The problem given involves calculating the number of moles of NaX needed to make a buffer solution using the Henderson-Hasselbalch equation. Here's the transcription for educational purposes:---**Buffer Solution Calculation**The \( K_a \) for the acid HX is \( 2.714 \times 10^{-5} \). How many moles of NaX need to be mixed with 2.586 L of 0.152 M HX to make a buffer with a pH of 4.922? Use the Henderson-Hasselbalch equation.--- **Note:** The Henderson-Hasselbalch equation is given by:\[\text{pH} = \text{pKa} + \log\left(\frac{[\text{A}^-]}{[\text{HA}]}\right)\]Where:- \([\text{A}^-]\) is the concentration of the conjugate base (NaX in this case).- \([\text{HA}]\) is the concentration of the acid (HX).- \(\text{pKa}\) is calculated from the \( K_a \) value: \(\text{pKa} = -\log(K_a)\).The problem involves calculating the concentration of NaX needed to achieve the desired pH.

We will first determine the moles of acid. we know pKa= -logka,we will make use of equation-

Answered: The K₂ for the acid HX is 2.714. 10-5.…

The K₂ for the acid HX is 2.714. 10-5. How many moles of Nax need to be mixed with 2.586 L of 0.152 M HX to make a buffer with a pH of 4.922? Use the Henderson Hasselbalch equation.

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: How many grams of solid ammonium chloride should be added to 1.50 L of a 0.204 M ammonia solution to…

A: The objective of this question is to determine the amount of solid ammonium chloride (NH4Cl) that…

Q: How many moles of NaOH need to be added to 200.0 mL of a 0.200 M solution of HF to make a buffer…

A: Introduction: We have to calculate number of moles of NaOH . Given : pH = 3.70 Ka= 6.8 × 10-4

Q: How many moles of sodium hydroxide would have to be added to 125 mL of a 0.409 M hydrocyanic acid…

Q: A buffer is 0.100 M in NH4CI and 0.100 M in NH3. When a small amount of hydrobromic acid is added to…

Q: How many grams of solid ammonium chloride should be added to 2.00 L of a 0.221 M ammonia solution to…

Q: What quantity in moles of HCI need to be added to 200.0 mL of a 0.200 M solution of NaF to make a…

A: Given:pH of buffer solution = 3.00Ka for HF = 6.8×10−4 The pKa for HF is calculated as:pKa=−logKa…

Q: Mixing 10 mL 1 M NH4Cl with 10 mL 1 M NH3 Why is this an effective buffer? Please provide the…

A: Buffer is the one which can be formed by the weak acid and its conjugate base or weak base and its…

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: Calculate the mass of C5H5NHCI (molar mass = 113.56 g/mol) that must be added to 0.80 L of 2.5 M…

A: Given, Kb of C5H5N( weak base) is 1.8 X 10-9Therefore, pKb = - log(Kb) =…

Q: You need to prepare 100.0 mL of a pH 4.00 buffer solution using 0.100 M benzoic acid (p?a=4.20) and…

A: Let y mL benzoic acid and (100 – y) mL sodium benzoate are mixed. For acidic buffer solution, pH =…

Q: How many moles of NaOH need to be added to 200.0 mL of a 0.200 M solution of HF to make a buffer…

Q: O adding 0.060 moles of HOCI

A: I Buffer are solution that contain a buffer pair of either a weak acid and a salt of its…

Q: What quantity in moles of NaOH need to be added to 200.0 mL of a 0.200 M solution of HF to make a…

Q: A buffer solution contains 1.7 M acetic acid and 2.6 M sodium acetate. The Ka of the acetic acid is…

A: Calculation of pKa of acetic acid: pKa=-log Ka=-log (1.8×10-5)=4.745

Q: How many grams of solid ammonium chloride should be added to 0.500 L of a 5.30×10-2 M ammonia…

A: This problem can be solved by using Handersen-Hasselbalch equation for weak base.

