Answered: Show the calculations for the mass of…

Show the calculations for the mass of 99.0% sodium acetate NaC2H3O2 salt that was needed to prepare the 250 mL acetic acid/acetate ion buffer solution that has a pH 4.5 and 0.10 M acetate ion.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter15: Additional Aqueous Equilibria

Section: Chapter Questions

Problem 90QRT: Which of these buffers involving a weak acid HA has the greater resistance to change in pH? Explain...

See similar textbooks

Related questions

Q: How would prepare 750ml of 0.1M NaCl, 0.5M Tris-HCl solution given that you have 5M NaCl and 1M…

A: Molarity is defined as the moles of solute present per liter of solution. For example: 5 M NaCl…

Q: 4.Calculate the pH of the buffer prepared by mixing 2.00 g of NaOH with 80.0 mmol of salicylic acid…

A: Moles of NaOH = 2.0040=0.05 mol = 50 mmol…

Q: Assuming the Ka is 2.37 x 10-5 for acetic acid, calculate the pH at the half equivalence point for a…

A: Acetic acid is a weak acid while NaOH is a strong base. So the titration of acidic acid with NaOH is…

Q: A buffer was prepared by adding 2.4 g ammonium nitrate to 100.0 mL 0.30 M ammonia (Kb = 1.8 x 10-5…

A: We have 2.4 g of ammonium nitrate , 100 ml of 0.3 M of ammonia, to this we added 10 ml of 0.3 M of…

Q: What mass (g) of dipotassium phthalate must be added to 750 mL of 0.0500 M potassium acid phthalate…

A: dipotassium phthalate = K2P phthalate = P pH = 5.75 [H3O+] = antilog(-5.75) = 1.778 x 10-6…

Q: Describe how you would accurately prepare 100.0 mL of a buffer solution with pH 4.7 using 1.0 M…

A: Given: pH = 4.7 Ka = 1.8 x 10-5 pKa = -log(1.8 x 10-5) = 4.745 [CH3COOH] = 1 M [NaOH] = 1 M…

Q: A student titrates 20.00 mL of 0.100 M triethylamine (CH3CH3)3N (Kb = 5.2 x 10-4) with a 0.100 M HCl…

Q: Solve for the pH level of an ammonia buffer. Given that it contains 500.0 mL of 0.3701 M ammonia and…

Q: c) Jack and Helen wish to sketch a weak acid strong base titration curve. Before they can do so,…

Q: Calculate the volume of 0.120M hydrocyanic acid, HCN (K, -4.9 x 10-10) solution, needed to prepare…

Q: A mixture contains initially benzoic acid C6H5CO2(weak acid), Ka = 6.28 x 10^-5, and its…

A: Given data : Ka of benzoic acid = 6.28 x 10^-5 , concentration of benzoic acid = 0.250 M…

Q: Prepare a buffer consisting of acetic acid and sodium acetate with a total acetic acid plus acetate…

A: The Henderson-Hasselbalch equation is labelled as equation (1) in which [acid ] and [conjugate base]…

Q: Prepare 500 mL of 0.1 M bicarbonate buffer solution, pH = 6, from 0.1 M stock solutions of carbonic…

Q: 0.02 M NaOH reagent was standardized using 0.1000 g Potassium hydrogen phthalate (204.22 g/mol) and…

Q: Find the solubility of AgCl in pure water, 0.10M KNO3, and 0.10M NaCl

A: AgCl is sparingly soluble salt , its solublity in absence of common ion " S " mol/L , in presence…

Q: Show your calculations for determining the mass of sodium acetate trihydrate (CH3COONa • 3 H2O) and…

Q: Describe how to mix up a buffer. Dissolve 1.20g of sodium dihydrogen phosphate and 0.885g of…

A: Please find the attachment.

Q: You are given 100.0 mL of the following buffer: 0.010 M HC2H3O2 and 0.010 M NaC2H3O2. What is the…

A: Given, HC2H3O2=0.010 M ; NaC2H3O2 =0.010 MKa=1.7×10-5we are asked to calculate the effective pH…

Q: Consider the titration of a 60.0 mL of 0.351 M weak acid HA (Ka = 4.2 x 10 °) with 0.400 M KOH. 5…

A: mmoles of Acid = 60.0mL • 0.351molL-1 = 21.06mmol mmles of Base = 75.0mL • 0.400molL-1 = 30mmol…

Q: A benzoate buffer is prepared containing 0.33 M benzoic acid and 0.28 M benzoate. The Ka of benzoic…

Q: Consider the titration of 20 mL of 0.60 M acetic acid (Ka = 1.8 x 10-5) with 0.20 M NaOH. What…

Q: How will you prepare 500 ml of 0.750 M citrate buffer with pH of 4.25 from solid citric acid…

