3. Which acid is most suitable to use when preparing a buffer with pH = 7?Α. ΗΝΟ,(Ка — 4.5 х 104)С. НОСІ (Ка —3.5 х 10*)4.0х 10-10)В. СН,СООН (Ка — 1.8 х 105)D. HCN (Kа%3D%3D

The buffer solution is the Solution which resist the change in pH when a small amount of acid or…

3. Which acid is most suitable to use when preparing a buffer with pH = 7? A. ΗΝΟ В. СН,СООН (Ка (Ка — 4.5 х 10-) 1.8 x 105) С. НОСІ (Ка — 3.5 х 10*) D. HCN (Ka 3 4.0 х 10-10)

3. Which acid is most suitable to use when preparing a buffer with pH = 7? A. ΗΝΟ В. СН,СООН (Ка (Ка — 4.5 х 10-) 1.8 x 105) С. НОСІ (Ка — 3.5 х 10*) D. HCN (Ka 3 4.0 х 10-10)

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

Publisher:Seager

Chapter9: Acids, Bases, And Salts

Section: Chapter Questions

Problem 9.117E

See similar textbooks

Related questions

Q: Calculate the pH of the above buffer after 10.00 mL of 1.000 M NaOH (0.01000 mol OH-1) was added to…

A: Here we are required to find the pH of the buffer solution after addition of 10 ml of 1M NaOH.

Q: What volume of 0.50 M HNO3 should be added to 200. mL of 0.20 M NH3 in order to create a buffer with…

Q: given 250. ml. of a 0.80 M diethylamine (C2H5)2NH2Br solution. Diethylamine-3 is a weak base with K,…

A: Given, Volume of Base = 250. ml = 0.250 L Concentration of Base = 0.80 M Mole of Base =0.80 ×…

Q: Please explain your reasoning, thank you! 75.0 mL of 1.35 M base, B, is titrated with 1.25 M…

A: IMPORTANT POINTS Neutralization reaction occurs Law of equivalence is applied. Millimoles of both…

Q: HCN] ka=4.0x10^-10 pka=10.32 An aqueous solution contains 0.447 M hydrocyanic acid. How many mL…

Q: Determine the pH at one-half of the equivalence point. Express your answer to two decimal places.…

A: The pH at the half of the equivalence point, at the equivalence point and the after adding 6.0 mL of…

Q: 3) i) A 25.0mL sample of a 30.0% HF solution has a density of 1.101g/mL. The sample is diluted to a…

A: (i) Given, Initial volume of the solution is 25.0 mL. Final volume of the solution is 500 mL.…

Q: 1. 10.0 mL of 0.40 M weak acid is being neutralized with 0.10 M NAOH. The results of this titration…

A: a. For the titration of a weak acid with a strong base, the pH at the equivalence point is greater…

Q: You need to make 800 mL of a 20x Laemmli-PAGE buffer whose working concentration (or 1x…

A: Molarity = given massmolar mass× 1volume in litres 1% solution = 1 g solute in 100 mL solution 52…

Q: A chemist needs a pH 3.5 buffer. Should she use NaOH with formic acid (Kₐ=1.8X10⁻⁴) or with…

Q: Calculate the pH during the titration with NaOH after addition of: a. 50 mL of 0.1 mol L-1 NaOH to…

A: Solution: We know that acid-base titration method is most used traditional method to calculate…

Q: Which of the following mixtures is not a buffer solution? A) 25.0 mL of 0.10 M ammonia plus 20.0…

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

Q: a) Calculate the pH of a buffer prepared by dissolving 8.00 g of HC7H5O2 and 10.0 g NaC7H5O2 in…

A: (a)Molarity of HC7H5O2 and NaC7H5O2 is determined as follows,Total volume of solution is 500 mL =…

Q: A solution was composed of 50.0 mL of 0.1 M C6H8O6and50.0 mL0.100M NaC6H7O6. a. Would this solution…

