Answered: Show by 2 net ionic equations how…

Science

Chemistry

Show by 2 net ionic equations how NaHCO3 may act as a buffer.

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: Calculate pH of a weak base/conjugate acid buffer solution. A 0.186-M aqueous solution of C6H5NH2…

A: For 0.186 M C6H5NH2pH = 9.07pOH = 14 - 9.07 = 4.93-log (OH-) = 4.93[OH-] = 10-4.93 = 1.17 × 10-5…

Q: An analytical chemist is titrating 243.2 mL of a 0.3300M solution of diethylamine ((C,H,), NH) with…

Q: Complete the following schemes by assigning the missing products or reagents. KOC(CH3)3 Br2 CH3I E…

A: Given reaction is:

Q: An analytical chemist is titrating 118.6 mL of a 0.5800M solution of diethylamine ((C,H,), NH) with…

Q: An analytical chemist is titrating 77.1 mL of a 0.5400M solution of piperidine (C,H,,NH) with a…

A: Step 1: Given the information:Molarity of ppiperidine = 0.5400 MVolume of piperidine = 77.1…

Q: What will happen when CH3NH3Cl is added to a CH3NH2 solution? Will it change the pH of the solution…

Q: would need with these questions step by step: Calculate the ratio of ethyl amine (CH3CH2NH2) to the…

Q: An analytical chemist is titrating 222.2 mL of a 0.3600M solution of methylamine (CH3NH₂) with a…

Q: Phosphoric acid is a triprotic acid with the p?a values p?a1=2.148, p?a2=7.198, and p?a3=12.375.…

A: Ionization of phosphoric acid is,

Q: buffer

Q: An analytical chemist is titrating 127.4 mL of a 0.1500M solution of methylamine (CH3NH₂) with a…

Q: You are studying a clear solution and you added the pH indicator methyl violet. The colour range of…

A: The color of a solution of pH 0.2 is needed to be determined on the addition of an acid-base…

Q: An analytical chemist is titrating 190.6 mL of a 0.3000M solution of methylamine (CH3NH₂) with a…

Q: Which one of the following mixtures in aqueous solution would be an effective buffer solution?…

A: Buffer is the solution of mixture of weak acid/weak base with its salt of strong base/strong acid

Q: 8. In this case, the pH of the Flint River is well-characterized at 7.92. Based on your chemical…

A: Hello. There are multiple questions posted together. The first question has been solved. To receive…

Q: What is the pH of a mixture of 0.039 M NaH2PO4 and 0.061 M NaHPO4? The pka of phosphate buffer is…

Q: A buffer solution is 0.384 M in H2CO3 and 0.328 M in KHCO3. If Kal H2 CO3 is 4.2 × 10-7, what is the…

A: Answer 1 As we know the pH of acidic buffer solution is given by the formula pH = pKa +…

Q: One of the buffers that contributes to pH stability in human blood is carbonic acid (H2CO3).…

A: If the pH of the blood increases the buffer will act in such a way that reduces the pH. It is the…

Q: 2) The ionization constant for NH3 in water is 1.8 x 10 - 5. Determine the hydroxide ion…

A: Welcome to bartleby ! As per company norms we cannot answer more than one question per session .So,…

Q: An analytical chemist is titrating 248.4 mL of a 0.1600M solution of diethylamine ((C¿H5),N with a…

A: Question is based on the concept of titrations. We have to calculate pH of the solution after adding…

Q: I'll give you 100%rating if you answer all questions. They are interconnected with each other that's…

A: The first method used is pH strip method and the 2nd method used is the titration method. The…

Q: An analytical chemist is titrating 215.4 mL of a 0.1400 M solution of methylamine (CH3NH₂) with a…

A: The question is based on the titrations. we are titrating a weak base with a strong acid. we need…

Q: Part b and C What volume of 0.110 M HCI is required for the complete neutralization of 1.10 g of Na2…

A: From the balanced chemical reaction between HCl and Na2CO3, we can solve these problems. 2HCl +…

Q: What is the pH of a buffer solution if you dissolve 300 ml of 1.65M Formic Acid (HCO2H) and 250 ml…

A: We will first calculate the millimoles of both weak acid and salt. And will find the final…

Q: An analytical chemist is titrating 169.0 mL of a 0.8600M solution of methylamine (CH3NH₂) with a…

A: The buffer is defined as the solution containing equal amount of a weak acid and its conjugate base…

Q: What [H2C03] needs to be added to 0.0250M NaHCO3 to obtain a buffer solution with a pH of 7.0?