Q: A buffer is made by mixed 0.2 M HAc and 0.1 M of NaAc the pH of the solution has been adjusted to…

A: The given question involves the calculation of the amount of NaOH needed to adjust the pH of a…

Q: 2. Phenol (C6H5OH) has a Ka of 1.6*10-10. Starting with a 100.0 mL solution that is 0.300 M phenol,…

A: Given that : Volume of C6H5OH=100mLIts concentration=0.300 MpH = 10Ka of C6H5OH=1.6×10-10So,…

Q: How many grams of solid ammonium chloride should be added to 1.00 L of a 0.243 M ammonia solution to…

Q: How many grams of solid ammonium chloride should be added to 2.00 L of a 0.172 M ammonia solution to…

A: It will form a basic buffer. And pkb for NH3 = 4.74 Molar mass of Ammonium chloride is 53.49 g/mol

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: buffer is made up of 0.3 L each of a 0.5 M KH2PO4 and 0.317 M K2HPO4. assuming that volumes are…

A: #(a): The dissociation equation for the weak acid conjugate base pair is: H2PO4-(aq) ⇌HPO42-(aq),…

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

Q: How many grams of solid potassium hypochlorite should be added to 0.500 L of a 0.189 M hypochlorous…

A: Note: Dear student since you have posted multiple questions we will solve only first question for…

Q: A buffer is prepared by mixing 43.9 g of NH3 and 43.9 g of NH4Cl in 0.548 L of solution. What is the…

Q: What quantity in moles of HCl need to be added to 200.0 mL of a 0.200 M solution of NaF to make a…

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 g of sodium nitrate (NaNO2, 100% ionized in water) do you need to add to 4.00L of 0.500M…

Q: 0.50 M solutions of each weak acid in the table are available. Choose an acid solution and determine…

A: According to Henderson-Hasselbalch equation, pH=pKa+log[conjugate acid][base]

Q: What quantity in moles of HCl need to be added to 200.0 mL of a 0.200 M solution of NaF to make a…

A: Buffer solution made of a mixture of weak acid and its conjugate base salt in aqueous…

Q: Suppose there is 1.00 L of an aqueous buffer containing 60.0 mmol of acetic acid (p?a=4.76) and 40.0…

Q: What quantity in moles of HCI need to be added to 200.0 mL of a 0.200 M solution of NaF to make a…

Q: A buffer solution contains 0.285 M hydrofluoric acid and 0.326 M potassium fluoride. If 0.0252…

A: Given, The molarity of Hydrofluoric acid = 0.285 M The molarity of Potassium fluoride = 0.326 M.…

Concept explainers

Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.

Question

The problem given involves calculating the number of moles of NaX needed to make a buffer solution using the Henderson-Hasselbalch equation. Here's the transcription for educational purposes:

---

**Buffer Solution Calculation**

The \( K_a \) for the acid HX is \( 2.714 \times 10^{-5} \). How many moles of NaX need to be mixed with 2.586 L of 0.152 M HX to make a buffer with a pH of 4.922?

Use the Henderson-Hasselbalch equation.

---

**Note:** The Henderson-Hasselbalch equation is given by:

\[
\text{pH} = \text{pKa} + \log\left(\frac{[\text{A}^-]}{[\text{HA}]}\right)
\]

Where:
- \([\text{A}^-]\) is the concentration of the conjugate base (NaX in this case).
- \([\text{HA}]\) is the concentration of the acid (HX).
- \(\text{pKa}\) is calculated from the \( K_a \) value: \(\text{pKa} = -\log(K_a)\).

The problem involves calculating the concentration of NaX needed to achieve the desired pH.

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 3

VIEW

Step by step

Solved in 3 steps with 2 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

How many grams of solid ammonium bromide should be added to 2.00 L of a 0.132 M ammonia solution to prepare a buffer with a pH of 8.330 ? grams ammonium bromide = -- How many grams of solid potassium cyanide should be added to 1.00 L of a 0.281 M hydrocyanic acid solution to prepare a buffer with a pH of 8.558 ?grams potassium cyanide = g.
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 is 1.76 x 10-5.
How many grams of sodium formate, HCOONa, are required to mix with 1.50 Liters of 0.500 M formic acid, HCOOH, in order to prepare a buffer solution with a pH that equals 4.00? pKa(HCOOH) = 3.74 and MM(HCOONa) = 52.01 g/mol
How many moles of NaOH need to be added to 200.0 mL of a 0.200 M solution of HF to make a buffer with a pH of 3.40? (Ka for HF is 6.8 × 10⁻⁴)
Help needed please
2. A buffer solution contains 0.15 mol of propionic acid (HC3H5O2) and 0.10 mol of sodium propionate (NaC3H5O2) in 1.20 L of the solution. What is the pH of the buffer after the addition of 0.01 mol of NaOH?
What quantity in moles of NaOH need to be added to 200.0 mL of a 0.200 M solution of HF to make a buffer with a pH of 3.10? (Ka for HF is 6.8 × 10⁻⁴)
How many grams of solid ammonium chloride should be added to 2.00 L of a 0.203 M ammonia solution to prepare a buffer with a pH of 8.480 ? grams ammonium chloride = g.