**Buffer Preparation Using Ammonium Chloride and Ammonia****Question:** How many grams of solid ammonium chloride should be added to 0.500 L of a 0.190 M ammonia solution to prepare a buffer with a pH of 9.850?**Answer:** Mass = 0.936 g---**Explanation:**To prepare a buffer solution with a desired pH, solid ammonium chloride is added to an ammonia solution. The precise amount required to reach a pH of 9.850 with the given volume and molarity of the ammonia solution is found to be 0.936 grams. Understanding buffer solutions:- Buffers are solutions that resist changes in pH when small amounts of acid or base are added.- The ammonia (NH₃) acts as a weak base, while the ammonium chloride (NH₄Cl) provides the conjugate acid (NH₄⁺).- This balance between NH₃ and NH₄⁺ maintains the pH close to the desired value, making it effective for buffering applications.

Given,Molarity of NH3 = 0.190 Mvolume of NH3 = 0.500 LpH = 9.850Kb of NH3 = 1.8 x 10-5

Answered: How many grams of solid ammonium…

How many grams of solid ammonium chloride should be added to 0.500 L of a 0.190 M ammonia solution to prepare a buffer with a pH of 9.850? Mass = 0.936 g

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: 6. Suppose you add aodiu hudroside to the buffered solution described on the board below We out the…

A: The given solution contains weak acid HA and the conjugate base A- of the acid. They together form a…

Q: The pH of a solution made by mixing 50.0 mL of 0.13 molar B, a weak base, with 20.0 mL of 0.19 M HCl…

A: The pOH of a solution by mixing weak base and HCl is calculated as,

Q: How many moles of sodium hydroxide would have to be added to 250 mL of a 0.435 M acetic acid…

Q: How many moles of sodium hydroxide would have to be added to 250 mL of a 0.385 M hypochlorous acid…

A: The volume of hypochlorous acid = 250 mL The molarity of hypochlorous acid = 0.385 M pH of buffer to…

Q: Which of the following combination of solutions will form a buffer solution? (A) 50.0…

A: Buffer solution: The solution which contains weak acid mixed up with its conjugated acid or a weak…

Q: dont know how to do this question

A: A buffer solution is a mixture of weak acid and it's conjugate base or weak base and it's conjugate…

Q: what volume of acetic acid 0.1 M and what volume of sodium acetate 0.1 M should be added together to…

A: Let the volume of acetic acid be x and the volume of sodium acetate solution be y. The pKa value of…

Q: A buffer solution contains 0.385 M ammonium bromide and 0.448 M ammonia. If 0.0245 moles of…

Q: An aqueous solution contains 0.442 M dimethylamine ((CH3)2NH). How many mL of 0.264 M hydrobromic…

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

Q: A buffer is prepared by adding 20.0g of sodium acetate to 500 mL of a 0.150 M acetic acid solution.…

A: mass of sodium acetate = 20.0 g molecular weight of sodium acetate = 82.03 g/mol Number of moles of…

Q: How many moles of sodium hydroxide would have to be added to 225 mL of a 0.404 M nitrous acid…

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 0.384 M acetic acid. How many mL of 0.203 M potassium hydroxide would…

A: Given => Molarity of acetic acid aqueous solution = 0.384 M Volume of this Solution = 225 ml pKa…

Q: 3. What is the pH of a buffer that is 0.175 M in a weak acid and 0.200 M in the acid's conjugate…

A: Given that: Concentration of weak acid [HA] = 0.175M [A-] = 0.200M Ka = 5.7×10-4

Q: An aqueous solution contains 0.447 M dimethylamine ((CH3)2NH). How many mL of 0.246 M…

A: we need to find the volume of 0.246 M perchloric acid added to form the buffer solution with pH…

Q: How many moles of potassium hydroxide would have to be added to 225 mL of a 0.416 M hypochlorous…

Q: How many moles of sodium hydroxide would have to be added to 150 mL of a 0.438 M acetic acid…

Q: An analytical chemist is titrating 152.0 mL of a 0.2100 M solution of benzoic acid (HC,H,CO,) with a…

A: Given: Concentration of HC6H5CO2 = 0.2100 M Volume of HC6H5CO2 = 152.0 mL Concentration of NaOH =…