A: Given: The volume of C6H8O6 in the solution = 50.0 mL The concentration of C6H8O6 in the solution =…

Q: What volumes of stock 0.500 M sodium propanoate and 0.500 M propanoic acid (pKa 4.88) are needed to…

Q: A buffer is prepared by combining 17.6 g of H2CO3 (carbonic acid) with 220 mL of 0.18 M NAOH and…

Q: A chemistry graduate student Is glven 100. mL of a 0.70M trimethylamine ((CH,) N solution.…

Q: What is the pH at the second equivalence point in the titration of 541 mL of 0.501M carbonic acid…

A: At second equivalence point, H2CO3 reacts completely with NaOH to form Na2CO3 and the net reaction…

Q: What olume of 17.1 M glacial acetic acid (HC2H3O2) must be added to 100.0 mL of 1.25 M KOH to form a…

A: Given, Molarity of glacial acetic acid=1.71M Volume of KOH=100mL Molarity of KOH=1.25M pH of…

Q: The pKa of lactic acid is 3.86. You have a mixture of lactic acid and sodium lactate, where the…

Q: Prepare 100 mLof a 0.01 M phosphate buffer, pH 7.70, from stock solutions of 0.1 M K2HPO4and 0.2 M…

A: The buffer to be produced is from K2HPO4 and KH2PO4. Here, K2HPO4 acts as conjugate base and…

Q: To prepare a 1.00 L of a buffer with a pH of 6.34 from 0.4 M Na3AsO4 ( A^3- ) and 0.3M HCl, the…

A: The reaction between Na2HAsO4 and HCl is shown below. Na2HAsO4+HCl→NaH2AsO4+NaCl Note: Only the…

Q: Preparation of 40 mL of an acetate buffer (pH 4.2) 0.2 M acetic acid (pKa = 4.8) and 0.2 M sodium…

A: pH is used to get the acidic or alkaline values of a solution. A buffer solution is one which…

Q: a) How many grams of sodium acetate, NACH3COO (molar mass: 82.0343 g/mol) should be combined with…

A: The answer to the following question is-

Q: What is the H30* | and the pH of a benzoic acid-benzoate buffer that consists of 0.15 M C6H5COOH and…

A: Given, [C6H5COOH] = 0.15M [C6H5COONa] = 0.38M

Q: What volume of 0.50 M HNO3 should be added to 200. mL of 0.25 M NH3 in order to create a buffer with…

Q: What is the pH of a 500 mL buffer containing 0.200 moles NH3 and 0.350 moles NH4CI? Kb = 1.8 x 10-5…

A: Buffer solution: The solution that resists the change in pH is known as a buffer solution. The…

Q: Calculate the pH of a solution that is 0.20 M HOC1 and 0.92 M KOCI. Ka = 3.5x10-8 pH = 8.16 b In…

Q: A titration of 65.0 mL of a sulfuric acid (H,SO) solution of unknown concentration with a…

A: Consider the given information is as follows; Volume of H2SO4 = VH2SO4 = 65.0 mL Concentration of…

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: You need to prepare 100.0 mL of a pli 4.00 buffer solution using (0.100 M henzoic acid (pk, = 4.20)…

Q: Imidazole (C3H4N2, MW = 68.07816, Kb = 9.80 x 10–8) can be used to create buffers at physiological…

A: Buffer are solution which resist change in PH when acid Or base are added

Q: Phosphoric acid is a triprotic acid (Kal = 6.9 × 10-3, K2 = 6.2 x 10-8, and Ka3 = 4.8 x 10-13). To…

Q: 3.) A 15.00 mL sample of 0.250M formic acid (HCOOH, Ka - 1.8 x 104) is titrated with 0.300 M sodium…

A: Given, Molarity of HCOOH = 0.250 M Volume of HCOOH = 15.00 mL = 0.015 L Acid dissociation…

