**Buffer pH Calculation****Problem Statement:**What is the pH of a buffer prepared by mixing 5.0 g of ammonia (NH₃) and 20.0 g of ammonium chloride (NH₄Cl) in enough water to form 2.50 L of solution? The \( K_b \) of ammonia is \( 1.76 \times 10^{-5} \).**Explanation:**To solve this problem, one would typically use the Henderson-Hasselbalch equation once the concentrations of the acid and base forms in the buffer solution have been calculated. It involves calculating the moles of ammonia and ammonium chloride, converting to molarity, and applying the equation to find the pH.Note: The problem involves understanding of buffer solutions, molarity calculations, and application of equilibrium constants.

Given that: Mass of ammonia = 5.0g Mass of ammonium chloride = 20.0g Kb = 1.76×10-5

Answered: 2. What is the pH of a buffer prepared…

2. What is the pH of a buffer prepared by mixing 5.0 g of ammonia (NH3) and 20.0 g of ammonium chloride (NH4CI) in enough water to form 2.50L of solution. The Kb of ammonia

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: A solution is prepared that is initially 0.24 M in trimethylamine ((CH 3),N), a weak base, and 0.30…

A: Given, Initial concentration of (CH3)3N = 0.24 M Initial concentration of (CH3)3NHCl = 0.30 M The…

Q: A buffer solution is made that is 0.423 M in HCN and 0.423 M in NaCN. If K, for HCN is 4.00 x 10-10,…

Q: To make a common phosphate buffer using potassium hydrogen phosphate and potassium dihydrogen…

A: Answer: A buffer solution is the type of solution that resist the change in its pH on adding small…

Q: The K, of hydroxylamine, NH,OH, is 1.10 x 108. A buffer solution is prepared by mixing 100.0 mL of a…

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

Q: The dissociation constant of lactic acid, a monoprotic acid found in sour milk, is 1.4 x 104. A…

A: 1) The given solution is not a buffer, as a buffer is formed by a weak acid and a salt of that weak…

Q: buffer solution is formed by adding 0.320 moles of solid sodium lactate, NaC₃H₅O₃, to 600.0 ml of…

Q: Fill in the blanks: A buffer solution is consists of 0.100 M HCN and 0.200 M NaCN. HCN + H₂O H30* +…

A: For a buffer 0.100M HCN and 0.200M NaCN, we have to find pH of solution. We have to find pH after…

Q: I mix 100 mL of 0.100 M HCl in 250 mL of 0.150 M NH3. I add 50.0 mL of 0.0500 M NaOH. What is the…

Q: A 1.0-L 0.010 M buffer with pH 6.50 is given as an assignment to a group of students. Which is the…

A: Buffers are the solutions that do not change their pH to large extent when small amount of conc.…

Q: A solution NH3 that contains 72 mL of 0.043 M ammonia, NH3, is titrated with 0.083 M HCI. The Kb of…

A: Moles of NH3 (M1) =0.043M Moles of HCl (M2)=0.083M Volume of NH3 (V1) = 72ml Volume of HCl (V2) =?

Q: You are asked to prepare a pH = 3.00 buffer solution startingfrom 1.25 L of a 1.00 M solution of…

A: (a) Given: Concentration of HF – 1.00 M pH of the buffer solution = 3.00 Volume of solution = 1.25 L…

Q: 2 chlorobutane +sodium hydroxide = alcohol

Q: A chemistry graduate student is given 300. mL of a 1.20M nitrous acid (HNO2) solution. Nitrous acid…

A: Answer:Buffer solution is a type of solution that resists the change in its pH on adding small…

Q: An aqueous solution contains 0.449 M ethylamine (C₂H5NH₂). How many mL of 0.303 M perchloric acid…

Q: 1. 50.0 ml of 0.1 M NaOH is added to 100.0 ml of 0.2 M HCN (Ka=6.2x10-10). What is the pH of the…

A: Since you have posted multiple questions, we are entitled to answer the first only. 1) Given:…

Q: suppose that the ph of buffer A turned out at ph 5.5 instead of ph 5.0 (100.0 mL of a 0.5 M buffer)…