Q: Determine the pH during the titration of 16.5 mL of 0.378 M hydrobromic acid by 0.524 M potassium…

A: Given : Concentration of hydrobromic acid (HBr) solution = 0.378 M Volume of hydrobromic acid…

Q: arterial blood plasma is buffered by the carbonic acid and bicarbonate ion, with a ratio of 1:20.…

A: Given: Ka of acid = 7.9 x 10-7 Concentration of carbonic acid = 0.1 M Ratio of carbonic acid and…

Q: What mass of NH4Cl must be added to 0.750 L of a 0.100-M solution of NH3 to give a buffer solution…

A: Interpretation - To determine the mass of NH4Cl when it must be added to 0.750 L of a 0.100-M…

Q: Ammonia is a convenient buffer system in the slightly basic range. (a) What is the pH of a buffer…

A: pH is defined as the negative logarithm of hydrogen ion concentration. It can be given as pH=-log…

Q: An aqueous solution contains 0.494 M ethylamine (C2H5NH2). How many mL of 0.206 M hydroiodic acid…

A: Given data,Molarity of ethylamine=0.494MMolarity of HI=0.206MVolume of buffer=225mL=0.225LpH=10.6…

Q: A buffer solution contains 0.345 M NaHSO3 and 0.430 M Na,SO3. If 0.0273 moles of perchloric acid are…

A: We will use buffer equation

Q: You want to prepare a buffer solution with pH equal to 3. How many grams of NaF (41.99 g/mol) should…

A: In this, we need to find oute moles of NaF first. Using that moles and molar mass for NaF, calculate…

Q: 8. What happens if a large amount of a strong acid or base is added to a buffer? Explain. ( C2)

A: In this question, we will explaining you what happened when we adding larger amount of acid or base…

Q: 1. Which of the following aqueous solutions are good buffer systems? . 0.35 M ammonia + 0.31 M…

A: Hi, we are supposed to answer one question. To get the remaining questions solved please mention…

Q: a) A chemist prepares a buffer solution by mixing 60.0 mL of 0.150 M NHs and 50.0 mL of 0.100 M…

Q: If 5.00g NH4Cl(s) is dissolved in 0.250M NH3, what volume of NH3 (in mL) is required to make a…

Q: 2. Which of the following mixtures (check the box) would result in a buffered solution when 1.0 L of…

A: Buffer solution is a solution who resist to change in pH. Buffer solution are of two type acidic…

Q: Please don't provide handwritten solution ...

A: The objective of this question is to determine the volume of 0.237 M perchloric acid that needs to…

Q: How many moles of potassium hydroxide would have to be added to 225 mL of a 0.478 M acetic acid…

A: Here KOH was added in acetic acid. pKa of acetic acid is 4.75 Now, 225mL 0.478M CH3COOH =…

Q: 20.3 mL of 0.144 M solution of nitric acid is titrated with 0.106 M NaOH solution. What is the pH…

A: Answer:pH tells about the strength of hydronium ion concentration in a solution and its value is…

Q: 11. Buffer X contains 8.0 mmol of NH3 and 8.0 mmol of NH. Buffer Y contains 20.0 mmol of NH3 and…

A: Given:Moles of Buffer X (NH3) = 8.0 mmol.Moles of Buffer X (NH4+) = 8.0 mmol.Moles of Buffer Y (NH3)…

Q: 6. Calculate the pH of the resulting solution when 20.0 ml of 0.25 M HCI is added with 20.1 ml of…

A: Using formula mixing of solutions:- Mmix.=M1V1+M2V2/V1+V2 After calculating [H+]=Mmix. Then use…

Q: How many milliters of 1.0 M NaOH must be added to a 200 mL of 0.10 M NaH2PO4 to make a buffer…

A: Given pH of the solution = 7.5 Volume of NaH2PO4 taken = 200.0 ml Molarity of NaH2PO4 taken = 0.10…

Q: How many milliliters of 1.92 M NaOH must be added to 275 mL of 0.11 M NaH 2PO4 to make a buffer…

A: Given:Find the volume of NaOH solution,A buffer solution is one that maintains its pH fairly…

Q: An aqueous solution contains 0.413 M hydrocyanic acid. How many mL of 0.319 M potassium hydroxide…

Q: A buffer solution was made by adding 9.35 mL of 0.50 M acetic acid and 0.628 g sodium acetate with…

Q: Calculate the pH of the buffer system made up of 0.15 M NH3NH3/0.35 M NH4ClNH4Cl.