A: A buffer solution is an aqueous solution consisting of a mixture of a weak acid and its conjugate…

Q: An analytical chemist is titrating 199.2 mL of a 0.3400M solution of formic acid (H, Co,) with a…

A: First we would Calculate moles of both acid and base using formula : Moles = Molarity × Volume (L)…

Q: An analytical chemist is titrating 89.4 mL of a 0.9900M solution of benzoic acid (HC H,CO₂) with a…

A: Benzoic acid react with NaOH to produce sodium benzoate and water, we will construct ICE table to…

Q: A buffered solution containing disolved aniline, C6H5NH2, and aniline hydrochloride, C6H3NH3Cl, has…

A: A. Given that : pH of the buffer solution = 5.71 Concentration of base (C6H5NH2) = 0.290 M The pKb…

Q: 2. Explain the term 'buffer capacity'.

A: Explanation of term "buffer capacity "

Q: An analytical chemist is titrating 78.3 mL of a 0.7900M solution of aniline (C6H5NH₂) with a 0.2500M…

Q: ne pka of HCOOH is 3.74 and the pH of an HCOOH, fer solution is 3.89, which of the following is…

A: pH of buffer solution is calculated by using Henderson Hessalbalch equation

Q: An analytical chemist is titrating 211.2 mL of a 0.5700M solution of aniline (CH₂NH₂) with a 0.7200M…

Q: Buffer solutions with the component concentrations shown below were prepared. Which of them should…

A: Given, (E). [CH3COOH] = 0.25 M, [CH3COO-] = 0.25 M(C). [CH3COOH] = 0.75 M, [CH3COO-] = 0.75 M(D).…

Q: An analytical chemist is titrating 112.7 mL of a 0.6400M solution of ethylamine (C₂H5NH₂) with a…

A: Given, Molarity of the ethylamine C2H5NH2 = 0.6400 M = 0.6400 mole/L The volume of the ethylamine…

Q: An analytical chemist is titrating 57.8 mL of a 0.6200M solution of methylamine (CH,NH,) with a…

Q: An analytical chemist is titrating 200.4 mL of a 0.6100M solution of methylamine (CH3NH2) with a…

A: Detailed explanation:Given the following:Volume of CH₃NH₂=200.4 mLMolarity of CH₃NH₂=0.6100 MpKb…

Q: An analytical chemist is titrating 202.9 mL of a 0.6300M solution of aniline (C,H,NH,) with a…

Q: 11.An acid-base equilibrium system is created by dissolving 0.20mol CH3COOH in water and diluting…

Q: Determine the mass of H2C2O4.H2O required to prepare 0.1N solution in 100 ml volume. Explain two…

A: Hi, since you have posted multiple questions, we will answer the very first question for you. Kindly…

Q: An analytical chemist is titrating 59.5mL of a 0.8600M solution of aniline C6H5NH2 with a 0.07400M…

A: Given data : Concentration of aniline = 0.86 M Volume of aniline = 59.5 mL Concentration of HNO3 =…

Q: For each of the following salts, write the dissociation reaction of the hydrolysis reactions for…

Q: The ability of a solution to resist changes to the pH from added acid or base depends upon the…

A: We know that best buffering occurs, when buffering capacity is 1.

Q: A compound has a pk, of 6.9. To 100 mL of a 1.0 M solution of this compound at pH 7.9 added 40 mL of…

Q: An analytical chemist is titrating 74.8 mL of a 0.7500M solution of propylamine (C,H,NH,) with a…

Q: An analytical chemist is titrating 143.3 mL of a 0.7900M solution of aniline (C6H5NH₂) with a…

A: Here we have to determine the pH of solution when 143.3 ml of aniline solution is titrated with…

Q: An analytical chemist is titrating 221.9 mL Oof a 0.9800M solution of propionic acid (HC,H,CO,) with…

Q: (The Ka value for HF is 6.6 x 10*.) 3. Using the value of K, from the previous question, show how to…

A: We’ll answer the first question since the exact one wasn’t specified. Please submit a new question…

Q: Which of the following solutions would have the highest buffer capacity? O A 1.00 L solution that…

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

Question

Show by 2 net ionic equations how NaHCO3 may act as a buffer.

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

Trending now

This is a popular solution!

