1. calculate the initial pH of the NH3/NH4+ buffer. How does it compare to the experimental value? 2. calculate the pH of the NH3/NH4+ buffer after the addition of HCl. How does it compare to the experimental value. 3. calculate the pH of the NH3/NH4Cl buffer after the addition of NaOH. How does it compare to the experimental value? ReortPart Four- Effectiveness of an NH3/NH4* BufferLabel two regular size test tubes 1 and 2 and place them in rack. Into tube 1 combine 5.0 mL of0.10M NH4C1 and 5.0 mL of 0.10M NH3 and mix well. Into test tube 2 add 10.0 mL of distilledwater. Using a pH meter, measure the pH of the buffer and the distilled water and record in thetable below (initial pH). Add 5.0 mL of 0.010M HCl to each test tube and measure the pH again.Discard the contents and rinse the test tubes. Again, into tube 1 combine 5.0 mL of 0.10M NH4C1and 5.0 mL of 0.10M NH3. Into test tube 2 add 10.0 mL of distilled water. This time, add 5.0 mLof 0.010M NaOH to each test tube and measure the pH again.pH afteraddition of HCIpH afteraddition of NAOHTest TubeInitial pH(1) NH3/NH4* buffer5.103.038.47(2) distilled water6.352.8311.29

We’ll answer the first question since the exact one wasn’t specified. Please submit a new question…

Answered: 1. calculate the initial pH of the…

Science

Chemistry

1. calculate the initial pH of the NH3/NH4+ buffer. How does it compare to the experimental value?

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter10: Potentiometry And Redox Titrations

Section: Chapter Questions

Problem 8P

See similar textbooks

Related questions

Q: Calculate the number of moles of HCl that must be added to 1.0 L of 1.0 M NaC2H3O2 to produce a…

A: Given that, 1.0 L of 1.0 M NaC2H3O2, i.e., [salt] = 1.0 mole. The Ka of NaC2H3O2 is 1.8×10-5. So,…

Q: An unknown sample was titrated with CH3COOH. After making the titration curve, no steep change was…

A: Given : Unknown sample is titrated with acetic acid. After making the titration curve, no steep…

Q: monoprotic acid has a Ka of 1.50×10−4. Sketch the titration curve for a 50.0 mL 0.10 M sample of…

A: IMPORTANT POINTS As dissociation constant given in the question is in the powers of 10-4 ,which is…

Q: you need to prepare 100.0ml of a pH=4.00 buffer solution using 0.100 M benzoic acid (Ka=6.30× 10-5)…

A: Given: molarity of benzoic acid=0.100 Mmolarity of sodium benzoate=0.240 Mvolume of buffer=100.0…

Q: Fill in the blanks: A buffer solution is consists of 0.100 M HCN and 0.200 M NaCN. HCN + H₂O H30* +…

A: For a buffer 0.100M HCN and 0.200M NaCN, we have to find pH of solution. We have to find pH after…

Q: Buffer solution has a pH of 7.2 and Ka of 6.2x10^-8 a. Calculate the pH after adding 10.00 mL of…

A: Buffer solutions are solutions containing acid-base conjugate pairs. These solutions possess a fixed…

Q: alculate the concentration of buffer components present in 226.00 mL of a buffer solution that…

A: Solution-Mol of HNO3 added = 6.0M ×1.70mL = 10.20 mmol NH3 will react with H+ to form NH4+ Before…

Q: tap water tap water Buffer Buffer (original pH) (pH after) (original pH) (pH after) addition of 0.1…

A: Solution: Buffer : A buffer solution is an aqueous solution consisting of a mixture of a weak acid…

Q: Which of the following combinations of aqueous solutions will result in the formation of a buffer…

A: for buffer solution both the pair of a weak acid with a conjugate base ( having one H+ less ).…

Q: Compute for the pH and generate a titration curve for the titration of 50.0 mL 0.0500 M NaOH with…

Q: In another experiment, the student titrated 50.0mL of 0.100MHC2H3O2 with 0.100MNaOH(aq). Calculate…

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

Q: Calculate the pH for each of the cases in the titration of 35.0 mL of 0.230 M NaOH(aq) with 0.230 M…

Q: Calculate the pH of 100.0 mL of a buffer that is 0.0750 M NH4Cl and 0.160 M NH3 before and after…

A: Given data,Molarity of NH4Cl=0.075MMolarity of NH3=0.160MVolume of buffer=100mL=0.100LMolarity of…

Q: a 22.1 ml sample of 0.506M formic acid is titrated with 0.506M NaOH. Calculate the pH after the…

Q: Would you calculate the ionic strength of this buffer? [Na2HPO4]=.024176 [NaH2PO4]=.1