Q: Acetic acid’s pKa is 4.75 and nitrous acid’s pKa is 3.16. If you made one buffer of equal parts…

A: Given: pKa of acetic acid = 4.75 pKa of nitrous acid = 3.16 And both the buffers have an equal…

Q: enty-five mL of 0.100 M lactic acid (K, = 1.4 x 10*) is titrated with 0.097 M KOH. a) What is the pH…

A: Soln

Q: 10- Which of the following can be classified as buffer solutions? a. 0.25 M HBr + 0.25 M HOB1 b.…

A: A buffer is a solution that contains a mixture of a weak acid and its conjugate base, or a weak base…

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: 1- Calculate the pH of 0.1 M KHCO3.

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

Q: You make a 200mM potassium phosphate buffer (pKa of 7.20) with monobasic potassium phosphate…

A: Given: Concentration of solutes = 200 mM = 0.200 M (Since 1 M = 1000…

Q: You need to prepare 100.0 mL of a pH 4.00 buffer solution using 0.100 M benzoic acid (pK, = 4.20)…

A: Given, Volume of the buffer solution = 100.0 mL pH = 4.00 [Benzoic acid] = 0.100 M [Sodium…

Q: Zane titrated 25.0 mL of 0.40 M propioic acid with 0.20 M NaOH. What volume of NaOH is needed to…

A: we have to calculate the volume of NaOH for equivalence point

Q: What is the pH of a 500 mL buffer containing 0.200 moles NH3 and 0.350 moles NH4CI? Kb = 1.8 x 10-5…

A: The given Kb value is, Kb=1.8 x 10-5 pKb=-log Kb =4.744 pKa=14-pKb =14-4.744…

Q: A buffer is created by mixing 600 mL solution of acid HA (0.500 M) with 700 mL of conjugate base A-…

Q: Q 1(h) Which buffer system will have the greatest buffer capacity at pH 5.5? Acetic acid/sodium…

A: h) Buffer capacity is more when it's pKa is nearer to its pH. pH = -log(H+) and pKa= - log (Ka)…

Q: = H+ + HPO;- Ka = 6.2 x 10-8 = H+ + SO?- Ka = 1.3 x 10-2 From the systems above, identify the…

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

Q: Topic: Equilibrium constants of weak acids and basis along with their applications in buffers.…

A: Buffers are substances which resist the change in pH values. Our blood is good example of buffer.…

Q: Phosphoric acid is a triprotic acid (Ka1 = 6.9 x 10-3, K2 = 6.2 × 10-8, and K,3 = 4.8 × 10-13). To…

Q: Choose the buffer with the greatest buffering capacity: d. 0.25M formic acid/formate buffer at…

A: We are given three different types of buffer solution at different pH and concentrations and we have…

Q: What mass of sodium benzoate, C6H5COONa should you add to 150 mL of a 0.15 M benzoic acid solution…

A: Introduction: Molarity of benzoic acid = 0.15 M Volume of benzoic acid = 150 ml pH = 4.25 Ka =…

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

3. Which acid is most suitable to use when preparing a buffer with pH = 7?
Α. ΗΝΟ,
(Ка — 4.5 х 104)
С. НОСІ (Ка —
3.5 х 10*)
4.0х 10-10)
В. СН,СООН (Ка — 1.8 х 105)
D. HCN (Kа
%3D
%3D

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

Introduction

VIEW

Calculation

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 1 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