Step by step

Solved in 1 steps with 1 images

SEE SOLUTION Check out a sample Q&A here

Similar questions

10 11 12 13 14 An analytical chemist is titrating 234.9 mL of a 0.2700M solution of ethylamine (C,H,NH,) with a 0.1500M solution of HNO2. The p K, of ethylamine is 3.19. Calculate the pH of the base solution after the chemist has added 484.1 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places. pH =| Submit Assignment Continue
Salt Solution 0.100 M NaHSO4 0.100 M Na₂CO3 0.100 M NH3 0.100 M NaCl Measured pH 1.40 11.41 11.31 2.83 For each solution having a pH less than 6 or greater than 8, write a balanced net ionic reaction that shows why the concentration of H₂O* (if the solution is acidic) or OH¯ (if the solution is basic) is greater in this solution than it would be in pure water alone. (Remember that net ionic reactions omit spectator ions.)
Calculate the volume (ml)of concentrated ammonia and the weight (gm) of ammonium chloride respectively to be taken to prepare 100 ml of buffer solution at a pH of 10 if the final concentration of the salt is 0.20 mol. Note that the molar concentration of concentrated ammonia is equal to 14.8 mol/liter, and that the pKb of ammonia is 4.76, and the molecular weight of ammonium :chloride 53.5 g/mole.lt is about
The pKa of Cl3CCO2H is 0.64. What is the pH of a 0.580 M solution? What percentage of the Cl3CCO2H is dissociated?
An analytical chemist is titrating 186.4 mL of a 0.3400M solution of methylamine (CH3NH₂) with a 0.6900M solution of HIO3. The pK² of methylamine is 3.36. Calculate the pH of the base solution after the chemist has added 98.0 mL of the HIO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HIO3 solution added. Round your answer to 2 decimal places. pH = 1 X Ś
An analytical chemist is titrating 123.0 mL of a 0.5600M solution of diethylamine ((C₂H₂), NH) with a 0.5300M solution of HNO3. The pK, of diethylamine 2 is 2.89. Calculate the pH of the base solution after the chemist has added 111.5 mL of the HNO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added. Round your answer to 2 decimal places.
Which solution below would have the greatest buffering capacity? The solution was prepared from a weak acid and the salt of its conjugate base. O 0.0708 M HCOOH and 0.0708 M HCOONa, Ka = 1.74e-4 O 0.175 M CICH2COOH and 0.175 M CICH₂COONa, Ka = 1.51e-3 O 0.0756 M HCOOH and 0.0756 M HCOOK, Ka = 1.74e-4 O 0.0730 M CICH2COOH and 0.0730 M CICH₂COOK, Ka = 1.51e-3
10 An analytical chemist is titrating 120.4 mL of a 0.5800M solution of piperidine (C5H₁NH) with a 0.7600M solution of HNO3. The pK, of piperidine is 2.89. Calculate the pH of the base solution after the chemist has added 64.0 mL of the HNO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added. Round your answer to 2 decimal places. pH = 0 Ś
I would need help with these problems, please show step by step: 35.00 mL of a 0.30 M HCl solution is titrated with 0.35 M NaOH. What is the pH of the solution after 40.00 mL of the NaOH has been added? 50.00 mL of 0.10 M HNO2 is titrated with a 0.10 M KOH solution. After 25.00 mL of the KOH solution is added, what will be the pH in the titration flask ? Calculate the pH at the equivalence point for the titration of 0.100 M HCl with 25.00 mL of 100 M NH3 .
You need to prepare a buffer solution from NaH2 PO4 and Naz HPO4 to have a pH of 8.00. What ratio of amounts of Naz HPO4 and NaH2PO4 should you take? (Ka2 = 6.2 × 10-8) (Simplify your answer completely.) n(Naz HPO4) n(NaH2 PO4)
An analytical chemist is titrating 126.8 mL of a 0.2600M solution of diethylamine ((C₂H), NH) with a 0.1600M solution of HNO3. The pK, of diethylamine is 2.89. Calculate the pH of the base solution after the chemist has added 83.3 mL of the HNO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added. Round your answer to 2 decimal places. pH = 0 x 5 ? do
An analytical chemist is titrating 225.3 mL of a 1.100M solution of formic acid (H,CO,) with a 1.200M solution of KOH. The pK, of formic acid is 3.74. a Calculate the pH of the acid solution after the chemist has added 99.62 mL of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added. Round your answer to 2 decimal places. pH = ]