How many grams of dry NH,Cl need to be added to 2.00 L of a 0.800 M solution of ammonia, NH3, to prepare a buffer solution that has a pH of 8.64? K, for ammonia is 1.8 x 10-5. Express your answer with the appropriate units.

How many grams of dry NH,Cl need to be added to 2.00 L of a 0.800 M solution of ammonia, NH3, to prepare a buffer solution that has a pH of 8.64? K, for ammonia is 1.8 x 10-5. Express your answer with the appropriate units.

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 8ALQ: You have a solution of the weak acid HA and add some of the salt NaA to it. What are the major...

See similar textbooks

Related questions

Q: Why the concentrations of buffer components must be high to minimize the change in pH from addition…

A: A buffer solution or pH buffer is an aqueous solution consisting of a mixture of a weak acid and…

Q: 3.28 g of sodium acetate (82 g/mol) added to 400 mL of acetic acid to produce a buffer solution that…

A: Moles of sodium acetate = mass/molar mass = 3.28/82 = 0.04 mol Let molarity of acetic acid = M…

Q: A 1.34 L buffer solution consists of 0.174 M butanoic acid and 0.250 M sodium butanoate. Calculate…

A: The pH scale is given by the scientist Sorensen in order to express the [H3O+] ion of a solution. It…

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…

A: Initial concentration of base is equal to final concentration of salt because base must be limiting…

Q: How do you use the Henderson–Hasselbalch equation to calculate the pH of a buffer containing a base…

A: Henderson–Hasselbalch equation is a relation between pH of acid and pKa (dissociation constant). For…

Q: A chemistry graduate student is given 300. mL of a 1.30M diethylamine ((C,H5), NH) solution.…

Q: A buffer is made by dissolving 10.5 g of sodium dihydrogen phosphate, NaH2PO4 and 12.0 g disodium…

Q: How many grams of dry NH4Cl need to be added to 2.40 L of a 0.800 M solution of ammonia to prepare a…

Q: Calculate the pH of a buffer that was prepared by mixing 90 mL of a 0.01M aqueous hydrocyanic acid…

A: HCN is a weak acid. In presence of base it produces it's conjugate base and form buffer solution.…

Q: Consider a buffer made by adding 132.8 g of NaC₇H₅O₂ to 300.0 mL of 1.09 M HC₇H₅O₂ (Ka = 6.3 x 10⁻⁵)…

Q: At 25 degrees Celsius, what is the pH of a buffer that contains 0.100 M dimethylammonium chloride…

A: dimethyl amine has pKa = 3.27

Q: At 25oC, a 1-L buffer solution is prepared by mixing acetic acid and sodium acetate. A) If the…

A: Use Henderson Hesselbalch's equation to get the pH of buffer solution having weak acid and its salt…

Q: Define the following terms: titration equivalence point buffer point molarity What instrument are…

A: 1. Titration = It is a laboratory method of quantitative chemical analysis in which the solution of…

Q: How many grams of hydrofluoric acid, HF, should you add to a 1.65 L of a 2.65 M sodium fluoride…

A: Given: pH = 3.45 pKa = 7.1 x 10-4 Volume, V (NaF) = 1.65 L Molarity, M (NaF) = 2.65 M The strong…

Q: A chemistry graduate student Is glven 100. mL of a 0.70M trimethylamine ((CH,) N solution.…

Q: A chemistry graduate student is given 125. mL of a 1.50M diethylamine ((C,H, NH solution.…

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

Q: 1. Acetate buffers are used in biochemical studies of enzymes and other chemical components of cells…

A: The Ka value of acetic acid is 1.8 × 10-5.pKa = -log(Ka) = -log(1.8 × 10-5) = 4.74.concentration of…

Q: A buffer is prepared by adding 2.50g of lithium fluoride to 125 mL of 0.648M hydrofluoric acid. You…

A: Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: Consider the titration of a 40.0 mL of 0.189 M weak acid HA (Ka = 2.7 x 10⁻⁸) with 0.100 M LiOH. a.…

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

Q: A chemistry graduate student is given 100. mL of a 0.50 M pyridine (CH,N) solution. Pyridine is a…

Q: 3.28 g of sodium acetate (82 g/mol) added to 400 mL of acetic acid to produce a buffer solution that…

A: Given 3.28 g of sodium acetate added to 400 ml of acetic acid to make buffer of pH =5 and pKa of…

Q: What is the pH of a buffer that contains 0.15 M CH3COOH and 0.10 M NaCH3COO (K, = 1.8 x 10$)?