A: Mathematically ionic strength is as follows:I=12∑CiniZi2Where, I=ionic strengthCi=concentration of…

Q: A buffer solution contains dissolved C6H5NH2 and C6H5NH3CI. The initial concentration of C6H5NH2 is…

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

Q: CHEMICAL EQUILIBRIUM 1. Calculate the pH of the solution of 0.026M ammonia and what is its percent…

A: Since, you have asked multiple question, so I will solved first question for you. You can see…

Q: How many moles of sodium hydroxide would have to be added to 125 mL of a 0.339 M hypochlorous acid…

Q: A 25.0-mL sample of 0.30 M HCl is titrated with 0.30 M KOH. What is the pH of the solution after…

Q: Which of the following solutions is a good buffer system? A solution that is 0.250 M H2SO3 and 0.250…

A: The buffer system is a solution that resists a change in pH whenever an acid or a base is added. It…

Q: A buffer solution contains dissolved C6H5NH2 and C6H5NH3CI. The initial concentration of C6H5NH2 is…

A: A buffer solution is formed by the dissolution of weak acid and its pH and pKa values should be…

Q: Volume the NaOh 0.100 M dispensed 17.10 ml pH 9.63. Calculate the molarity of HCl solution (15 ml of…

Q: If you had always titrated to a bright pink color, what reagent would have been in excess and how…

A: A titration is an analytical method to find the concentration of an unknown solution from a solution…

Q: A lactic acid/lactate ion buffer solution contains 0.25 MM HC3H5O3HC3H5O3 and 0.78 MM…

Q: Calculate the pH before and after the addition of 10.0 mL of 0.10 M nitric acid to 100. mL of each…

A: Given, Molarity of HNO3 = 0.10 M Volume of HNO3 in mL = 10.0 mL Volume of the buffer = 100 mL…

Q: A buffered solution of 4.80 pH and a total of 50mL is made by mixing 40mL of 1.0M acetic acid with…

A: Buffer solution It is an aqueous solution formed by mixing weak and its conjugate base. No. of…

Q: A 100.0 mL sample of 0.10M NH3 is titrated with 0.10M HNO3. Determine the pH of the solution after…

A: Given that the 100.0 mL sample of 0.10M NH3 is titrated with 0.10M HNO3. Number of millimoles of NH3…

Q: A 50.050.0 mL solution of 0.1600.160 M KOHKOH is titrated with 0.3200.320 M HClHCl. Calculate the pH…

A: The titration reaction taking place is given by, => HCl + KOH --------> KCl + H2O Given :…

Q: Does it matter how much water is used to dissolve the unknown monoprotic acid? Explain your answer.…

A: Yes , It matter how much water is used to dissolve the unknown monoprotic acid to make it into…

Q: Give a clear handwritten answer of this buffer solution ..we need to find out buffer pH...given 0.3…

A: Given, The molarity of ammonia = 0.3 35 M and The molarity of ammonium bromide = 0.457 M and if we…

Q: find the initial pH of 0.2000 L of a buffer solution that is 0.195 M methylamine and 0.125 M…

A: Given : Concentration of methylamine i.e CH3NH2 = 0.195 M Concentration of methylammonium nitrate…

Q: What weight of sodium formate must be added to 400.0 mL of 1.00 formic acid to produce a buffer…

A: Given volume of HCOOH = 400.0 mL Concentration of formic acid = [HCOOH] = 1.00 M Concentration of…

Q: a. Calculate the pH in the titration of 50.0 mL 0.03200 M chloroacetic acid (Ka = 1.36 x 10 ¹) after…

A: Given :- Volume of Chloroacetic acid, ClCH2COOH = 50.0 mL Molarity of Chloroacetic acid, ClCH2COOH…

Q: Compare the two situations below using the titration curves. Adding HCl to a solution of NaOH with a…

A: The acid-base titration is proceeded by the neutralization of an acid by base or its vice-versa. The…

Q: Approximately how much Sodium Hydroxide was added when the titration curve reached the equivalence…

A: Equivalence point is point in titration at which the amount of titrant added is just enough to…

Q: What chemical would have to be in the same solution as CHO2- in order to form a buffer? Question…

Q: A buffer works best when the concentration of weak acid is high and ___________ its conjugate base's…

A: Interpretation - A buffer works best when the concentration of weak acid is high and ___________…

Q: During a titration of HCl and NaOH solution, which chemical substance at the equivalence point…

A: During the titration of HCl (Strong Acid) with NaOH (Strong Base) will produced a water along with…

Q: 1. When a small amount of acid is added to a non-buffered solution, there is a large change in pH.…

A: Solving only first question in accordance to guidelines. You can repost remaining questions

