Answered: Write a balanced chemical equation for…

Write a balanced chemical equation for the equilibrium reaction occurring in a buffer containing NH3 and NH4Cl. Write the equation so that its equilibrium constant is equivalent to Ka.

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.83QE

See similar textbooks

Related questions

Q: Consider a buffer solution prepared from HOC1 and NaOC1. Which is the net ionic equation for the…

A: A molecular equation is defined as the chemical equation which is written using the chemical formula…

Q: Why does a buffer resist changes in pH?

A: Why does a buffer resist changes in pH has to be given,

Q: A buffer solution includes a weak acid and its conjugate base. Include states of matter. Write a…

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

Q: Differentiate the carbonate buffer and phosphate buffer systems in terms of pH and pKa. Give…

A: Difference between the carbonate and phosphate buffer is given below and also function of each…

Q: Write a balanced chemical equation for the equilibrium reaction occurring in a buffer containing NH3…

Q: A buffer is prepared by dissolving a base, HONH2, and its conjugate acid, HONH3NO3, in some water.…

A: Buffer solution is a combination of a weak acid and its conjugate base or a weak base and its…

Q: What is the pH of a buffer solution that contains 20.0mL of 0.10M H2CO3 and 50.0mL of 0.10M NaHCO3?

A: We would use Henderson Hasselbalch equation to calculate the pH of buffer solution.

Q: How you would prepare 0.50 L of a 2.5 M bicarbonate/carbonate buffer system at a pH of 10.0.

A: The ratio of carbonate and bicarbonate ions in the given buffer solution can be calculated using…

Q: Explain how a buffer solution of carbonic acid and bicarbonate will react when: a strong acid,…

A: pH of a buffer solution remain unchanged with addition of few drops of acid and base.

Q: How does the buffer react to the addition of acids and bases? In comparison, how does water react to…

A: Buffer solutions are aqueous solutions that resist the change in pH on addition of small amount of…

Q: What is the PH of a buffer system that is 0.200 M hydrocyanic acid (HCN) and 0.120 M sodium cyanide…

A: Given: The concentration of acid, [HCN]= 0.200 M The concentration of salt, [NaCN]=0.120 M…

Q: What is the pH of a buffer solution that is 0.40 M in formic acid (HCHO2) and 0.90 M in sodium…

A: Given: pKa of formic acid = 3.74 Concentration of formic acid = 0.40 M Concentration of sodium…

Q: An aqueous solution is prepared by dissolving 0.23 mol of hydrazoic acid and 0.27 mol of sodium…

A: Given: Buffer solution of hydrazoic acid i.e. HN3 and sodium azide i.e. NaN3.

Q: Classify these salts according to Strength and Role in the Buffer system 1. NaOCl 2. NaNO3 3.…

A: 1. NaOCl is neutral salt and it cannot alter pH 2. NaNO3 is neutral salt and it can't alter the pH…

Q: . It is possible to make a buffer that functions well near pH 7, using citric acid, which contains…

A: A buffer solution is the one where the weak acid and its conjugate base or a weak base with its…

Q: In the lab, you perform an experiment in which you add HCIO4 and a beaker containing NH3. What will…

A: Equivalence point is the point in titration at which the amount of titrant added is just enough to…

Q: How does the buffer solution absorb the added H+ and OH- to make the pH change very small?

A: A buffer can be acidic or basic in nature. A buffer that contains a weak acid with its conjugate…

Q: what is the ph of a buffer solution composed of 0.50m formic acid and 0.70m sodium formate

A: Answer: 3.90 Given buffer solution contains formic acid, HCOOH , a weak acid, and sodium formate,…

Q: Show with the appropriate equations how a sodium acetate-acetate acid buffer prevents each of the…

A: The buffer solutions are solutions whose pH do not change considerably Upon addition of strong acid…

Q: A lactic acid/lactate ion buffer solution contains 0.11 M HC3H;O3 and 0.78 M C;H;O3¯, respectively.…

A: pH is a scale used to specify the acidity or basicity of an aqueous solution. A buffer solution is…

Q: Why does buffer capacity increase as the concentration of buffer increases?

