you have found the pKa to be 10.3. “Acid-free” paper should have a pH between 8.7 and 10.2. What is the equilibrium concentration of carbonate in your buffer (in mM) if you add 0.635 mM calcium carbonate to pulp that started with 0.395 mM acid (pH=3.37)?

you have found the pKa to be 10.3. “Acid-free” paper should have a pH between 8.7 and 10.2. What is the equilibrium concentration of carbonate in your buffer (in mM) if you add 0.635 mM calcium carbonate to pulp that started with 0.395 mM acid (pH=3.37)?

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter17: Principles Of Chemical Reactivity: Other Aspects Of Aqueous Equilibria

Section17.2: Controlling Ph: Buffer Solutions

Problem 4RC: 4. To prepare a buffer containing CH3CO2H and NaCH3CO2 and having a pH of 5, the ratio of the...

See similar textbooks

Related questions

Q: A 25.00 mL sample of magnesium hydroxide solution is titrated with 0.00500 M HCl and 2 drops of…

Q: A student titrated 50.0mL of a 0.10 M solution of a certain weak acid with NaOH(aq), what is the…

A: Step 1: From the given graph, it is clear that pH range 6 to 10 is found at 25.0 mL of NaOH added.…

Q: Which one of the following indicators is best suited for titrating 0.05 M pyridine (pKb = 8.82) with…

Q: What masses of dinmethylamine and dimethylammonium chloride do you need to prepare 6.00 L of pH =…

Q: What is the pKa of a 0.2M solution of an unknown monoprotic acid that has a pH of 4.2?

A: We have find out Pka of solution of an unknown monoprotic acid that has a pH of 4.2

Q: What is the mole ratio of ammonia (with a pKb of 4.75) to ammonium chloride in a buffer with a pH of…

Q: 2- one liter of buffer solution contains 0.1 mole of benzoic acid and 0.2 mole of sodium benzoate…

A: Here we are required to find the Change in pH of the buffer solution

Q: Sulfate buffer? Your laboratory is out of materials to make phosphate buffer and you are…

A: A buffer solution is formed by the weak acid and its conjugate base or weak base and its conjugate…

Q: Prepare 1.0 L of 0.2 M citrate buffer, pH 5.3. Assume the availability of crystalline citric acid…

A: Concept based on the buffer solutions

Q: Starting with solid glycine-HCl and 0.75 M NaOH, how would you prepare 500 mL of 0.050 M glycine…

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

Q: What acid-base indicator should be used for the titration of 50.00mL of 0.0500 N HCl with 0.0500 N…

Q: 10.71

A: Molarity of HCl(M)= 0.050 M Volume of HCl(V) = 25 mL Mmol of HCl = M × V = 0.050 × 25 = 1.25…

Q: You have been asked to prepare 1 L of a 100 mM TRIPS (pKa 6.9) buffer. How much should you take of…

A: From the Henderson Hasselbalch equation pH = pKa + log [salt]/[acid] The base used to make TRIS…

Q: 4) How many grams of potassium azide (KN3, MM = 81.118 g/mol) are present in 250.0 mL of a pH 4.20…

A: Buffer is a solution which has a specific pH and resist a change in its pH when any acid or a base…

Q: A student titrates 0.590 g of the monoprotic weak acid potassium hydrogen phthalate (KHP) using…

A: The question is based on the concept of titrations. we are titrating a weak acid KHP with a strong…

Q: If 24.8 mL of 0.107 M acid with a pKa of 5.76 is titrated with 0.102 M NaOH solution, what is the pH…

A: pH = pKa + log [salt]/[acid] Number of moles = molarity x volume (L)

Q: A chemist is titrating a 32.5 mL sample of 2.00x10^-3 M benzoic acid with 8.00x10^-4 M Ca(OH)2. At…

A: Given that: Volume of benzoic acid = 32.5 mL Concentration of benzoic acid = 2.00 x 10-3 M…

Q: A biochemist prepares two stocks of sodium phosphate buffer by titrating phosphoric acid with sodium…

A: Given: pKa of phosphoric acid are 2.15, 7.20 and 12.35 Volume of 7.20 buffer is 50.0 mL Volume of…

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

Q: What is the pH of a buffer solution made with 0.789M benzoic acid with Ka = 6.5 x 10^-5 and 0.659M…

A: Ka = 6.5 × 10-5 So, pKa = - log (6.5 x 10-5) = 4.187 By using Henderson Hasselbalch eqn ,…

Q: Which acid-conjugate base system should you use to prepare a buffer with a pH of 9.0?…