A: Given : Concentration of weak acid CH3COOH = 0.15 M And concentration of conjugate base salt of weak…

Q: Calculate the pH of a buffer solution made from 1.000 g of sodium chlorate NaClO3 and 0.9561 g of…

A: Write the expression for pH. pH = pKa + log[salt][acid] Here, pKa is the negative logarithm of acid…

Q: Consider a buffer made by adding 43.1 g of (CH:):NH21 to 250.0 mL of 1.42 M (CH.):NH (Kb = 5.4 x…

Q: 3. (6)What is the pH of a buffer that is 0.12M lactic acid (HC3H5O3) and 0.1OM sodium lactate? Ka=…

Q: butter solution: 600.0 ml 0.550 M CHCOOH 0.325 M NACH,COO K1.76 x 10 Determine the pH of the…

Q: Tris(hydroxymethyl)aminomethane is a common base used to prepare buffers in biochemistry. Its Kb is…

Q: How much sodium formate (HCOONA, 68.0069 g/mol) do you need to add to 400. ml of 1.00 M formic acid,…

A: Molarity of formic acid = 1.00 M pH of buffer = 3.500 Volume of buffer = 400 mL = 400 × 10-3 L Ka =…

Q: Consider a buffer made by adding 132.8 g of NaC₇H₅O₂ to 300.0 mL of 1.09 M HC₇H₅O₂ (Ka = 6.3 x 10⁻⁵)…

Q: 1. What is the pH of a buffer that contains 0.15 M CH,COOH and 0.10 M NACH,COO (K, = 1.8 x 10 )?

A: 1) Given, Concentration of CH3COOH solution = 0.15 M [CH3COOH] = 0.15 M Concentration of NaCH3COO…

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: Determine the mass (in grams) of sodium formate that must be added to 1.00 L of 0.180 M formic acid…

A: Buffer is the solution of mixture of weak acid/weak base with its salt of strong base/strong acid

Q: A chemistry graduate student is given 250. mL of a 0.30M chloroacetic acid (HCH,CICO,) solution.…

A: We have to calculate the mass of salt added.

Q: suitable

A: Buffer solution worked at pH = pKa-1 to pKa +1 Here pH = 7.0 then range should be 6 to 8 at this…

Q: : Calculate the pH of the following acid-base buffers. 100 mL of 0.025 M formic acid and 0.015 M…

A: A buffer solution is prepared. When a strong base is added into a weak acid solution, then the…

Q: a)What is the pH of a mixture of 0.042 M NaH2PO4 and 0.058 M Na2HPO4? (b) If 1.0 mL of 10.0 M NaOH…

A: Molarity of NaH2PO4 = 0.042 M Molarity of Na2HPO4 = 0.058 M

Q: -4 What A chemistry graduate student is given 100. mL of a 1.10 M trimethylamine ((CH,) N) solution.…

A: From the buffer solution of (CH3)3N and (CH3)3NHBr: [Salt]: Salt concentration. [base]: base…

Q: A buffer solution that is made with equal volumes of 2.5M citric acid and 0.5M sodium citrate? The…

A: The volumes of citric acid and sodium citrate are equal. Ka of citric acid = 8.4 x 10-4 The…

Q: A 1.43 L buffer solution consists of 0.179 M butanoic acid and 0.300 M sodium butanoate. Calculate…

A: The pH of an acidic buffer can be calculated by using Henderson equation pH = pka + log10…

Q: A chemistry graduate student is given 450. mL of a 0.50M methylamine (CH,NH,) solution. Methylamine…

Q: A chemistry graduate student is given 125. mL of a 1.30M dimethylamine ((CH,) NH) solution.…

A: Buffer solution: It is a special type of mixture of a weak acid or a weak base and its conjugate…

Q: A chemistry graduate student is given 300. mL of a 0.80 M methylamine (CH, NH,) solution.…

A: Given: Volume of solution = 300 mLMolarity of CH3NH2 = 0.80 MpH of solution = 10.92Kb of CH3NH2 =…

Q: What mass of A chemistry graduate student is given 125. mL of a 1.30 M acetic acid (HCH,CO,)…

A: Handerson Hasselbalch equation – Buffer solution is mixture of weak acid and its conjugate base.…

Q: A chemistry graduate student is given 100. mL of a 0.50M methylamine (CH,NH,) solution. Methylamine…

Q: A chemistry graduate student is given 250. mL of a 1.40M trimethylamine ((CH,) N) solution.…

