il and II d. Il and III O e. I and III

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter10: Potentiometry And Redox Titrations

Section: Chapter Questions

Problem 7P

See similar textbooks

Related questions

Q: 1. Which of the following would be effective buffers. (circle effective buffers) HCN/NACN desired…

Q: 2. A0.2001g sample of Na2CO3 required 25.10ml of x's HCI to reach endpoint. The x's HCl was titrated…

A: Molarity can be defined as the concentration of a substance in 1 L of the solution. The mathematical…

Q: back titration done for this analysis?

A: Ans. D. NH3 is a weak base and large amount of titrant is needed to reach equivalence point.…

Q: a). Which is the more effective buffer? 0.35 M NaH2PO4/0.15 M H3PO4 0.35 M NaH2PO4/0.20 M H3PO4…

A: Hi! Thank you for the question, As per the honor code, we are allowed to answer one question at a…

Q: Question 7b Ph at The midpoint of the titration. My answer is not matching the study guide answer…

A: If any solution/liquid is able of holding the pH when any basic or acidic solution is further mixed…

Q: Calculate the pH at 25°C of 291.0 mL of a buffer solution that is 0.310 M NH4Cl and 0.310 M NH3…

A: Buffer solution : It is a special type mixture of weak acid or base and its conjugate salt. The…

Q: ich of the following 1:1 mixtures would be best suited to form a buffer closest to a pH of 3.70? A)…

A: According to the Henderson-Hasselbalch’s equation, the pH range lies in between pKa±1. So, the…

Q: Which of the following equations are predominant in calculations of pH for the buffer solution of…

A: The Henderson-Hasselbalch equation can be given as follows: where C.B: Conjugate Base A: Acid or…

Q: Ammonia is a convenient buffer system in the slightly basic range. (a) What is the pH of a buffer…

Q: Calculate the pH at 25°C of 183.0 mL of a buffer solution that is 0.230 M NH4Cl and 0.230 M NH3…

A: The Henderson Hasselbalch equation for basic buffer is given as :

Q: Which of the following would be effective buffers. (circle effective buffers) HCN/NaCN desired…

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

Q: fect of concentration of buffer H2PO4- + H2O ======== HPO4^-2 + H3O+ CASE1. Using 0.1 M phosphate…

A: Since you have posted a question with multiple sub-parts, we will solve first three subparts for…

Q: 20.0 mL of the 0.50 M LiOH are added to 25.0 mL of 0.40 M H2SO4. What is the pH at this point in the…

Q: Consider Titration of 50 mL of 0.20M H3A (Ka1= 8.2×10^-4 , Ka2= 2.9×10^-8 Ka3= 3.7×10^-11) titrated…

A: When a strong acid reacts with a strong base, then salt formation will happen and the reaction will…

Q: Create a schematic diagram on how to prepare a Phosphate Buffer NaH2PO4 - K2HPO4 with a final volume…

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

Q: A) 2.0 mL of 85% (w/w) concentrated H3PO4 (density 1.73 g/cm3) is diluted to 500 mL with water. What…

Q: A 15.00 mL sample of 0.355 M H3PO4 (Ka,1 7.52 x 10-3, Ka,2 6.23 x 10-8, Ka,3 2.1 x 10-13) is…

A: (a) For first equivalent point: H3PO4 + NaOH ----->…

Q: 2. A 25.00mL sample of 0.360M NAOH is being titrated with 0.425M HNO3. a.) What is the pH of the…

A: pOH= -log[OH-] pOH+ pH= 14

Q: -4 A chemistry graduate student is given 100. mL of a 1.50M trimethylamine (CH,),N)s solution.…

Q: Describe, stepwise, how you would prepare 0.8 L of a 0.25 M phosphate buffer, pH 12.5, using…

A: The question is based on the concept of buffer solution. A buffer is a solution which resist any…

Q: chemist needs to prepare a buffer solution with ph = 10.00 and has both Na2CO3 and NaHCO3 in pure…

Q: 12. What volume (in mL) of a 0.150 M Na2SO3 solution must be added to 20.0 mL of a 0.120 M NaHSO3…

Q: 1.00 L of an aqueous solution containing 0.1026M of compound B and 0.0296M of its conjugate acid HB*…