A: The solutions which have a nearly constant value of pH or they resist any change in pH value are…

Q: When you prepare a buffer, it is recommended to use a weak acid whose pKa is close to the pH…

A: Here we have to explain why to make a buffer solution the weak acid chosen should have pKa close to…

Q: Write the Henderson-Hasselbech equation for ammonium/ammonia buffer system.

Q: A buffer solution made from NaHCO3 and NazCO3 has a pH in the range of 9-11. Write balanced…

Q: Write the chemical equation for the reaction that occurs when 0.10 M hydrochloric acid (HCI) is…

A: 0.10 M hydrochloric acid (HCl) is added to the buffer solution that is made up of acetic acid…

Q: >A buffer contains significant amounts of ammonia and ammonium chloride. Write equations showing…

A: A buffer solution consists of specific amounts of weak acid and its conjugate base or specific…

Q: What is pH of blood? Is it acidic, basic or neutral? Name and write the formula of the buffers which…

A: Interpretation- To tell about What is pH of blood? Is it acidic, basic or neutral? Name and write…

Q: What mass of sodium formate must be added to 400 mL of 1.00 M formic acid to produce a buffer…

A: We have to find mass of sodium formate must be added to 400 mL of 1.00 M formic acid to produce a…

Q: Calculate the pH of a NH4+ buffer system when 10.0 mL of 0.1 M NH3 is mixed with 1.0 mL of a 0.001 M…

A: The value of pOH using the Henderson-Hasselbalch equation is calculated as: pOH=pKb+logConjugate…

Q: Write a net ionic equation that shows how this buffer neutralizes added base (NaOH).

Q: What is a buffer solution? What constitutes a buffer solution?

A: Ab buffer solution is a solution that consists of a mixture of weak acid along with its conjugate…

Q: What is the pH of buffer solution containing 0.25 M acetic acid and 0.4 M sodium acetate ?

A: Answer:- this question is answered by using the simple concept of calculation of pH of a buffer…

Q: What is the general composition of a buffer and in your own words explain why it resists change in…

A: Buffers are made up of specific solute pairs to accomplish this a Weak acids and its derived salts…

Q: Write the carbonate buffer equation and explain how it works to buffer blood pH

A: A mixture of a weak acid and corresponding conjugate base or vice-versa results in the formation of…

Q: The Henderson-Hasselbalch equation relates the pH of a buffer to the relative concentrations of the…

A: Buffer solution is prepared, when an strong base is added into weak acid solution then resulting…

Q: What are the characteristics of an effective buffer?

Q: Define the following terms: a. Henderson–Hasselbalch equation b. bicarbonate ion c. protein buffer…

A: Henderson-Hasselbalch equation is used to calculate the pH value of a given buffer solution. It was…

Q: 4. CH3NH3CI Makes a buffer with HCIO, 5. CIO4 Makes a buffer with CH3NH3B 6. CH3NH2 Lewis base, not…

A: Superacid HClO4 Lewis acid, not a Bronsted Lowry acid BeF2 is the Lewis acid since it can accept…

Q: Describe the meanings of acidosis and alkalosis. How do buffers function in this system?

A: To define acidosis,alkalosis and the function of buffer in this system is given.

Q: When a buffer contains equal concentration of the acid and its conjugate base, the pH of the buffer…

Q: When the pH is below the pKa, is the buffer species more or less than 50% protonated? Explained in…

A: Given -> pH is below the pKa value.

Q: Identify the buffer system(s) - the conjugate acid-base pair(s)- present in a solution that contains…

A: A buffer system is possible only if the mixture contains weak acid, such as HF, and a salt of this…

Q: What is the effect of concentration of the weak acid on pH of the buffer solution? Explain.

Q: Which statement describes the action of a buffer composed of propionic acid (CH, H, COOH) and sodium…

Q: A buffer contains H2P04- and HPO42-. write the reaction that occurs when NaOH is added.

A: The buffer has H2PO4- and HPO42- The conjugate acid will be H2PO4- and conjugate base will be…

Q: What factors influence the effectiveness of a buffer? What are the characteristics of an effective…

A: Buffer helps to resist the change in pH of a solution when a little amount of acid or base added. An…

Q: How does dilution with water affect the pH of a buffer solution?