Q: Calculate the pH of the 0.30 M NH3/ 0.36 M NH4Cl buffer system. What is the pH after addition of 20…

Q: HF Ka = 3.5 X 10-4 HC2H3O2 Ka =1.8 X 10-5 HCN Ka = 4.9 X 10-10…

A: A good buffer range is about always pH = Pka ( + or -) 1 Pka = -logKa Pka = -log 3.5 x 10-4 Pka =…

Q: Calculate the pH of the 0.30 M NH3 / 0.36 M NH4Cl buffer system. What is the pH after addition of…

Q: A sample of a certain monoprotic weak acid was dissolved in water and titrated with 0.150 M NaOH,…

A: Given: Concentration of NaOH = 0.150 M Volume f NaOH required to reach equivalence point = 16.00 mL…

Q: (a) Calculate the pH of the 0.39 M NH3/ 0.73 M NH4Cl buffer system. pH = (b) What is the pH…

A: 1)Use basic buffer equation PH+PoH= 14 2) use Acidic buffer equation to get answer. Buffer is…

Q: The following question refers to a 2.0-liter buffered solution created from 0.72 M NH3 (Kb = 1.8 ×…

A: Second option. 9.70

Q: a 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3. Determine the pH of the solution after…

Q: If the equivalence point of the titration is when the pH is 4, what indicators could you use? Acidic…

A: The value of pH at equivalence point of the titration is 4 (given).

Q: The titration on the right was performed by placing 10.00 mL solution in an Erlenmeyer flask and…

A: when a weak base is titrated strong acid, before equivalence point we get buffer solution.

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

1. calculate the initial pH of the NH3/NH4+ buffer. How does it compare to the experimental value?

2. calculate the pH of the NH3/NH4+ buffer after the addition of HCl. How does it compare to the experimental value.

3. calculate the pH of the NH3/NH4Cl buffer after the addition of NaOH. How does it compare to the experimental value?

Reort
Part Four- Effectiveness of an NH3/NH4* Buffer
Label two regular size test tubes 1 and 2 and place them in rack. Into tube 1 combine 5.0 mL of
0.10M NH4C1 and 5.0 mL of 0.10M NH3 and mix well. Into test tube 2 add 10.0 mL of distilled
water. Using a pH meter, measure the pH of the buffer and the distilled water and record in the
table below (initial pH). Add 5.0 mL of 0.010M HCl to each test tube and measure the pH again.
Discard the contents and rinse the test tubes. Again, into tube 1 combine 5.0 mL of 0.10M NH4C1
and 5.0 mL of 0.10M NH3. Into test tube 2 add 10.0 mL of distilled water. This time, add 5.0 mL
of 0.010M NaOH to each test tube and measure the pH again.
pH after
addition of HCI
pH after
addition of NAOH
Test Tube
Initial pH
(1) NH3/NH4* buffer
5.10
3.03
8.47
(2) distilled water
6.35
2.83
11.29

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

Trending now

This is a popular solution!