A: For buffer solution change in pH can be predicted by Henderson–Hasselbalch equation. pH = pKa +…

Q: 0.50 M solutions of each weak acid in the table are available. Choose an acid solution and determine…

A: Henderson Hasselbalch equation shows relation between pH and pKa. So, we will solve the above…

Q: Suppose you have an aqueous solution prepared by dissolving 0.051 mol of NaH2PO4 in 1 L of water…

Q: Titration of (4.77300x10^-1) grams of monoprotic weak acid (dissolved in KCl) required…

A: Given: Mass of weak acid = 4.77300x10-1 gram Concentration of NaOH = 1.965 x 10-1 M Volume of NaOH…

Q: For each, specify B for buffer on N for not a buffer. Then specify whether the solution is acidic,…

Q: Don’t ever mix acid with cyanide (CN) because it liberates poisonous HCN(g). But, just for fun,…

A: (a)

Q: B)

A: The milliliters of NaOH are needed to reach the equivalence point is to be calculated. The…

Q: 8. If a buffer solution is best made by selecting an acid that has a pKa value within 1.00 unit of…

Q: Calculate the pH of a buffered solution that is prepared by dissolving 0.3mol of NaHCO3and 0.45mol…

A: Since you have posted multiple questions, we are entitled to answer the first only.

Q: What volumes of 0.50 M HNO2 and 0.50 M NaNO2 must be mixed to prepare 1.00 L of a solution buffered…

Q: A) How many grams of Sodium fluoride (NaF) should be added to 612 ml solution of 0.4 M Hydrofluoric…

Q: Iminodiacetic acid (IDA) is often used in ion exchange resins as a way to remove heavy metals from…

A: Solution - ɑA2- = 4.6 × 10-3 Kf =[Ni A22-] /[Ni 2+][ɑ A2-]2 C 2IDAA [Ni A22-] /[Ni 2+] C 2IDAA =…

Q: aching and le + ment/kCovalentAchivity.do?koatorassiqnmeent-take [Review Topics) [References) Use…

Q: Consider a 1.00 L solution which is 0.010 M CH3CO2H and 0.10 M NaCH3CO2. Ka = 1.8*10-5 a. What is…

A: This question can be solved using henderson-hesselbech equation.

Q: a. Calculate the number of moles of HCI(g) that must be added to 1.0 L of 1.1 M NaC,H3O2 to produce…

Q: An aqueous buffer solution of volume 100 cm3 consists of 0.20 M CH3COOH and 0.20 M NaCH3CO2.…

A: a) Calculation of pH of the solution: Thus pH of the solution in 3 significant figures is 4.75

Q: If the buffer prepared by mixing 0.30 M C2H5NH;HCI(aq) with 0.50 M C3H;NH2 in the previous question…

Q: Calculate the pH of a buffered solution that is prepared by dissolving 0.3mol of NaHCO3 and 0.45mol…

A: Since you have posted multiple questions, we are entitled to answer the first only.

Q: Calculate the pH of the above buffer after 10.00 mL of 1.000 M NaOH (0.01000 mol OH1) was added to…

Q: a) Calculate the pH of a buffer system made up of 0.25 M C6H5COOH and 0.35 M C6H5C00ONA. b)What is…

Q: A buffer solution is made from 135 mL of 0.395 M in HC2H3O2 and 115 mL 0.345 M NaC2H3O2 (the Ka of…

Q: pH

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

Q: A buffer solution is 0.366 M in HF and 0.372 M in KF . If Ka for HF is 7.2×10-4 , what is the pH of…

A: In above question acidic buffer is formed so pH of solution of directly determined using formula :…

Q: buffer solution is prepared by dissolving 1 mol of lactic acid C3H6O3, with Ka = 1.4 × 10-⁴ and 1…

A: We have to find pH of solution

Q: Which solution below would have the greatest buffering capacity? The solution was prepared from a…

A: Given, buffer solutions are: 0.197 M HOC2H4NH2 and 0.197 M HOC2H4NH3Cl, Kb = 3.20e-5 0.0966 M NH2OH…

Q: 5. a. Suppose a solution contains 0.50 M NaH2PO4 and 0.80 M N22HPO4. What pH should be expected for…