A: The pH of a buffer solution is given by: where [A-] is the concentration of the salt and [HA] is…

Q: A buffer is prepared using lactic acid (HLac) and sodium lactate (NaLac). 0.300 dm3 of the 0.500…

A: Given: pKa of lactic acid = 1.4 * 10-4

Q: Use the buffer equation to calculate the pH of buffer solutions prepared by dissolving the following…

Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

Write a balanced chemical equation for the equilibrium reaction occurring in a buffer containing NH₃ and NH₄Cl. Write the equation so that its equilibrium constant is equivalent to K_a.

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

Step 2

Step 3

Step 4

Trending now

This is a popular solution!

Step by step

Solved in 4 steps with 3 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

What is the number of moles of 10.0 g NH₄Cl? What is the molar concentration of NH₄Cl? What is the pH of the buffer solution?
One of the buffer systems the human body has to regulate pH is based on the phosphate anion. If blood has a pH of 7.40, and the three Ka values for phosphoric acid are 7.52 × 10−3, 6.23 × 10−8, and 4.8 × 10−13, write the chemical equilibrium equation showing the phosphate species that are involved in this buffer.
2. Explain the term 'buffer capacity'.
Equimolar quantities of potassium fluoride and hydrofluoric acid are placed into solution. What happens to the buffer system if some hydrochloric acid is added to the solution? The hydrochloric acid reacts with the fluoride ions so the pH decreases only slightly. The hydrochloric acid reacts with the fluoride ions so the pH decreases significantly. ) The hydrochloric acid reacts with the hydrofluoric acid so the pH increases only slightly. The hydrochloric acid reacts with the hydrofluoric acid so the pH increases significantly.
To 1.0 L of a 0.36 M solution of HClO2 is added 0.19 mol of NaClO. Calculate the [HClO2][HClO2] at equilibrium. Express your answer using two significant figures.
A buffer solution is 0.080 M in lactic acid (Ka = 1.8 × 10−4) and 0.070 M in sodium lactate. The pH of the solution is
10.0 ml of HCl was added to 100.0 ml of a 0.2 M solution of NH4Cl (Ka=1.8x10-5). The resulting equilibrium pH was 1.4.What is the equilibrium concentration of NH3?
Calculate the pH of each of the following buffered solutions. Ka(HC, HgO,)= 1.8 × 10 5 1.0.19 M acetic acid/0.29 M sodium acetate pH = 2. 0.29 M acetic acid/0.19 M sodium acetate pH = 3. 0.060 M acetic acid/0.21 M sodium acetate pH = 4. 0.21 M acetic acid/0.060 M sodium acetate pH = Visited
3. A formic acid buffer is prepared with 0.010 M each of formic acid (HCOOH) and sodium formate (NaCOOH). The Ka for formic acid is 1.8 x 104. What is the pH of the solution? What is the pH if 0.0020 M of solid sodium hydroxide (NaOH) is added to a liter of buffer? What would be the pH of the sodium hydroxide solution without the buffer? What would the pH have been after adding sodium hydroxide if the buffer concentrations had been 0.10 M instead of 0.010 M? eit af
33. Consider a buffer solution that contains 0.45 M HCOOH and 0.55 M NaHCOO. Note that the Ka for formic acid (HCOOH) is 1.8 x 104. (a) Calculate the pH of this buffer solution. pH = (b) Write the net ionic chemical equation that occurs when potassium hydroxide (KOH) (MW of KOH = 56.1 g/mol) is added to the buffer. (c) If 0.260 g of solid KOH is added to 250. mL of this buffer solution, what is the resulting pH of the solution? New pH =
Determine the concentration of C₆H₅NH₃⁺ in a buffer solution by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the concentration of C₆H₅NH₃⁺. Complete Parts 1-3 before submitting your answer. A buffer solution contains dissolved C6H5NH2 and C6H5NH3Cl. The initial concentration of C6H5NH2 is 0.50 M and the ph of the buffer is 4.20. The kb for C6H5NH2 is 3.8 * 10^-10.
11.An acid-base equilibrium system is created by dissolving 0.20mol CH3COOH in water and diluting the resulting solution to a volume of 1.0 L. What is the effect of adding 0.020 mol CH3COO (aq) to this solution? How will pH change (calculate pH before and after the addition. Ka of CH3COOH is 1.76 x10-5)? How will concentrations of CH3COOH and CH3COO at equilibrium change?