Q: Consider a buffer made by adding 42.3 g of (CH3)2NH2I to 250.0 mL of 1.42 M (CH:)»NH (Kb = 5.4 x 10…

A: pH is a scale which is used to determine the acidity or basicity of a solution. pH = pKa + log…

Q: Acid Ka HF 6.7 x 10^-4 HC2H3O2 1.8 x 10^-5 A student…

A: At equivalence point, the number of moles of acetic acid will be equal to that of NaOH and whole…

Q: A chemistry graduate student is given 100. mL of a 1.30M dimethylamine ((CH3), NH solution.…

A: Mass of (CH3)2NH2Br is to be determine

Q: A chemistry graduate student is given 125. mL of a 1.00 M methylamine (CH ,NH,) solution.…

A: Given : concentration of (CH3)3N = 1.00 M volume of (CH3)3N solution = 125 mL = 0.125 L…

Q: How many grams of dry NHạ Cl need to be added to 2.00 L of a 0.100 M solution of ammonia, NHa, to…

A: In this question, we have to find out the correct answer of given problem by the help of the…

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

100%

How many grams of dry NH,Cl need to be added to 2.00
L of a 0.800 M solution of ammonia, NH3, to prepare a
buffer solution that has a pH of 8.64? Kµ for ammonia is
1.8 x 10-5.
Express your answer with the appropriate units.

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

Answer

Trending now

This is a popular solution!

Step by step

Solved in 5 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

Calculate the pH of a solution prepared by mixing 49.0 mL of butyric acid, HC4H7O2, with 6.15 g of KOH in water. The following data about butyric acid may be helpful: density=0.9595g/mL;K a =1.54105
Sketch a titration curve for the titration of potassium hydroxide with HCl, both 0.100 M. Identify three regions in which a particular chemical species or system dominates the acid-base equilibria.
Consider all acid-base indicators discussed in this chapter. Which of these indicators would be suitable for the titration of each of these? (a) NaOH with HClO4 (b) acetic acid with KOH (c) NH3 solution with HBr (d) KOH with HNO3 Explain your choices.
Estimate the pH that results when the following two solutions are mixed. a) 50 mL of 0.3 M CH3COOH and 50 mL of 0.4 M KOH b) 100 mL of 0.3 M CH3COOH and 50 mL of 0.4 M NaOH c) 150 mL of 0.3 M CH3COOH and 100 mL of 0.3 M Ba(OH)2 d) 200 mL of 0.3 M CH3COOH and 100 mL of 0.3 M Ba(OH)2
You have a solution of the weak acid HA and add some of the salt NaA to it. What are the major species in the solution? What do you need to know to calculate the pH of the solution, and how would you use this information? How does the pH of the solution of just the HA compare with that of the final mixture? Explain.
Calculate the pH of a solution made by dissolving 1.87g of sodium caproate (NaC6H11O2) in water and diluting it toa total volume of 500mL. For the caproate ion, Kb=7.58 x 10^-10
What is the pH of a solution prepared by combining 0.258 mol of a newly discovered weak acid (Ka = 1.3 x 10-4) with 0.156 mol of the salt containing its conjugate base in 1.4 L of water?
Calculate the pH of a solution that is composed of 90.0 mL of 0.345 M sodium hydroxide, NaOH, and50.0 mL of 0.123 M lactic acid, HC3H5O3. (Ka of lactic acid = 1.38x10-4)
A tablet of a common over-the-counter drug contains 200 mg of caffeine (C8H10N4O2). What is the pH of the solution resulting from the dissolution of two of these tablets in 225 mL of water? (For caffeine, Kb = 4.1 x 10–4.)
Determine the base ionization constant (in x 10^5) of a 0.0925 g sample of week base (molar mass = 17.03 g/mol), B, that is dissolved in water to produce 100 mL of a solution with a pH of 11.00.
1. The ionization constant (Kb) of pyridine (C5H5N) is 5.62 x 10–4. If 11.3 grams of sample of pyridine is dissolved in 250.0 mL of water, what are the equilibrium concentration of all species present?2. A certain acidic vitamin is essential for all mammals since it plays a role in mineral absorption. A 0.125 M solution of this acid is found to have a pH of 2.034. Based on the table below, what most likely is the identity of this unknown acid? (Note: For this problem, treat the acid as if it is a monoprotic acid.)
A solution of volume 0.500 L contains 1.68 g NH3 (Kb = 1.8 x 10^-5) and 4.05 g (NH4)2SO4. How many milliliters of 12 M HCI must be added to 0.500 K of the original solution to change its pH to 9.00?