Procedure I. Preparation of acetate buffer solutions with different pH values 1. Calculate the salt and acid volumes required to prepare 10 ml of the acetate buffer with the following ratio of sodium acetate and acetic acid: Test tube #3: Ratio - 9:1 Salt volume Acid volume ml ml

Procedure I. Preparation of acetate buffer solutions with different pH values 1. Calculate the salt and acid volumes required to prepare 10 ml of the acetate buffer with the following ratio of sodium acetate and acetic acid: Test tube #3: Ratio - 9:1 Salt volume Acid volume ml ml

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: points? I. The end point of a titration is reached when the titrant and analyte are…

A: Equivalence point is defined as the point where the concentration of titrant is equivalent to the…

Q: A buffer solution contains 0.314 M hydrocyanic acid and 0.307 M potassium cyanide. If 0.0366 moles…

A: Given,(i) Molarity of hydrocyanic acid =0.314 MMolarity of potassium cyanide =0.307 Mvolume of the…

Q: 1. Determination of Vitamin C in Grape Juice acid, which gives the characteristic citrus taste to…

A: Citrus fruits contain Vit C. It is antioxidant that is essential for human body. Vit C content can…

Q: 14 12- 10- 8- 6- A 10 ***** B 20 30 40 Volume titrant (mL) 50 60 The region labeled "C" is the…

A: The titration curve is the curve between pH and the volume.The objective of this question is to…

Q: how would i find the average titre value in ml if I have 10% ethanol 1.3 ml (of water used) as…

A: Titration is the quantitative method of estimating the strength of the any component. Molarity is…

Q: When a reaction of HCl + NaOH and Acetic acid + NaOH are reacted and a drop of universal indicator…

A: Answer: In the given problem acid-base titration is taking place where acid is the analyte and base…

Q: 2. A student titrated 25.0 mL of a buffer with 0.116 M HCI. The observed titration curve is shown…

A: The buffer must be a basic buffer, containing a weak base BOH and its salt BCl.

Q: 8. pH at the half equivalence point of an acid-base titration equals a) Ka of the acid b) pKa of the…

A: Introduction For any particular solution, pH of that solution can be derived by applying the…

Q: Use the data reported in Table 1 and plot two separate graphs of measured pH against the volume of…

A: We need to plot graphs for pH against volume of NaOH added.

Q: The sodium bicarbonate NaHCO3, sample is only 72.56% pure after it has been analyzed by the student…

A: Since you have posted a question with multiple sub parts, we will provide the solution only to the…

Q: Bacro4 1.17x10 Calculate the solubility at 25 °C of AgCl in pure water and in a 0.0030M AGNO,…

A: We will calculate solubility in water and AgNO3

Q: When a 28.4 mL sample of a 0.467 M aqueous hydrofluoric acid solution is titrated with a 0.446 M…

A: Answer: In this question we have to calculate the pH of two types of solution those are forming at…

Q: (1) Mass of KHP (g) 0.6364 g (2) Moles of KHP Convert to moles (M.W. 204.22 g/mole) (3) Initial…

A: Given that, the mass of potassium hydrogen phthalate (KHP) = 0.6364 g and the molecular weight of…

Q: b) Answer the following questions related to titration technique i) What is difference between…

A: (i) Acidimetry titration v/s Alkalimetry titration Acidimetry Alkalimetry It…

Q: When a 27.3 mL sample of a 0.322 M aqueous hypochlorous acid solution is titrated with a 0.469 M…

A: 1.) Hypochlorous acid ia a weak acid and potassium hydroxide is a strong base , so they will react…

Q: 1) Calculate fluoride, CaF2, has a solubility product of 3.2*10-11. This means you can titrate a…

A: As per the rule only the first three subparts can be answered

Q: what is the average molarity of the unknown NaOH for your three titrations ? trial 1 mol=…

A: Average molarity can be defined as , molarity of all the trials devide by no. of trial. Molarity =…

Q: 7 9. A calculate tit titration is HNO3 titration Sketch 50.00 titrated me and titration a and potta…

A: Titration curve basically contains the volume of titrant as an independent variable and pH of…

Q: The pH curve generated by titrating phosphoric acid with sodium hydroxide will have _________…

A: Basicity of acid is equal to equivalence point.

Q: Calculation of the ionization constant for acetic acid from the measured pH of the acetic acid…

A: Given, Average pH = 3.11

Q: What is the pH of a buffer solution containing 1.25 M NH3 and 0.78 M NH,NO3? The base dissociation…

A: NH3 is a weak base and NH4NO3 is its salt , so they form a basic buffer solution. We first use…

Q: An acid is found to have a Kg = 2.6 × 10-4. Calculate the value its pKa. O a. +8.25 O b. -3.59 Ос…

A: You have multiple questions so i will solved first question for you rest of question post…

Q: None

A: To ensure a comprehensive understanding of the buffer properties and related calculations, here's a…

Q: How would the results of an experiment change if a basic buffer was utilized instead of an acidic…

A: The results of an experiment would change if a basic buffer was used instead of an acidic buffer in…

Q: Complete the qualitative test for cations diagram

A: According to the question, We need to fill in the qualitative test table for cation.