A: Buffer solution is defined as a solution which resists any change in its pH value even when small…

Q: To a 500 mL of buffer solution consisting of 0.25 M Acetic acid (HAc) and 0.50M Sodium acetate…

A: As per Henderson Hasselbalch equation, pH of a buffer solution = pKa + log [salt] / [acid] Here acid…

Q: Calculate the pH of a bicarbonate/carbonate buffer in which the concentration of sodium bicarbonate…

A: The buffer is basically a solution whose pH does not change much by adding a small amount of acid or…

Q: A chemistry graduate student is given 500. mL of a 0.40M ammonia (NH₂) solution. Ammonia is a weak…

A: The question is based on the concept of the pH of the solution.It is defined as a negative logarithm…

Q: What is the pH of the buffer solution that contains 1.1 g of NH, CI in 250 mL of 0.080 M NHs? Is the…

A: Henderson equation for basic buffer solution is pOH = pKb + log [salt][base]

Q: 4. Formic acid, HFor, has a K value of 1.8 x 104. You need to prepare 125 mL of a buffer hav- ing a…

Q: You need to prepare a pH = 9.20 buffer solution containing NH3 and NH4Cl. If you start with 0.63 M…

A: Buffer Question and finding the concentration of Salt to make a buffer of pH = 9.2

Q: A buffer is made using 100.0 mL of 0.100 M CH;CH,COOH (propanoic acid) and 100.0 mL of 0.100 M…

A: A buffer is an aqueous mixture of a weak acid with its conjugate base or a strong base with its…

Q: A chemistry graduate student is given 100. mL of a 1.40M methylamine (CH3NH2) solution. Methylamine…

A: pKb = - log Kb = - log (4.4 * 10-4 ) = 3.36pKa = 14-pKb = 14- 3.36…

Q: Consider the buffer system of carbonic acid (H₂CO₂) and its salt, KHCO3, which provides the…

A: 1.) A base will react with acidic part of the buffer. 2.) The reaction can be determined on the…

Q: An aqueous solution contains 0.430 M ammonia (NH3). How many mL of 0.384 M nitric acid would have to…

Q: A buffer prepared by adding 115.0 mL of 0.17 M NH3 to 145.0 mL of 0.15 M NH4NO3. What is the pH of…

Q: A buffer solution contains 0.50 mol of acetic acid and 0.50 mol of sodium acetate in 1.0 L of…

A: Given, Moles of CH3COOH = 0.50 mole Moles of CH3COONa = 0.50 mole Volume in L = 1.0 L a). What…

Q: A pH buffer is a solution that resists changes in pH when acids or bases are added to it—typically,…

A: We have to prepare 7.00 L of pH = 12.00 buffer.

Q: 8. Which of the following is TRUE about buffer solution? a. pH of buffer solution will never change…

A: Buffer solution is made up of weak acids or weak bases with their conjugate base or conjugate acid.…

Q: Calculate the pH of a buffer solution prepared by dissolving 0,48 mole of sodium fluoride (NaF) and…

A: Buffer solution is a type of solution which resist the pH change when small amount of acid or base…

Q: Choose one option only. Buffer A. prepared by mixing 1.32 mol NH3 and 3.26 mol NH4Cl into 2.20 L of…

A: To check the correct Statement, we would first calculate pH of each buffer solution using Henderson…

Q: Consider the titration of 50.00 mL of 0.100 M benzoic acid (HC7H5O2, Ka = 6.3 × 10−5) (aq) with…

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

Q: Consider a buffer made from 255 mL 0.10 M HC2H3O2 and 125 mL 0.10 NaC2H3O2. Ka for HC2H3O2 is 1.8 x…

A: Moles of HC2H3O2 = Molarity × Volume = 0.10 M ×0.255 L Moles of…

Q: A solution contains 0.339 M HA (K₂5.39-10) and 0.771 M NaA. What is the pH of this solution? What is…

Q: A buffer is prepared by adding 4.8 g of (NH4)2SO4 to 425 mL of 0.258 M NH3. Assuming that the volume…