Step by step

Solved in 4 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

Make 50 ml of the extraction buffer containing the following ingredients using the stock solution you made (1M Tris-HCl, 5 M NaCl, 0.5 M EDTA, and 10% SDS). You add each solution into one sterile tube using sterile pipets and add an appropriate amount of sterile ddH2O to make it 50 ml. Include the amount of sterile ddH2O. Extraction buffer composition: 200 mM Tris-HCl (pH 8.0) 2 M NaCl 25 mM EDTA (pH 8.0) 1% SDS
why is it necessary to test the ph? EXTRME DETAIL PLEASE PROCEDURE To a six inch test tube was added thiamine hydrochloride (0.65 g), followed by water (2mL). The mixture was gently shaken until homogeneous, and then ethanol (7.5 mL)was added. Finally, sodium hydroxide (10%, 1.5 mL) was added and the mixture wasgently stirred to ensure complete mixing.Benzaldehyde (3.8 mL) was then added at room temperature in one portion with gentlestirring. The pH of the resulting reaction mixture was determined and adjusted to >10by dropwise addition of 10% sodium hydroxide.
Standard solution : 0.201 grams of acetylsalicylic acid was combined with 10 mL of 0.5 M NaOH, then transfered to a 100 mL flask and filled the rest of the way with water Then 0.500 mLs of the standard solution was transfered to a 10.00 mL flask and diluted to the 10 mL mark with 0.02 M of buffered iron chloride. This step was repeated using 0.400, 0.300, 0.200, 0.100 mLs of the standard solution Questions: A.) determine the concentration of the acetylsalicylic acid in the 100.00 mL volumetric flask containing the solution from which the standards were made. B.)determine the concentration of the acetylsalicylic acid in each of the 10.00 mL calibration solutions. I only need the work for 0.400 mLs C.)Make a scatter plot (on the computer again) of absorbance versus concentration for the calibration samples. On the plot, add a linear trendline, and display the equation and the R2 value on the chart. Take your time to label the axes
BUFFER CAPACITY EXPERIMENT Part 1: Preparation and pH Meter Calibration Prepare 50 mL of 0.5 M acetic acid from a concentrated stock. Prepare 50 mL of 0.5 M sodium hydroxide from a solid. Part 2: Buffer Capacity Transfer 20 mL of 0.5 M acetic acid (Ka is 1.75*10-5), stir at a slow setting and measure the pH reading is stabilized. Add 1.0 mL of 0.5 M NaOH and measure the pH. Continue adding 0.5 M NaOH in 0.5 - 1.0 mL increments until a major spike in pH occurs. After the spike, add another two 0.5 – 1.0 mL increments of 0.5 M NaOH. Create a pH vs. Volume graph to determine the range of the buffer’s capacity. Compare the actual data (nonstandard conditions) with the theoretical data under standard conditions. I NEED HELP WITH CALCULATIONS AN SMALL RESULT INTERPRETATION DESCRIPTION PLEASE TO UNDERSTAND WHAT I DID AND WHY THANKS
Accurately weigh out about 6g copper(ii) sulfate crystals into a weighing boat. Use the copper(ii) sulfate crystals to make up 250cm3 of standardized copper (ii) sulfate solution Pipette 25cm3 of this solution into a conical flask Add 1.5g potassium iodide and swirl thoroughly Titrate this solution with standard 0.1 moldm-3 Na2S2O3 in a burette. When the iodine color fades, add 1 cm3 starch indicator. Use your titration data below to calculate the percentage by mass of copper in the copper(ii) sulfate crystals.
1. These are balances that have a maximum loading of 10 to 30 g with a precision of 60.01 mgA. semi-microanalyticalB. MicroanalyticalC. MacrobalancesD. Triple Beam Balance2. Which type of curve is normally produced when plotting the change in the concentration of a specie of some function and the amount of reagent added?A. Titration curveB. Sigmoidal CurveC. Phase Transition curveD. Calibration curve3. In the dead dear case study, silver diethyldithiocarbamateforms a colored solution when it binds with arsenic, what do we call substance like silver diethyldithiocarbamate?A. Secondary standard reagentB. Precipitating agentC. Chelating agentD. Primary standard reagent
You want to make a solution of the primary standard sodium oxalate. It has a molecular mass of 133.999 g/mol (no error). Your analytical balance has an error of 0.2 mg. You add some weighing paper to the balance and it reads a mass of 0.23626 g. You then add sodium oxalate onto the weighing paper until the mass registers as 2.8539 g. You carefully transfer this to a 250.0 ml volumetric flask with an error of 0.1 ml and dissolve the sodium oxalate in a sufficient volume of water. What is the concentration of the oxalic acid (in M) and what is the absolute error (also in M).
A deepwell water sample of 100 mL was titrated with 0.010 M EDTA at pH 10 ( with Mg-EDTA pH 10 buffer reagent) and consumed 31 mL. Calculate the Total Hardness of the water sample as mg CaCO3. Ans in 3 sig figures. no need to write the unit.
How would you make up 1 L of a 20X stock solution of the following buffer? 50mM glucose (FW=180.16)25mM Tris (FW 121.1)10mM EDTA (FT=372.24) I think, I already calculated the grams of each one, but I don't know how to do the 20X Glucose: 9.008gTris: 3.02gEDTA:3.72G
create a qulaitative analysis separations flow chart for the separation of Sb3+ and Cd2+
Determining the Ksp of Calcium Hydroxide: Ca(OH)2 (s) ↔ Ca2+ (aq) + 2OH– (aq) Ksp = [Ca2+][OH–]2 The molarity of the hydrochloric acid used was 0.050 M.15.00 mL of filtered Ca(OH) 2 was measured out for the titration.Calculate the [Ca 2+ ]. Explain, please. Trial Initial Buret Reading Endpoint Buret Reading Endpoint Volume Equivalence Point Volume 1 80 ml 9.31 pH 12 ml 12.60ml
The water hardness of tap water has been determined to be 120 (= 120 mg CaCO3 per 1 L of water). After the tap water has run through the ion exchange column, titration of a 20.00 mL sample used only 0.70 mL of 0.0100 M EDTA, to reach the endpoint. Calculate the effectiveness of the ion exchange column: what is the % of the calcium, removed by the ion exchange column? Provide your answer in % and without decimal. ( Please type answer note write by hend)