Answered: Determine the mass of sodium formate…

Determine the mass of sodium formate that must be dissolved in 250.0 cm3> of a 1.4 M solution of formic acid to prepare a buffer solution with pH = 3.36.

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter21: Potentiometry

Section: Chapter Questions

Problem 21.22QAP

See similar textbooks

Related questions

Q: You add 5.00 mL of 0.100 M NaOH to 25.00 mL of pure water, and to this mixture you then add 10.00 mL…

Q: A buffer solution contains 0.239 M acetic acid and 0.420 M potasslum acetate. If 0.0243 moles of…

Q: When 40 mL of benzoic acid (C.HSCOOH) and 35 mL of potassium hydroxide were titrated, the pH at the…

A: At equivalence point salt potassium benzoate is formed in which C6H5COO- undergoes hydrolysis.…

Q: For a weak acid (CH3COOH) that is titrated with a strong base (NaOH), what species (ions/ molecules)…

A: The stoichiometric point is also known as the equivalence point. It is the point when the complete…

Q: How many moles of CH₃NH₃Cl need to be added to 200.0 mL of a 0.500 M solution of CH₃NH₂ (Kb for…

A: We have given that pH = 10.80 and we know that pH + pOH = 14 So pOH = 14-…

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

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: how many grams of NH4Cl must be added to 1 liter of 1.0 M NH4OH solution to prepare a buffer…

Q: A buffer solution contains 0.371 Mhydrocyanic acid and 0.449 M potassium cyanide. If 0.0218 moles of…

A: pH = pKa + log[salt]/[acid]

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: Calculate the volume of concentrated ammonia and the weight of ammonium chloride you would have to…

A: we have to prepare 175 ml of 0.40 M of NH4Cl : mili moles NH4Cl = 0.4m.mole/ml x 175ml = 70 m.moles…

Q: A solution was found to have a PH of 6.3 with the acid 100x in excess of it conjugate base. What is…

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

Q: An aqueous solution contains 0.464 M hypochlorous acid.How many mL of 0.364 M sodium hydroxide would…

A: The reaction between the sodium hydroxide and hypochlorous acid as shown below. At standard…

Q: How many moles of CH₃NH₃Cl need to be added to 200.0 mL of a 0.500 M solution of CH₃NH₂ (Kb for…

A: First calculate mole of primary amine use basic buffer equation PH+poh=14 Mole of C13NH2C1= xMole of…

Q: 50.00 mL of 0.200 M sodium dihydrogen pyrophosphate (N22H2P207) solution is combined with 25.00 mL…

A: Buffer solution is prepared, when an strong base is added into weak acid solution then resulting…

Q: A 1.46 L buffer solution consists of 0.171 M butanoic acid and 0.341 M sodium butanoate. Calculate…

A: Given, Volume of the buffer = 1.46 L Molarity of butanoic acid = [Butanoic acid] = 0.171 M…

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

Q: An aqueous solution contains 0.464 M hypochlorous acid.How many mL of 0.364 M sodium hydroxide would…

A: The reaction as follows,

Q: The addition of an acidic solution to a buffer solution with a pH of 8.3 would most likely result in…

Q: When 42.6 mL of 0.100 M Ba(OH)2 is mixed with 98.6 mL of 0.200 M HCI, the reaction goes to…

A: A numerical problem based on pH concept, which is to be accomplished.