A: pH = 9.0 According to Henderson hasselbach equation pH of buffer solution can be calculated as- pH…

Q: A mixture of 0.15 M acetic acid and 0.34 sodium acetate is given. Calculate the pH of the medium if…

A: The given data contains, Acetic acid = 0.15 M. Sodium acetate = 0.34 M. pKa of acetic acid = 4.87

Q: Prepare 1.0 L of a 0.1 M histidine buffer, pH 7.0, starting with histidine dihydrochloride…

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

Q: 5. Magnesium hydroxide (Mg(OH)2) has a pKsp value of 11.25. In a solution at pH 10, what is the…

A: Given, pKsp of Mg(OH)2 = 11.25 pH = 10 What is the maximum Mg2+ concentration in µmol/L = ? What…

Q: 4. ( You are performing the titration of a buffer with a pKa of 7.2. You start at the pka, and after…

A: A Buffer solution resist the change of pH,When small amount of acids ar base is added.

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

Q: A biochemist Deeds to preserve an enzyme in 0.50 M acetate buffer at pH 5.5.(Ka of acetic acid? 1.8…

A: Concept Based on Buffer solutions. Correct answer : option 'a' Calculation part is attached in step…

Q: A hypochlorous acid buffer is prepared with 0.10 moles HCIO and 0.10 moles CIO- and pH = pKa = 7.40.…

A: pH = pKa + log[salt]/[acid] ClO- + HCl -----> HClO + Cl- Number of moles of HClO formed =…

Q: Weak Acid Conjugate Base Ka pK. C20,2- HPO,2- HC204 6.4 x 10-5 4.19 H2PO, 6.2 x 10-8 7.21 HCO3 co,-…

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

Q: What is the ratio of the concentration of acetic acid and acetate ions required to prepare a buffer…

Q: The addition of 40.0 mL of HCl to 1000 mL of 0.5 M phosphate buffer changes the pH from 7.5 to 6.8.…

A: Given: The initial pH of the phosphate buffer = 7.5 Since 7.5 is closest to the pKa2 value of H3PO4,…

Q: In a lab, you titrate 27.0 mL of 0.100 M acetic acid (CH3COOH, a weak acid, pKa 5.756, Ka 2.75 x…

Q: You were given with 0.025 M acetic acid and 0.025 M NaOH. You were then instructed to prepare a 10.0…

Q: 6. If 25.1 mL of 0.109M acid with a pKa of 5.27 is titrated with 0.108 M NaOH solution, what is the…

A: The volume of acid V1=25.1 mL The concentration of acid C1=0.109 M The strength of an acid is pKa =…

Q: Which is the buffer region in the titration curve below? A 7 D mL of titrant Hd

A: A buffer is the solution of a weak acid and its conjugate base that resists any change in the pH…

Q: Calculate the change in pH when 5.8 mL of 1.6 M NaOH are added to 100. mL of buffer solution in…

Q: 125 mL of a 0.109 M phenylalanine (pKal = 1.83, pKa2 = 9.13) solution is titrated with 0.223 M NaOH.…

A: Since phenylalanine is a weak acid with pKa1 = 1.83 and pKa2 = 9.13 And since pKa1 >> pKa2…

Q: What is the appropriate acid-base indicator for the titration of 50.00 mL of 0.100 N NaOH with…

A: NaOH is a strong base and HCl is a strong acid. The titration will involve a sudden change from…

Q: Hi, I need help with this step-by-step please thank you .

Q: What mass of NH4Cl (Mw = 53.492 g mol-1) has to be dissolved in 750 mL of 0.25 M NH3 (pKa = 9.26) to…

A: 750 mL of 0.25 M NH3 pKa = 9.26 solution is mixed with a certain amount of NH4Cl to prepare a…

Q: alculate the change in pH that occurs when 0.5mmol of strong acid is added to 100ml of 0.05M lactic…

Q: Ja In titrating 10 ml of 0.1 N HA (pKa-4),the pH after the addition of 7 ml 0.IN 10.1N 3 NaOH is О…

A: Go through the solution provided

Q: pH VERSUS VOLUME TITRANT ADDED 14 12 |U 10- 8- 6- 4 RST 210- 0- 0.0 20.0 40.0 60.0 80.0 Volume NaOH…

A: From the given figure, it is clear that the amount of NaOH added at the equivalence point = 40 mL…

Q: 3 points (1): A buffer solution after the addition of 20.0 mL of 1.00 M NAOH solution to 500.0 ml of…

Q: Given with 0.025 M acetic acid and 0.025 M NaOH How will you prepare a 10 mL 0.02 M acetate buffer…