Q: 5. How to prepare 50mL of 375 mM citrate buffer pH 1.8 (8% (v/v) ethanol)

A: Concept: Buffer solution: a buffer solution ( pH buffer or hydrogen ion buffer) is defined as an…

Q: a)Calculate the theoretical pH of the HCI solution before and after addition of ten drops of 0.1 M…

A: Buffer is a solution that resists change in pH when small amount of strong acid is added to it.…

Q: Dase B) a weak acid (analyte) titrated with a strong base C) a strong base (analyte) titrated with a…

A: From the graph. pH is decreases continuously. And initially pH is greater than 7 . Then it is…

Q: Determine the relationship between the observed/apparent value (EX) VERSUS that of the true value…

A: To determine relationship between observed/apparent value (EX) vs. ET by writing <, > or = on…

Q: 8. What is the molar solubility of Ni(OH)2 in a basic solution with a pH of 11.0?

Q: None

A: The reaction is H2SO4 + 2NaOH - Na2SO4+ 2H2OOne mole of H2SO4 REQUIRED 2 Mole of NaOH So 1 mole NaOH…

Q: Question 15 An unknown student takes 25.0 ml sample of an unknown weak base solution with a an…

Q: 2 A student determined the concentration of a weak acid, acetic acid, by a titrimetric method using…

A: A question based tools in analytical chemistry that is to be accomplished.

Q: What are the two ways to determine that the equivalence point has been reached in the reaction? O…

A: An acid base titration is a titration in which the concentration of an unknown acid can be…

Q: The titration curve between an acid and a base is shown below. a) Name an acid and a base that could…

A: An indicator helps in visualizing the end point of the titration. It changes colour at the end…

Q: What species can I use from the choices below to neutralize a solution of hydrofluoric acid (V=120…

Q: What ratio of NaCN to HCN is needed to prepare a pH 10.20 buffer? (Ka of HCN is 4.9 x 10-¹⁰)

Q: ncentration of Hydrochloric Acid (M) 0.07036 22°c Temperature (C) Titration 3 Titration 1 Titration…

A: The data given is, And the concentration of HCl = 0.07036 M

Q: A 15.0 mL solution of Sr(OH), is neutralized with 39.5 mL of 0.350 M HCI. What is the concentration…

A: Acid reacts with base to form salt and water. Write the reaction of given acid with base.…

Q: I Review I Constants I P III LI IS LILI alivin, ti e connceIILI aliun UI Dase iS KNOWN aliu Can Ue…

Q: What is the pH of a buffer solution containing 0.50 M acetic acid and 0.50 M sodium acetate? The…

Q: What is pH with 0.00 mL NaOH added? What is pH 12.50 mL (half- way equivalence point) What is pH at…

A: pHHydrogen potentials are referred to as pH. It indicates the hydrogen ion concentration in a…

Q: A solution is prepared at 25 °C that is initially 0.39M in chloroacetic acid (HCH,CICO,), a weak…

Q: A buffer is made up of equal volumes (451.8 mL of each) of 0.812 M A H and 0.885 M A minus. 24.51 mL…

A: Given question is related to the calculation of number of moles of weak acid present in a buffer…

Q: 6. What is the pH of a mixture of 5 ml of 0.1 mol/litre sodium acetate and 4 ml of 0.1 mol/litre…

A: Solution: In this problem we will calculate pH using henderson equation.

Q: OH will the pH of the solution be equal to the pKa of acid? pH Curve 14 12 10 8 8 10 12 14 16 18 20…

A: Half neutralization point at which both acid and base neutralize by 50% so salt and acid will remain…

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

Procedure
I. Preparation of acetate buffer solutions with different pH values
1. Calculate the salt and acid volumes required to prepare 10 ml of the acetate buffer
with the following ratio of sodium acetate and acetic acid:
Test tube #3: Ratio - 9:1
Salt volume
Acid volume
ml
ml