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: If the acceptable buffer range of the solution is ±0.10 pH units, calculate how many moles of H3O+…

A: pH drop is 0.1 then initial pH = 9.6837 pH drop max = pH = 9.6837-0.1 = 9.5837…

Q: How many moles of NH4Cl must be added to 2.0 L of 0.10 M NH3 to form a buffer whose pH is 9.00?…

A: This problem can be solved by using Henderson Hasselbalch equation of pH according to which :…

Q: An aqueous solution contains 0.339 M nitrous acid. How many mL of 0.370 M sodium hydroxide would…

Q: If a buffer solution is 0.260 M in a weak base (Kb=8.4×10−5) and 0.480M in its conjugate acid, what…

Q: A buffer solution contains 0.476 M ammonium bromide and 0.339 M ammonia. If 0.0340 moles of…

Q: The pH of a buffer solution that is made by mixing 124 mL of 0.156 M of acetic acids (pls=4.74) with…

Q: A buffer solution contains 0.472 M hydrocyanic acid and 0.249 M sodium cyanide. If 0.0290 moles of…

Q: When 32.3 mL of 0.100 M Ba(OH)2 is mixed with 197.2 mL of 0.200 M HCl, the reaction goes to…

A: The reaction result in the formation of Barium chloride. The pH of a solution is the negative…

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: How many grams of dry NH4C1 need to be added to 2.50 L of a 0.800 M solution of ammonia, NH3 , to…

A: NH3 + NH4Cl forms a basic buffer. For a basic buffer: pOH = pKb + log c2/c1 pH + pOH = 14

Q: You have at your disposal an ample quantity of a solutionof 0.100 M HCl and 400 mL of a solution of…

A: Given: Concentration of HCl = 0.100 M Volume of NaCN solution = 400 mL = 0.400 L…

Q: A buffer solution contains 0.227 M ammonium chloride and 0.450 M ammonia. If 0.0418 moles of nitric…

A: A solution of ammonium chloride in ammonia is a buffer solution of a weak base and the salt of its…

Q: 100.0 mL 0.15 M aqueous HF (K₁ = 6.8 x 104) is mixed with 125.0 mL 0.23 M NaF. What is the pH of the…

Q: In what volume ratio should you mix 1.0 M solutions of NH4Cl and 1.0 M NH3 to produce a buffer…

Q: A buffer solution contains 0.405 M NAHSO3 and 0.332 M Na,SO3. If 0.0248 moles of potassium hydroxide…

A: Given data, Molarity of NaHSO3 =0.405M Molarity of Na2SO3 = 0.332M Volume of buffer = 150mL = 0.150L…

Q: What volume of 0.200 M HCl must be added to 250.0 mL of 0.300 M sodium mandelate to produce a buffer…

A: An acidic substance is the substance that can give H+ ions. They are corrosive and sour in nature.…

Q: A buffer was prepared by mixing exactly 200 mL of a 0.60 M NH3 solution and 300 mL of a 0.30 M NH4Cl…

A: Given: Volume of NH3 solution = 200 mL Concentration of NH3 solution = 0.60 M Volume of NH4Cl…

Q: How many moles of CH₃NH₃Cl need to be added to 200.0 mL of a 0.500 M solution of CH₃NH₂ (Kb for…

A: Given, Volume of solution (v) = 200 mL = 0.2 L Molarity of Base (M) = 0.500 M Kb of base = 4.4×10⁻⁴…

Q: An aqueous solution contains 0.345 M dimethylamine ((CH3)2NH). How many mL of 0.370 M hydroiodic…

Q: An aqueous solution contains 0.443 M hypochlorous acid. How many mL of 0.213 M potassium hydroxide…

A: Given, [HClO] = 0.443 M [KOH] = 0.213 M Volume of the solution = 125 mL pH of buffer = 7.530…

Q: What volume of 0.500 M HNO2 should be added to 500 mL of 0.750 M KNO2, so that the pH of the…

Q: A buffer solution contains 0.268 M ammonium chloride and 0.311 M ammonia. If 0.0169 moles of…

A: Given -> Molarity of NH4Cl = 0.268 M Molarity of NH3 = 0.311M Moles of HI = 0.0169 mole Volume of…

Q: What mass of sodium acetate, NACH3 CO2 , must be added to 1.00 L of 0.080 M acetic acid to give…

Q: An aqueous solution contains 0.305 M methylamine (CH3NH2). How many mL of 0.365 M hydroiodic acid…

A: Interpretation- To determine the volume ( mL) of 0.365 M hydroiodic acid would have to be added to…

Q: Would a 0.010 M buffer solution or a 0.10 M buffer solution have a greater buffering capacity for…

A: Buffering capacity refers to the amount of added base or added acid that can be neutralized by a…

Q: Calculate the resulting pH when 1.00L of 1.00M H2SO4 is added to a tank containing 1.00*107 L of…

A: From the molarity: M: molarity in mole/Litre. n: number of moles. V: volume in Litre.

Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

Determine the mass of sodium formate that must be dissolved in 250.0 cm³> of a 1.4 M solution of formic acid to prepare a buffer solution with pH = 3.36.

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

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 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

Calculate the molar solubility of BaCrO4 Barium Chromate at: • Water • 0.0500 mol.L-1 solution of the cation
3. Calculate the (a) pH (b) pOH (c) percent ionizaton of 0.100 M ammonia. NH3 kb = 1.8x10^-5 4. Give five (5) techniques on how to produce an ideal precipitate in the analysis of sodium fluoride, NaF with silver nitrate, AgNO3 as precipitant using precipitation gravimetry. please answer all questions. I don't have questions left so i cannot repost the other question
b) In the development of a method for the determination of formic acid by neutralization volumetry, the pH was calculated as a function of the addition of NaOH for the titration of 25.00 mL of 0.1280 mol/L formic acid with NaOH standardized with concentration of 0.0670 mol/L. With reference to this titration curve, determine the pH of the solution after the addition of 5.00 mL of titrant and at the equivalence point. Data: Ka=1.70x10-4. Present the results with two places after the comma and show your calculations. c) Based on the table below, indicate which indicators could be used to determine the end point of this titration.
The molar solubility of CuCO3 at 298K is 1.5811×10-5 M. Determine the Ksp of this salt.
From the given information in the table calculate for both titration1 and 2: 1)moles of thiosulphate titrated (mols) 2) moles of hypochlorite (mols) 3) mass of sodium hypochlorite (g) 4) wt% of sodium hypochlorite
The molar solubility is 1.33x10^-5
(a) I f t he molar solubilit y o f CaF2 at 35 °C i s1.24 x 10-3 mol/L, what is Ksp at this temperature? (b) It isfound that 1.1 x 10-2 g SrF2 dissolves per 100 mL of aqueoussolution at 25 °C. Calculate the solubility product forSrF2. (c) The Ksp of Ba(IO3)2 at 25 °C is 6.0 x 10-10. What isthe molar solubility of Ba(IO3)2?
A solution is prepared by dissolving 1.800 g of sodium acetate (CH3COONa) into 100.00 mL of a 0.180 M solution of acetic acid. The Ka of acetic acid is 1.8 x 10-5. What is the pH of the solution?
Explain the imporatnce of adding HCl during the washing of the initial precipitate
6g of impure NaOH were dissolved in water and the solution was completed to become 1L ,if 25ml of this solution were titrated with 18ml of 0.1 sulphuric acid ,the % of sodium hydroxide in the sample equals .... [NaOH=40g/m]
Why do you have to titrate until or above pH = 12.5 ± 0.2 to properly identify the unknown acid solution?
Ammonium acetate buffer is used as an important reagent for studying molecular biology, biological buffers, reagents and DNA and RNA purification. Ammonium acetate (0.24M) in combination with cold 66% (v/v) ethanol quantitatively precipitated RNA from very dilute solutions (greater than or equal to μg/ml) after centrifugation. Ammonium acetate (CH3COONH4) is also a salt of weak acid (CH3COOH) and weak base (NH4OH). The Ka and Kb are equal to 1.8 x10-5. The pH of this salt solution will be, a. pH > 7 b. pH ≈ 7 c. pH < 7 d. both cation and anion don’t hydrolyze. e. none of the above.