A: The Henderson hasselbalch equation for calculation of pH of a buffer is pH = pKa + log[base][acid]…

Q: If 0.50 mL of 0.087 M HCl is added to the solution in (a), how many moles of the acetic acid, sodium…

A: Here we are required to find the percent change in pH of the buffer when acid is added.

Q: A buffer is made by adding 19.4 grams of lithium fluoride

A: 1. Moles of LiF (salt) : n = W/ M = 19.4 g/25.94 g/mol = 0.75 mol…

Q: An aqueous solution contains 0.329 M methylamine (CH3NH2). How many mL of 0.305 M perchloric acid…

Q: You want to prepare a buffer solution with pH equal to 3. How many grams of NaF (41.99 g/mol) should…

A: pH of a buffer solution is equals to 3. Volume of HF = 250 mLConcentration of HF = 0.350 MWe have to…

Q: How many moles of sodium hydroxide would have to be added to 125 mL of a 0.376 M hydrocyanic acid…

A: Ka of HCN = 6.2 × 10-10 pka = -log(ka) = 9.2

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

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: Determine the mass of ammonium chloride required to produce buffer solution from the given data:

VIEW

Step 2: Calculation for mass of ammonium chloride required to produce buffer solution:

VIEW

Solution

VIEW

Step by step

Solved in 3 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

You need to prepare a pH = 9.20 buffer solution containing NH3 and NH4Cl. If you start with 0.71 M NH4Cl solution, what concentration of NH3 l will you need to also start with? (Kb for NH3 is 1.8x10-5)
There are 0.250 ml of a Buffer solution, where the concentration is 0.225 M of sodium acetate and 0.225 M of acetic acid. What will the change in pH be if 30 ml of a 0.1 M HCl solution are added?
How many milliliters of 1.05 M NaOH must be added to 125 mL of 0.15 M NaH2PO4 to make a buffer solution with a pH of 6.30?
What [NH3] needs to be added to 0.0010M NH4Cl to obtain a buffer solution with pH of a 7.3?
3. A buffer solution contains 0.125 moles of ammonium chloride added to 500.0 ml of 0.500 M solution of ammonia. A) What is the pH of this buffer? B) What is the pH after the addition of 0.0100 moles of HCI bubbled into 500.0 mL of the buffer?
1. The pH of a buffer solution containing 0.5 mole/litre of CH:COOH and 0.5 mole/litre CH:COON has been found to be 4.76. What will be the pH of this solution after 0.1 mole/litre HCI has been added to the buffer? Assume that the volume is unchanged. Ka = 1.75 x 105 2. A litre of solution containing 0.1 mole of CH;COOH and 0.1 mole of CH;COON provides a buffer of pH 4.74. Calculate the pH of solution after the addition of 0.02 mole NaOH. Ka = 1.8 x 105.
How many moles of sodium hydroxide would have to be added to 225 mL of a 0.349 M nitrous acid solution, in order to prepare a buffer with a pH of 3.570? moles
How many grams of dry NH4Cl need to be added to 2.50 L of a 0.300 M solution of ammonia, NH3 , to prepare a buffer solution that has a pH of 8.74? Kb for ammonia is 1.8×10−5 . (Please type answer no write by hend)
8b.
7. A solution was made by mixing 50.0 mL of 0.750 M HCN with 25.0 mL of water. What is the pH of this solution? The pka of HCN = 9.31. 8. One of the compounds featured on the TV series "Breaking Bad" was hydrofluoric acid (HF), pKa = 3.14. a) A solution of HF has a pH = 1.77. What was the initial [HF] for this solution in mol L-1? b) What is the equilibrium concentration of F in this solution in mol L-1? c) What is the percent ionization of HF in this solution?
An aqueous solution contains 0.386 M dimethylamine ((CH3)2NH).How many mL of 0.379 M perchloric acid would have to be added to 250 mL of this solution in order to prepare a buffer with a pH of 10.800.
What is the pH of a buffer made by dissolving 0.2 mol of KBrO and 0.6 mol of HBrO in 850 mL of solution? What is the pH if the solution is diluted to 2 L?