**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: How many moles of potassium hydroxide would have to be added to 150 mL of a 0.477 M hydrofluoric…

A: Given: V=150mL;[HF]=0.477;pH=3.150;Ka=6.3x10−4The value in this question may have been different…

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: A buffer solution contains 0.294 M nitrous acid and 0.416 M potassium nitrite. If 0.0246 moles of…

A: Given- Concentration of nitric acid =0.294M Concentration of potassium nitrite =0.416M Moles of…

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

Q: you wish to prepare a pH=3.00 buffer solution using HF and NaF. what mass of NaF (s) would you need…

A: HF is a weak acid with pKa = 3.14 NaF or F- (aq) is the conjugate base of HF. Desired pH of the…

Q: A student was required to prepare 250.0 mL of a hypochlorous acid/sodium hypochlorite buffer in…

Q: A buffer solution contains 0.340 M ammonium chloride and 0.203 M ammonia. If 0.0488 moles of sodium…

A: To calculate the pH of the buffer solution after adding NaOH solution , we would first calculate the…

Q: How many grams of solid ammonium bromide should be added to 1.50 L of a 0.0879 M ammonia solution to…

A: The objective of this question is to determine the amount of solid ammonium bromide that needs to be…

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: Ammonia is a weak base and form a buffer solution with NH4Cl The pH of buffer is close to 9-10.…

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

Q: An aqueous solution contains 0.415 M dimethylamine ((CH3)2NH). How many mL of 0.274 M perchloric…

A: An aqueous solution of 0.415 M dimethylamine (CH3)2NH0.274 M perchloric acidpH = 10.6Volume = 150 ml

Q: An aqueous solution contains 0.318 M dimethylamine ((CH3)2NH). How many mL of 0.209 M nitric 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: 6. How many grams of KOH must be added to 500.0 mL of 2.0 M CH3COOH to prepare a 30 [1] sri…

Q: An aqueous solution contains 0.348 M nitrous acid. How many mL of 0.236 M sodium hydroxide would…

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: How many moles of sodium hydroxide would have to be added to 225 mL of a 0.316 M acetic acid…

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: How many moles of sodium hydroxide would have to be added to 125 mL of a 0.339 M hypochlorous acid…

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

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 buffer solution contains 0.302 M NaHSO3 and 0.438 M K2SO3. If 0.0168 moles of hydrochloric acid…

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

Q: You are titrating 20.0mL sample of 0.131 M Ba(OH)2 with 0.350 M HCL. (a) What volume in mL of…

A: Answer -

Q: How many grams of dry NH4Cl nned to be added to 2.50 L of a 0.200 M solution of ammonia, NH3, to…

Q: An aqueous solution contains 0.30 M ammonium bromide. One liter of this solution could be converted…

A: Given-> Molarity of NH4Br = 0.30 M Volume = 1 L

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: A buffer solution contains 0.235 M ammonium bromide and 0.314 M ammonia. If 0.0164 moles of…

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: You have a 0.10 M aqueous NH3 solution. Calculate a) the number of moles b) the number of grams of…

A: H-H equation can be used to pH determination as, pOH = pKb + log [moles of conjugate acid] / [moles…

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: 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 solution contains 0.361 M nitrous acid and 0.244 M sodium nitrite. If 0.0185 moles of…

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

Q: You need to prepare a pH = 9.20 buffer solution containing NH3 and NH4Cl. If you start with 0.71 M…

A: NH3 and NH4Cl form a basic buffer . We know that pH + pOH =14

Q: How many grams of solid ammonium bromide should be added to 1.50 L of a 6.42x102 M ammonia solution…

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

A buffer solution contains 0.219 M ammonium bromide and 0.312 M ammonia. If 0.0603 moles of perchloric acid are added to 250 mL of this buffer, what is the pH of the resulting solution ? (Assume that the volume does not change upon adding perchloric acid) pH =
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?
How many moles of potassium hydroxide would have to be added to 125 mL of a 0.438 M hydrocyanic acid solution, in order to prepare a buffer with a pH of 9.090? moles
ions A buffer solution contains 0.342 M sodium hydrogen sulfite and 0.216 M sodium sulfite. If 0.0445 moles of sodium hydroxide are added to 250 ml of this buffer, what is the pH of the resulting solution? (Assume that the volume does not change upon adding sodium hydroxide). pH =
A buffer solution contains 0.228 M ammonium chloride and 0.315 M ammonia. If 0.0274 moles of nitric acid are added to 125 mL of this buffer, what is the pH of the resulting solution ? (Assume that the volume change does not change upon adding nitric acid) pH
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?
10a.
8b.
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?
8.) The buffer solution, in addition of small amount of strong acid or strong base will change the pH. True or False