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

Question Completion Status: For Solution A, approximately how many mL of HCI were needed to exceed the buffering capacity of this solution? Enter the number only. Don't enter units as part of your answer and don't use commas or scientific notation. Titration curve of Solution A 14 13 12 11- 10 9 8 pH 7 6 5 4 3 2 1 5 4 3 2 1 HCI added (mL) 0 1 2 3 4 5 NaOH added (mL) 14 13 12- 11 10 9 8 pH 7 6.8 2 65 4 3 2 1 Titration curve of Solution B Click Save and Submit to save and submit. Click Save All Answers to save all answers. 54 32 1 HCI added (mL) 0123 NaOH added (mL)
A 100.0 mL buffer is to be made so that the [ HC,H3O2 ] = 0.159 M HC2H3O2. How many milliliters of 2.500 M HC2H3O2 (aq) stock solution are needed? IMPORTANT: When entering your answer: • Enter the number only (no units) • Do not leave any spaces • Use a leading zero before the decimal when necessary o Report your number to 2 decimal places (regardless of the significant figures) • Correctly round your answer to the 2nd decimal place (margin of allowed error is only + 0.01, so always use un-rounded numbers in your calculations). If the last digits are zeros they will not display once you click away, but the answer will still be marked correct. Examples: 12.34 or 0.56
Redox (Dichromate Titrations) Which of the following indicators is a redox indicator used in the dichromate titration? a) Diphenylamine sulfuric acid b) Bromocresol green e) Phenolphthalein d) Ferric ion e) Methyl orange
I. Preparation of acetate buffer solutions with different pH values 1. Calculate the salt and acid volumes required to prepare 10 ml of the acetate buffer with the following ratio of sodium acetate and acetic acid: Test tube #1: Ratio - 1:9 Salt volume Acid volume ml ml
A 50.00 (±0.02) mL portion of an HCl solution required 29.71(±0.02) mL of 0.01963(±0.0032) M Ba(OH)2 to reach an end point with bromocresol green indicator. ? of HCL = 29.71?? ? 0.01963 ???? ??(??)2 ?? ? 2 ???? ??? ???? ??(??)2/ 50.00?? = 0.02333 ? Calculate the uncertainty of the result (absolute error).Calculate the coefficient of variation for the result.
all 3 parts please
A 24.0 mL sample of 0.115 M sulfurous acid (H,S03) is titrated with 0.1019 M KOH At what added volume of base solution does the first equivalence point occur? Express your answer in mililiters to three significant figures. V. mL Submit Request Answer Vorue nertlel
@ Prepare a "pH curve" as follows: a) Find the pH of the acid solution just before the end point when 0.1 ml of base less than the end point voiume has been added. potnt, therefore at the end of the titration ph - 7. We are assuming that end point equals equivalence b) Repeat calculation 'a' for a volume 1 ml less and 5 ml less then end point and before any base is added. That is Oml base added.) Before end point, we assume that all the base is used up by the acid. c) Assuming you had continued the titration past the end point, calculate the pH when 0.1 ml of base beyond end point had been added. d) Repeat calculation 'c' for 1 ml, S ml and 10 ml of base beyond end point. Show all calculations and record your results in a table similar ta the one shown below: excess H+ excess OH 0 -5 -1 END PT -.1 +.1 +1 +5 +10 (ML) BASE VOLUME 20 24 24-9 25 25.1|26 30 35 pH
Thank you! Data included in pictures! No hand drawn graphs!! Determine the equivalence point and the endpoint of the sudsy ammonia/citric acid reaction by graphing the titration data (pH vs volume citric acid) from Table 3: Titration of Sudsy Ammonia with 0.25 M Citric Acid Data with the Chosen Indicator. Draw a green arrow (use ‘Insert Shape’ feature to do this once you have copied your graph from Excel) on your graph indicating the data point that represents your equivalence point. Draw a blue arrow (use ‘Insert Shape’ feature to do this once you have copied your graph from Excel) on your graph indicating the data point that represents your endpoint. Use a graphing software to create the x-y scatter plot showing the pH of the experimental solution as a function of the volume of citric acid (the titrant) added for the titration data in Question 9. On your graph, the x-axis should be the volume of citric acid added (mL), and the y-axis should be the pH of the experimental…
2 A student determined the concentration of a weak acid, acetic acid, by a titrimetric method using a standard NaOH solution and a pH meter for end point detection. Table 1.0 below shows the data that was obtained by the student. Table 1.0: Potentiometric titration of acetic acid with 0.100 M standard NaOH solution Burette Reading Volume of NaOH added (mL) pH reading 11.54 0 3.14 12.25 0.71 3.70 13.40 1.86 4.16 16.59 5.05 4.77 17.50 5.96 4.93 19.35 7.81 5.24 20.41 8.87 5.49 21.00 9.46 5.68 21.60 10.06 5.96 21.83 10.29 6.14 22.01 10.47 6.34 22.12 10.58 6.48 22.20 10.66 6.68 22.30 10.76 6.97 22.38 10.84 7.73 22.41 10.87 9.21 22.49 10.95 10.04 22.55 11.01 10.57 22.61 11.07 10.83 23.00 11.46 11.35 23.31 11.77 11.62 23.71 12.17 11.76 24.30 12.76 11.89 25.20 13.66 12.03 Plot a curve of pH versus the volume of NaOH and determine the end point a.
M of NaOH: 0.100 Volume of HCI 25mL = 0.025L Moles of HCI = 2.5 mol What is the Volume of NaOH equivalence point: What is Moles of NaOH equaivalence point: What is pH at equivalence point? What is calculated pH and experimental pH of NaOH at 0.00 mL , 12.50 mL, 25mL, and 30 mL. Also what is the Error percentage for each one?