Repeat the procedure in Exercise 61, but for the titration of 25.0 mL of 0.100 M pyridine with 0.100 M hydrochloric acid (Kb for pyridine is 1.7 109). Do not calculate the points at 24.9 and 25.1 mL.
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
Imidazole (C3H4N2, MW = 68.07816, Kb = 9.80 x 10–8) can be used to create buffers at physiological pH’s. How many grams of imidazole and how many milliliters of 6.00 M HCl would be required to make 500.0 mL of 0.1000 M imidazole buffer with a pH of 7.20?
An employer is interviewing 4 applicants for a job as a laboratory technician and askseach of them how to prepare a buffer solution with a pH close to 11.000.Use these ka’s to help you: Show your workPropionic Acid, CH3CH2COOH, ka = 1.34 x 10-5 Ethanamine, CH3CH2NH2, kb = 6.3 x 10-4 Jung says he would mix CH3CH2COOH & CH4CH3COOHDominique says she would mix CH3CH2 NH2 & CH3CH2COOHJoshua says he would mix CH3CH2COOH & CH3COONaKyla says she would mix CH3CH2NH2 & CH3CH2NH3BrWho would you hire based on their ability to make a buffer?_________________________
What will be the appropriate pH of a buffer prepared by mixing 100 ml of 0.1 M Na2HPO4 and 100 ml of 0.1 M NaH2PO4? (For H3PO4, pKa1 = 2.1; pKa2 = 6.8; pKa3 = 12.5) Ans in 2 significant figures
Tris(hydroxymethyl)aminomethane [(HOCH2)3CNH2—Tris, or THAM] is a weak base frequently used to prepare buffers in biochemistry. Its Kb is 1.2 × 10−6 and pKb is 5.92. The corresponding pKa is 8.08, which is near the pH of the physiological buffers, and so it exhibits good buffering capacity at physiological pH. What weight of THAM must be taken with 100 mL of 0.50 M HCl to prepare 1 L of a pH 7.40 buffer?
A. What two compounds would be best to use in preparing a pH 9.0 buffer solution? justify your answer. Assume you have the acids and the sodium salts of their conjugate bases available to you. Answer: The two compounds best fo preparing a buffer solution with a pH of 9.0 would be hydrocyanic (HCN) and phenol (HOc6H5) because their pKa values are 9.40 and 9.80 respectively making their pH levels the closest to 9. B. WHat mass ration of sodium to acid is needed to prepare this buffer? C. Can this buffer solution better resist pH changes from a string acid addition or strong base addition?
Consider how best to prepare one liter of a buffer solution with pH = 3.79 using one of the weak acid/conjugate base systems shown here. Weak Acid Conjugate Base Ka pKa HC2O4- C2O42- 6.4 x 10-5 4.19 H2PO4- HPO42- 6.2 x 10-8 7.21 HCO3- CO32- 4.8 x 10-11 10.32 How many grams of the sodium salt of the weak acid must be combined with how many grams of the sodium salt of its conjugate base, to produce 1.00 L of a buffer that is 1.00 M in the weak base?grams sodium salt of weak acid = grams sodium salt of conjugate base =
Give good solution Asap Buffer A: CH3COOH 40.0 mL; NaOH 20.0 mL; H2O 20 mL Buffer B: CH3COOH 40.0 mL; NaOH 30.0 mL; H2O 10 mL Please identify how the buffer capacity of Buffer A and Buffer B change if the volume of water added was doubled. And does the the buffer capacity increase, decrease, or remain the same. Pleas explain why in detail?
How many grams of Na2CO3 (FM 105.99) should be mixed with 1.70 g of NaHCO3 (FM 84.01) to produce 100 mL of buffer with pH 10.00? For carbonic acid, H2CO3 . Report the answer to the correct number of significant figures
Describe, stepwise, how you would prepare 0.8 L of a 0.25 M phosphate buffer, pH 12.5, using K3PO4·H2O (f.w. = 230.28) and K2HPO4 (f.w. = 174.18). H3PO4 ⇌ H2PO4- + H+ pKa1 = 2.12 H2PO4- ⇌ HPO4-2 + H+ pKa2 = 6.8
Suppose you are given solutions of 1.00 M acetic acid and 1.00 M sodium acetate and are asked to make 100.00 mL of buffer at pH 5.00 using only these two solutions. What volume, in milliliters, of acid would you need? The pKa of acetic acid is 4.75.