A: Here we have to prepare a 0.02 M acetate buffer solution of pH= 5.5 of volume 10ml from 0.025M…

Q: Which one of the following indicators is best suited for titrating 0.05 M methylamine (pK, = 3.19)…

A: Answer is explained below. In the given problem, there is a reaction between methylamine (weak base)…

Q: A buffer is made using 200.0 mL of 0.100 M (CH3)3N (trimethylamine) and 100.0 mL of 0.300 M…

A: The ratio of the mass of a substance to the molar mass of the substance is known as the moles of…

Q: Which of these compounds would be the best buffer at pH 5.0: formic acid (pKa = 3.8), acetic acid…

A: Given: The pH of the buffer solution = 5.0 The pKa of formic acid = 3.8 The pKa of acetic acid =…

Q: A 15.4 mL aliquot of hypochlorous acid that has a concentration of 0.16 M will be titrated with…

A: Given: The titration of hypochlorous acid with NaOH. And the titration is till 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

you have found the pK_a to be 10.3. “Acid-free” paper should have a pH between 8.7 and 10.2. What is the equilibrium concentration of carbonate in your buffer (in mM) if you add 0.635 mM calcium carbonate to pulp that started with 0.395 mM acid (pH=3.37)?

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

Calculations:

VIEW

Result:

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 steps with 7 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

Which of these buffers involving a weak acid HA has the greater resistance to change in pH? Explain your answer. (i) [HA] =0.100 M = [A] (ii) [HA] = 0.300 M = [A]
You are performing the titration of a buffer with a pKa of 7.3. You start at the pKa, and after 4mL of 1M HCl your buffer reaches pH 6.3. How many more mL of HCl should you need to go to pH 5.3? (4mL, more, or less than 4mL?) Clearly explain your answer
A student was told to make a pH=10.0 buffer from NH3 and NH4Cl. What concentration of NH3 and NH4Cl need to be used if the ionic strength needs to be 0.200. Ka of NH3 = 5.69 x 10-10 and pKa = 9.245
After a buffer solution of carbonic acid (with pKa of 3.75) was added with 1ml of sulfuric acid, the resulting pH of the carbonic acid buffer solution is 1.25. Do you think the carbonic buffer system still works effectively after the addition of the said acid?
What is the pH of a solution prepared by mixing 800 ml of 0.25 M formic acid and 200 ml of 0.25 M NaOH? (The pKa of formic acid/formate buffer is 3.75. Show how you arrived at your answer
A chemist needs a pH 3.5 buffer. Should she use NaOH with formic acid (Kₐ=1.8X10⁻⁴) or with acetic acid (Kₐ=1.8X10⁻⁵)? Why? What is the disadvantage of choosing the other acid? What is the role of the NaOH?
Explain qualitatively how you would prepare a buffer of phosphoric acid at a pH of 7. For phosphoric acid, pKa12.15, pKa27.20 and pKa3 12.15. Then, using Le Chatelier principle and the appropriate equilibrium, explain how the buffer will react to the addition of a small amount of base and a small amount of acid
You have been asked to prepare 1 L of a 100 mM TRIPS (pKa 6.9) buffer. How much should you take of the base and how much of the acid form to get a pH of 7.5? show your work
What is the pKa of a 0.2M solution of an unknown monoprotic acid that has a pH of 4.2?
In a titration, 25.00 mL of 0.1000 M triethyl amine ((CH3CH2)3N) is titrated with 0.0500 M hydrochloric acid (HCl). The following data was obtained: mL HCl added pH 0.00 11.86 25.00 10.71 50.00 6.79 What is pKa for the triethylammonium ion? 3.29 10.71 11.86 6.79
Your goal is to make a buffer with a pH of 4.75 from acetic acid and sodium acetate. Assume the pKa for acetic acid is 4.74. What is the volume of 1 M sodium acetate added to make your buffer? Report your answer to the tenths place. To do this, we use the Henderson-Hasselbach Equation pH = pkA + log (base/acid) where pkA = 4.74 for acetic acid, pH = target pH and [base] /[acid] = x/(1-x) since we don't know the concentration of the base, we will call it x the acid is just 1-x, assuming the two add up to 100% solve for x, and then you know the mL of base and acid to add.
A 100.00-mL sample of 0.2000M glycine, A+ form (see structure below), was titrated with 0.2000Mof NaOH. Ka1 of glycine = 3.16x10-3; Ka2 of glycine = 2.51x10-10 a) What is the pH after the addition of 100.00 mL of NaOH?(b) What is the pH after the addition of 180.00 mL of NaOH