A: The concentration of a solution can be defined in terms of molarity as the ratio of the amount of…

Q: 4. Formic acid, HFor, has a K, value of 1.8 x 10-4. You need to prepare 100 mL of a buffer hay- ing…

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

Q: Ka for HPO42- = 4.4 x 10-13. A buffer system of 1.00 mole of Na2HPO4 and 1.00 mole of Na3PO4 to…

A: The weak acid component of the buffer is Na2HPO4 or HPO42-(aq). The conjugate base component of the…

Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

Which of the following equations are predominant in
calculations of pH for the buffer solution of NaH2PO4?
I. H3PO4 + H20 2 H30* + H2PO4
II. H2PO4 + H20 2 H30* + HPO,2-
II. HPO,2 + H20 H30* + PO43-
Select one:
O a. Only II
O b. I and II
O c. I, Il and II
O d. Il and III
O e. I and III

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

A 0.3012g sample of an unknown monoprotic acid requires 24.13mL of 0.0944MNaOH for neutralization to a phenolphthalein end point. There are 0.32mL of 0.0997MHCl used for back titration. a. How many moles of OH are used? How many moles of H+ from HCl? _______moles OH ________moles H+ b. How many moles of H+ are there in the solid acid? Use Eq.5. ____________ moles H+ in solid c. What is the molar mass of the unknown acid? Use Eq.4. ____________ g/mol
Fifty cm3 of 1.000 M nitrous acid is titrated with 0.850 M NaOH. What is the pH of the solution (a) before any NaOH is added? (b) at half-neutralization? (c) at the equivalence point? (d) when 0.10 mL less than the volume of NaOH to reach the equivalence point is added? (e) when 0.10 mL more than the volume of NaOH to reach the equivalence point is added? (f) Use your data to construct a plot similar to that shown in Figure 14.10 (pH versus volume NaOH added).
Malonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid w ith NaOH, stoichiometric points occur at pH = 3.9 and 8.8. A 25.00-mL sample of malonic acid of unknown concentration is titrated with 0.0984 M NaOH, requiring 31.50 mL of the NaOH solution to reach the phenolphthalein end point. Calculate the concentration of the initial malonic acid solution. (Sec Exercise 113.)
A good buffer generally contains relatively equal concentrations of weak acid and conjugate base. If you wanted to buffer a solution at pH = 4.00 or pH = 10.00, how would you decide which weak acidconjugate base or weak baseconjugate acid pair to use? The second characteristic of a good buffer is good buffering capacity. What is the capacity of a buffer? How do the following buffers differ in capacity? How do they differ in pH? 0.01 M acetic acid/0.01 M sodium acetate 0.1 M acetic acid/0.1 M sodium acetate 1.0 M acetic acid/1.0 M sodium acetate
A 1.0-LL buffer solution contains 0.100 molHC2H3O2molHC2H3O2 and 0.100 molNaC2H3O2molNaC2H3O2. The value of KaKa for HC2H3O2HC2H3O2 is 1.8×10−51.8×10−5. Calculate the pHpH of the solution upon addition of 21.4 mLmL of 1.00 MHClMHCl to the original buffer. Express your answer using two decimal places.
40.00mL of a 0.100M benzoic acid (Bz) solution are mixed with 20.00mL of 0.100M sodium hydroxide solution. What is the pH of the resulting solution if the Ka of benzoic acid 6.5 x10 -5 and the pKa = 4.19? (Use the Henderson Hasselbach Equation with mmol). Reaction: HOBz + OH- ---> H2O + OBz-
To create a buffer solution, 40.00mL of a 0.100M benzoic acid (Bz) solution are mixed with 20.00mL of 0.100M sodium hydroxide solution. What is the pH of the resulting solution if the Ka of benzoic acid 6.5 x10 -5 and the pKa = 4.19? (Use the Henderson Hasselbach Equation with mmol). Reaction: HOBz + OH- ---> H2O + OBz- From the buffer solution above, youo take a 10.00mL portion of the buffer. Using all of the information provided, how much conjugate acid and conjugate base are in the 10.00mL portion that you took out? Group of answer choices 0.167mmol 0.500mmol 0.222mmol 0.333mmol