A: Formula used : pOH = pKb - log[base]/[salt] Also pH + pOH = 14

Q: A titration is performed in which 0.10 M LIOH is added to a 200.0 mL sample of 0.40 M HF. What is…

A: HF is a weak acid it reacts with LiOH which is a strong base and gives fluoride ion. Now this…

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

**Buffer pH Calculation**

**Problem Statement:**

What is the pH of a buffer prepared by mixing 5.0 g of ammonia (NH₃) and 20.0 g of ammonium chloride (NH₄Cl) in enough water to form 2.50 L of solution? The \( K_b \) of ammonia is \( 1.76 \times 10^{-5} \).

**Explanation:**

To solve this problem, one would typically use the Henderson-Hasselbalch equation once the concentrations of the acid and base forms in the buffer solution have been calculated. It involves calculating the moles of ammonia and ammonium chloride, converting to molarity, and applying the equation to find the pH.

Note: The problem involves understanding of buffer solutions, molarity calculations, and application of equilibrium constants.

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

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

2
6. Which of the following mixtures would create an effective buffer? Give your reasoning in each case. a) 0.10 mol HCl and 0.10 mol NaOH in 1.0L H₂O. b) 0.10 mol NH3 and 0.15mol NH4Cl in 1.0L H₂O. c) 0.010mol HCN and 0.20mol NaCN 1.0L H₂O. d) 0.10 mol NH4Cl and 0.20mol NaCN in 1.0L H₂O. e) 0.10 mol HCl and 0.20mol NaCN 1.0L H₂O.
8b.
4. What is the pH of a buffer made from 0.42 M H3BO3 and 0.22 M H2BO3-, if the Ka for H3BO3 is 7.3 x 10-10 ? (use 2 decimal places for pH)
A chemistry graduate student is given 300. ml. of a 1.40M chlorous acid (HCIO₂) solution. Chlorous acid is a weak acid with K-1.1 x 10 What mass of NaCIO, should the student dissolve in the HCIO, solution to turn it into a buffer with pH -1.947 You may assume that the volume of the solution doesn't change when the NaCIO, is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. X
bha A buffer prepared by dissolving oxalic acid dihydrate (H2C2O4·2H2O) and disodium oxalate (Na2C2O4) in 1.00 L of water has a pH of 5.333. How many grams of oxalic acid dihydrate (MW = 126.07 g/mol) and disodium oxalate (MW = 133.99 g/mol) were required to prepare this buffer if the total oxalate concentration is 0.241 M? Oxalic acid has pKa values of 1.250 (pKa1) and 4.266 (pKa2).
3. Please solve the following chemistry problem.
How many moles of CH;NH;CI need to be added to 200.0 mL of a 0.500 M solution of CH3NH2 (Kb for CH3NH, is 4.4 x 104) to make a buffer with a pH of 9.70?
A chemistry graduate student is given 125. mL of a 1.00 M methylamine (CH ,NH,) solution. Methylamine is a weak base with K,=4.4× 10 *. What mass of CH,NH,Br should the student dissolve in the CH,NH, solution to turn it into a buffer with pH =11.05? You may assume that the volume of the solution doesn't change when the CH,NH,Br is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.
A buffer solution consisting of 0.15 moles of ammonia dissolved in half a liter of water. How much ammonium chloride (gram) must be added to this solution so that its pH value is equal to 9.4 at a temperature of 25 C.The Kb of ammonia is equal to 1.8x 10 -5,and the molecular weight of ammonium chloride is 53.5 g/mole.*
An analytical chemist is titrating 239.7 mL of a 0.6100M solution of benzoic acid (HC,H,CO, with a 0.4400M solution of NaOH. The p K, of benzoic acid is 4.20. Calculate the pH of the acid solution after the chemist has added 135.5 mL of the NaOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH solution added. Round your answer to 2 decimal places. pH = U
3. A buffer solution is prepared by adding 5.50 g of ammonium chloride and 0.0188 mol of ammonia to enough water to make 155 mL of solution. What is the pH of the buffer? (Ka for NH4+= 5.6 x10-10),