Q: 2. 20.0 mL of 0.1000 M Benzoic Acid (HC7H5O2) in a flask is being titrated with 0.1000 M NaOH…

A: Note: Since you have posted multiple independent questions in the same request, we will solve the…

Q: Consider the titration of 30.0 mL of 0.050 M NH3 with 0.025 M HC1. Calculate the pH after the…

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

Q: A solution of 100.0 mL of 0.0400 M sodium propanoate (the sodium salt of propanoic acid) was…

A: Hello. Since the question contains more than three sub-parts, the first three sub-parts shall be…

Q: Calculate the mas of KC2H3O2 that must be added to 500.0mL of a 0.200 M HC2H3O2 (Ka = 1.8 x 10-5)…

A: Given→ Volume of HC2H3O2 = 500.0 mL Molarity of HC2H3O2 = 0.200 M Ka…

Q: A student was told to make a pH=10.0 buffer from NH3 and NH4Cl. What concentration of NH3 and NH4Cl…

A: To make a pH=10.0 buffer from NH3 and NH4Cl we first Calculate the The Value of Pkb from given…

Q: Find the pH of the buffer containing 0.0005 M acetic acid and 0.00045 M sodium acetate without…

Q: suppose there is 1.00L of an aqueous buffer containing 600.0 moral & acetic acid (pk. 4.76) and 40.0…

A: NaOH is a base and when it is added to the buffer , it gets add up to the base concentration and…

Q: What mass of sodium benzoate should you add to 150.0 mL of a 0.17 molL−1 benzoic acid solution to…

Q: Consider the titration of a 60.0 mL of 0.355 M weak acid HA (Ka = 4.2 x 10⁻⁶) with 0.400 M KOH.…

A: Molarity is the ratio of moles of solute to volume of solution in L. Molarity = Moles of…

Q: A buffer is made using 45.0 mL of 0.750 M HC3H5O2 (Ka = 1.3x10-5) and 55.0 mL of 0.700 M NaC3H5O2.…

Q: Consider the titration of 100.0 mL of 0.200 M acetic acid (Ka = 1.8 x 10-5) by 0.100 M KOH .…

A: The question is based on the concept of titrations. we are titrating a weak acetic acid with a…

Q: Calculate the pH during the titration of 50.00 mL of 0.0500 M NaOH with 0.1000 M HCl after the…

A: 50 mL of 0.0500 M of NaOH titrated against 0.100 M HCl at different volumes.

Q: Describe how you would prepare a 100.0 mL buffer solution with a pH of 4.24 and an acetic acid…

A: Given data : For preparing 100 mL buffer solution with a pH =4.24 An acetic acid concentration =…

Q: 25.0 ml of 0.50M HA (Ka = 3.0 x 10-7) is titrated with 0.45M NaOH. Calculate the pH at the endpoint.

A: We need to find the pH at the end point for the given titration

Q: I did an experiment called Potentiometric Analyses where we titrate NaOH with a solid unknown weak…

A: 2 mole of OH- neutralizes 1 mole of acid Formula used : Molarity = no. of moles/vol(Lt)

Q: How many grams of sodium acetate (82.03 g/mol) should you add to 250 mL of 0.100 M acetic acid (Ka =…

A: The pKa is calculated as follows,

Q: In the heat of solution experiment If 10 ml of the solution of oxalic acid is diluted to 100ml amd…

A: Given : Initial volume of oxalic acid = 10 ml Final volume of oxalic acid = 100 ml Volume used…

Q: A buffer is prepared using lactic acid (HLac) and sodium lactate (NaLac). 0.300 dm3 of the 0.500…

A: Given, Concentration of lactic acid, [HLac] = 0.5 mol.dm-3 = 0.5 mol/L (1 dm3 = 1 L) Volume of…

Q: A buffer is created by mixing 600 mL solution of acid HA (0.500 M) with 700 mL of conjugate base A-…

Q: Calculate the pH of a 100.-mL buffer prepared with 1.30 g of imidazole (C3H¾N2) and 1.30 g of…

A: By addition of acid , base part of buffer system i.e. imidiazole unit reacts with acid to form salt…

Q: 2. Calculate the molar solubility and then the Ksp value for Ca(OH)2 at room temperature and 100 °C…

A: Given - Volume of Ca(OH)2 at 25°C = 5.0 mL Molarity of HCl at 25°C = 0.0120 M…

Q: A 1.0 ml protein solution in 0.500 M TRIS buffer, pH 7 with 0.250 M NaCl was dialyzed overnight…

Q: A buffer is made using 200.0 mL of 0.100 M (CH3)3N (trimethylamine) and 100.0 mL of 0.300 M…

A: The ratio of the mass of a substance to the molar mass of the substance is known as the moles of…

Q: 10.0 ml of .15M H3A (Ka1 = 2.5 x 104, Ka2 = 3.5 x 10-8, Ka3 = 5.0 x 10-12) is titrated with .10M…

A: The titration curve for the titration of 10.0 mL of 0.15 M triprotic acid H3A with 0.10 M NaOH…

Q: Calculate the pH during the titration of 20.00 mL of 0.1 M NaOH with 0.100 M HCl after the addition…

A: Given - Volume of NaOH = 20.00 ml Molarity of NaOH= 0.1 M Molarity of HCl = 0.100 M

Q: Consider the titration of a 60.0 mL of 0.355 M weak acid HA (Ka = 4.2 x 10⁻⁶) with 0.400 M KOH.…

A: The question is based on the concept of titration. we are titrating a weak acid with a strong base…

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

Show the calculations for the mass of 99.0% sodium acetate NaC2H3O2 salt that was needed to prepare the 250 mL acetic acid/acetate ion buffer solution that has a pH 4.5 and 0.10 M acetate ion.

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 by step

Solved in 2 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

A buffer is prepared by dissolving 0.062 mol of sodium fluoride in 127 mL of 0.0399 M hydrofluoric acid. Assume no volume change after NaF is added. Calculate the pH of this buffer.
A mixture contains initially benzoic acid C6H5CO2(weak acid), Ka = 6.28 x 10^-5, and its concentration is 0.250 M, and sodium benzoate of 0.400M. 500mL of this buffer were titrated with a strong base 250 mL of NaOH that has a pH of 12.875. a) What should the pH be after the addition of the base? b) Why do you think that this pH is correct? Please explain in terms of what really happened during the process that led to this pH, what specific ions or molecules affected the result? c) Sketch the titration curve that will result from this process. d) Predict the pH at the equivalence point, less, more, or equal to 7? Explain?
Show your calculations for determining the mass of sodium acetate trihydrate (CH3COONa • 3 H2O) and the volume (in ml) of 2.0 M acetic acid needed to make 100 mL of the acetate buffer containing 1.0 M acetic acid and 0.2 M acetate.
Calculate the mas of KC2H3O2 that must be added to 500.0mL of a 0.200 M HC2H3O2 (Ka = 1.8 x 10-5) solution to form a pH = 5.25 buffer solution.
A 250.0-mg sample of an organic monoprotic weak acid was dissolved in an appropriate solvent and titrated with 0.091 M NaOH, requiring 29.5 mL to reach the end point. Determine the compound’s equivalent weight.
Calculate the pH of the solution for every 0.1 ml of the titrant (from 0 mL to 30 mL) and generate a titration curve using Excel. A 100.0-mL aliquot of 0.100 M diprotic acid H2A (pK1 = 4.00, pK2 = 8.00) was titrated with 1.00 M NaOH Highlight each stage in the titration and the equivalence point. Also, obtain the first derivative of the curve (that is ΔpH / Δvolume).
How will you prepare 500 ml of 0.750 M citrate buffer with a pH of 4.25 from solid citric acid (C6H8O7) and solid sodium citrate (Na3C6H5O7)? The Ka of citric acid is 7.40 x 10-4
Calculate the pH at 0, 25, 50, 100 and 150.0mL titrant in the titration of 50.0mL of 0.500 M acetic acid with 0.25 M NaOH.
A student was told to make a pH=10.0 buffer from NH3 and NH4Cl. What concentration of NH3 and NH4Cl need to be used if the ionic strength needs to be 0.200. Ka of NH3 = 5.69 x 10-10 and pKa = 9.245
A chemist adds enough of the theoretical ionic compound MX2 to form a saturated solution. She knows X- is a weak base, so she titrates the solution and finds that [X-] = (1.0x10^-4) M. What is the value for Ksp of MX2 Note: Your answer is assumed to be reduced to the highest power possible.
Prepare a buffer consisting of acetic acid and sodium acetate with a total acetic acid plus acetate concentration of 250 mM and a pH of 5.0. What concentration of acetic acid and sodium acetate should you use? Assuming you wish to make 2 liters of this buffer, how many moles of acetic acid and sodium acetate will you need?
Calculate the molarity of the acid (HA) and the conjugate base (A- ) . For acetate, use grams-to-mol conversion and divide it by the total volume. For (aceitic acid), use M1V1=M2V2. Consider the total volume of your buffer (50 mL + 10 mL). a) [A-] = b) [HA] = I am not sure how to answer this or if it is related to this info that we were given at the top of the page: "A buffer is made by mixing 2.0 g of sodium acetate (NaA: 1 mol / 82 g) and 10 mL of 3.0 M acetic acid. Then 50 mL of water is added to the mixture. Find the pH of this buffer!"