A buffer was made by mixing 0.1404 moles of HN3 with 0.1025 moles of KN3 and diluting to exactly 1 liter. What will be the pH after addition of 10.00 mL of 0.2367 M HBr to 50.00 mL of the buffer? Ka(HN3) = 1.900e-5. Note: only a portion of the original buffer is used in the second part of the problem.
Calculate the pH of 1.00 L of 0.195 M HC2H3O2 /0.125 M C2H3O2 - buffer system after the addition of 10.20 mL of 1.00 M HCl. [HC2H3O2: Ka = 1.8 x 10-5 ) (b) Compare the new pH with what you calculated from problem 1. Is the HC2H3O2 /C2H3O2 - mixture effective as a buffer? Explain. (c). Which buffer system is the best choice to create a buffer with pH = 7.20? Explain your choice. (HC2H3O2 Ka = 1.8 x 10-5 ; NH4 + Ka = 5.6 x 10-10; HClO2 Ka = 1.1 x 10-2 ; HClO Ka = 2.9 x 10-8 ) HC2H3O2/KC2H3O2 NH3/NH4Cl HClO2/KClO2 HClO/KClO. Solution part a,b,c properly fast
0 / 6 ptsWhich of the following buffer systems is best for a buffer with [OH–] equal to 1.00 × 10–7 M? Acidity constants for the weak acid in each buffer are given below. CH3CO2H/CH3CO2– (pKa 4.74) H2PO4–/HPO42– (pKa 7.20) CH2ClCO2H/CH2ClCO2– (pKa 2.86) HCO2H/HCO2– (pKa 3.75) All of these buffer systems will work equally well. HCO3–/CO32– (pKa 10.2)
a) At temperature 25°C, 0.02 M hydrazine, N2H4 solution is 0.69% ionised. Calculate the i. Concentration of OH- ion ii. ionisation constant, Kb b) Calculate the mass of sodium benzoate, C6H5COONa that should be added to 500 mL of 0.2M aqueous benzoic acid, C6H5COOH solution to produce a buffer with pH 3.50?[ Ka for C6H5COOH = 6.3 x10-5] c) When a 1 x 10-3 moldm-3 solution of CaCl2 is mixed with an equal volume of a 1 x 10-3 moldm-3 solution of Na2SO4, will precipitate form? (Ksp CaSO4= 2 x 10-5) Do you mean that pH? That was all the given information the question gave.. I don't understand how to use the ionised part the most
You will be handling cells that are viable at pH 5.5. Which of the following buffer systems should you use for these cells? Explain your answer. A. CH3COOH - CH3COO- , Ka of CH3COOH = 1.8x10^(-5) B. NH3 - NH4+ , Kb of NH3 = 1.8x10^(-5) C. HONH2, HONH3+ , Kb of HONH2 = 9.1x10^(-9) D. C5H5N, C5H5NH+ , Kb of C5H5N = 1.5x10^(-9)

SEE MORE QUESTIONS

Recommended textbooks for you

Appl Of Ms Excel In Analytical Chemistry

Chemistry

ISBN:

9781285686691

Author:

Crouch

Publisher:

Cengage

Chemical Principles in the Laboratory

Chemistry

ISBN:

9781305264434

Author:

Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Publisher:

Brooks Cole

Chemistry: An Atoms First Approach

Chemistry

ISBN:

9781305079243

Author:

Steven S. Zumdahl, Susan A. Zumdahl

Publisher:

Cengage Learning

Chemistry

ISBN:

9781133611097

Author:

Steven S. Zumdahl

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

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

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Appl Of Ms Excel In Analytical Chemistry

Chemistry

ISBN:

9781285686691

Author:

Crouch

Publisher:

Cengage

Chemical Principles in the Laboratory

Chemistry

ISBN:

9781305264434

Author:

Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Publisher:

Brooks Cole

Chemistry: An Atoms First Approach

Chemistry

ISBN:

9781305079243

Author:

Steven S. Zumdahl, Susan A. Zumdahl

Publisher:

Cengage Learning

Chemistry

ISBN:

9781133611097

Author:

Steven S. Zumdahl

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

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

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS