I-Determining the Concentration of Sulfuric acid solution (H so.) by titrating it with NaOH Solution Table 1 Burette Reading (NaOH) Trial Initial reading Final reading AV Added Volume: AV (V1) (V2) 1 o mL 18.07 mL 18.07 mL 36.39 mL Vavg of NaOH V=

I-Determining the Concentration of Sulfuric acid solution (H so.) by titrating it with NaOH Solution Table 1 Burette Reading (NaOH) Trial Initial reading Final reading AV Added Volume: AV (V1) (V2) 1 o mL 18.07 mL 18.07 mL 36.39 mL Vavg of NaOH V=

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter17: Complexation And Precipitation Reactions And Titrations

Section: Chapter Questions

Problem 17.23QAP

See similar textbooks

Related questions

Q: 3. A 0.1093-g sample of impure Na2CO3 was analyzed by the Volhard method. After adding 50.00 mL of…

A: Given , mass of impure Na2CO3=0.1093 gVolume of AgNO3= 50.00 mLConcentration of AgNO3=0.06911…

Q: The Ksp value of CaSO4 is 2.4 x 10-5. If a professor made 1500 mL of a CaSO4 solution, then how many…

A: Given : Ksp of CaSO4 = 2.4 x 10-5 Volume of solution= 1500 ml

Q: Report sheet for Titration of vinegar Part I: Standardization of the NaOH solution with KHP…

A: The balanced equation for the reaction of NaOH(aq) and KHP(aq) is: NaOH(aq) + KHP(aq) →NaKP(aq) +…

Q: In his next experiment, he needs to determine the Ksp and identity of a sparingly soluble salt MF2.…

A: Since you have asked a question with multiple subparts, we will answer only first 3 subparts for…

Q: Exp. 4 Part 2 Titration of a Solution containing Ca(s) and Water Titrant: 0.30 MHC1 Data Trial 1…

Q: If 56.0 mL of a 0.85 M Ca(NO3)2 was mixed with 87.5 mL of 0.70 M NaCl, what is the final…

A: By writing balanced chemical equation and using mole mole analysis we can solve this problem.

Q: 10. The color change of a chemical indicator requires an over titration of 0.03 mL. Calculate the…

A: Given, The error in measurement = 0.03 mL The experimental values are 50.00 mL, 10.0 mL, 25.0 mL,…

Q: OH Calculate the percentage purity of naproxen (FW 230.26) from the following data. 210.7 mg of…

A: Given: The formula weight of naproxen is 230.26 g/mol. The amount of naproxen taken is 210.7 mg. The…

Q: 11. A 3.00-L sample of urban air was bubbled through a solution containing 50.00 mL of 0.0116 M…

A: Given that Volume of sample of urban air=3L Molarity of Ba(OH)2 solution=0.0116M Volume of Ba(OH)2…

Q: Based on the table below, calculate F-factor and X in the water sample. (Berdasarkan jadual di…

Q: Starting with 2.0 g of hand sanitizer in 10 mL of methanol (density of methanol = 0.791 g/mL), the…

A: Given that

Q: The KI used in this lab has a concentration of 0.500M. In trials 1-4, 1.0 ml of this solution is…

A: Concentration is defined as amount of solute per unit amount of solvent or solution. Molarity…

Q: Suppose Missy bon bon have 20.3 L sample of gas that contains an impurity, CO. The sample was then…

Q: В. In her next experiment. she needs to determine the Ksp and identity of a sparingly soluble salt…

Q: В. In his next experiment, he needs to determine the Ksp and identity of a sparingly soluble salt…

A: In the above solution MF2 is sparingly soluble. It is titrated with 0.0110M HNO3.

Q: 4) Given the following analyses of groundwater (reported as mg/L): Ca²+ = 16.5; Mg²+ = 3.1; Na = 13;…

Q: Name Post-Laboratory Questions (Use the spaces provided for the answers and additional paper if…

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

Q: . Add Ca(OH)2 to 250.0 mL distilled water with stirring until equilibrium is achieved.

A: The given compound dissociation-- Ca(OH)2(s) Ca2+(aq) + 2 OH−(aq) [OH−] = 2[Ca2+] (after…

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

Q: 2.1 Preparing primary standard potassium acid phthalate (KHP) solution for standardizing the 0.1 M…

A: KHP and NaOH react with each other in a stoichiometric ratio of 1:1.

Q: Jessica made 300 mL of primary standard using 2.35 g of sodium carbonate. She then conducted a…

A: Given - Mass of primary standard, sodium carbonate = 2.35 g and its volume is = 300…

Q: The concentration of the "A" solution of propanol is 3.0×10-3 M, using GC method, the height of this…

A: Gas chromatography is analytical technique that is used to quantify the amount of component present…

Q: to form Ba(IO3)2, 500 mL of 0.5000 M Ba(NO3)2 was mixed with 500 mL of 0.0500 M NaIO3. Ksp=…

Q: Prepare 100.00 mL of a solution with ALL the following chemicals into together; CHEMICALS PROVIDED

A: We have to Prepare 100.00 mL of a solution

Q: You are to make 300mL of 20mM EDTA buffer (C10H16N2O8) solution from powder. How much EDTA powder…

A: We need to make 300mL of 20mM EDTA buffer (C10H16N2O8) solution Number of moles of solution…

Q: Prepare 250 mL stock acetic acid solutions and from this solution prepare 100 mL of each standard…

A: A numerical problem based on preparing stock and working solutions, which is to be accomplished.

Q: Concentration sodium thiosulfate solution used: 0.056 mol L-¹ ACCURATE TITRATION VOLUME OF SODIUM…

Q: ANALYSIS OF VINEGAR A 25.00 mL vinegar sample was diluted to 250-mL using a volumetric flask. A…

A: Dilution Formula :- When a solution of molarity M1 and volume V1 is diluted by adding water to a…

Q: Ksp = 1.8 A solution contains 0.0040 M NazPO4. Calculate the minimum concentration (in M) of Ag'…

A: Ionic compounds have a strong tendency to dissociate into their individual ions in an aqueous…

Q: A 15.00 g sample containing mixed alkali and other inert components was dissolved and diluted to 300…

A: We have find out the The volume of titrant needed to neutralize NaOH is _________ mL.The volume of…

Q: You should determine how you will make the following solutions: 1- 0.8 M NAOH + 20 mM EDTA: Make 250…

A: Stock solution is a standard solution of high concentration. It can be diluted to lower…

Q: A 0.500-g sample containing BaBr2 (FM = 297.14) is dissolved in 50 mL of distilled water. Titrating…

Q: 5. Repeat the titration at least two additional times recording your data in the data table. Do not…

A: 6. We have to write a net ionic equation for the reaction between FeCl2 and KMnO4 . Oxidation half…

Q: (a) Standard Ag1 solution was prepared by dissolving 1.224 3 g of dry AgNO3 (FM 169.87) in water in…

A: Given data,Mass of AgNO3=1.2243gMolecular weight of AgNO3=169.87g/molVolume=500mL=0.5LVolume of Cl2…

Q: PRE-LAB QUESTIONS 1. A student dissolves 2.006 g of FeSO4-7 H₂O in 40 mL of sulfuric acid and then…

A: #2(a): Mass of FeSO4.7H2O standard taken = 2.047 g Molar mass of FeSO4.7H2O = 55.845 + 32.065 +…

Q: standard solutions (mg/L, n = 5) are converted to azo dye and the slope of the calibration curve is…

A: According to Lambert Beer law, the absorbance of a solution is proportional to its concentration and…

Q: Concentration sodium thiosulfate solution used: 0.056 mol L-1 ACCURATE TITRATION VOLUME OF SODIUM…

Q: [D] [N] [A] Trial 1 Trial 2 Trial 3 0.1 N 0.1 N 0.1 N 0.1 N HCI 0.1 N HCI 0.1 N HCI NaOH NaOH NaOH…

Q: the titrant was consumed in each run? Trial 1: 0.009981 M Trial 2: 0.009862 M Trial 3: 0.01029 M

Q: You collected the following data from a titration experiment using a 0.123M standardized NaOH…

A: Initial burette reading = 0.56 ml Final burette reading = 19.20 ml Volume delivered (ml ) = ?

Q: Following the monograph procedure, determine the weight in grams of sodium carbonate (MW-106 g/mol)…

A: The volume of H2SO4 = 21.3 mL. The mass of Na2CO3 = 1.1142 g.

Q: A 10.00 mL sample of alcoholic ethyl acetate was diluted to 100.00 mL. 20.00 mL was aliquoted and…

A: Answer: These questions are based on the stoichiometric calculation where moles of KOH will be…

Q: How do I find the total moles of Cl in 100 mL flask and the Cl concentration? I don’t know if I need…

A: Dilution factor:

Q: 100% 41 Safari File Edit View History Bookmarks Window Help Wed 4:51 PM A uk.instructure.com My…

A: Number of moles of KHP can be determined as follows,

Q: An unknown sample of Cu2+gave an absorbance of 0.262. Then 1.00 mL of solution containing 100 ppm…

Q: A 25.00 mL of pond water was analyzed using Winkler method. A standardized sodium thiosulfate…

A: A numerical problem based on Winkler's method, which is to be accomplished.

Q: Calculate the volume of each solution, volume of water and the total volume. 0.00150 M Fe³+. 0.00150…

A: Here , sample A , B and C are made by mixing two solutions and water and the final volume is 15.00…

Q: Table 1. Titration data Trial 1 Trial 2 Trial 3 Initial burette reading (mL) 1.43 2.50 1.33 Molarity…

A: Given: Trial-1 Trial-2 Trial-3 Initial burette reading 1.43 2.50 1.33 Molarity of NaOH…

Q: A 1.500-g sample of dried soil was analyzed for nitrogen using Kjeldahl procedure. The receiving…

Question

Help me please

I- Determining the Concentration of Sulfuric acid solution (H_So,) by titrating it with NaOH Solution
Table 1
Burette Reading (NaOH)
Trial
Initial reading
Final reading
AV
Added Volume: AV
(V1)
(V2)
1
o mL
18.07 mL
18.07 mL
36.39 mL
V=
|Vavg of NaOH
V=

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 with 1 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

8-49 A solution of NaOH base was titrated with 0.150 M HCI, and 22.0 mL of acid was needed to reach the end point of the titration. How many moles of the unknown base were in the solution?
Potassium hydrogen phthalate is a solid, monoprotic acid frequently used in the laboratory as a primary standard. It has the formula KHC8H4O4. This is often written in the short-hand notation as KHP. If 25.0mL of a potassium hydroxide solution are needed to neutralize 2.26g of KHP, what is the molarity of the potassium hydroxide solution? Potassium hydrogen phthalate sometimes called potassium biphthalate, as shown on this bottle is an acid that is convenient to store and use because it is a solid.
A solution of HCl was titrated against sodium carbonate. What is the normality of acid for Trial 3 in the given data? T1 T2 0.3562 0.3479 0.3042 Weight (g) Initial V (mL) 0.80 1.60 0.40 Final V (mL) 35.20 36.70 39.80 Vol HCI used (ml) 35.10 39.40 N of HC (eq/L) 0.1954 0.1870 Average N of HCl (eq/L)
Esc 2 What is the concentration of a solution made with 0.245 moles of KOH in 400.0 mL of solution? 1 F1 ! + A 4x Q N Bi F2 NO @ 2 W S Alt X F3 # 3 JL E F4 D 14 C $ 4 F5 R F ► 11 % 5 V F6 A T G ^ (0 F7 6 B Y H F8 & 7 2 DELL U N F9 * S 8 J F10 ( 3 9 F11 J K O A ) O F12 L Alt PrtScr P 7 BU +/- 4 1 Inse- [ VER ?
3:59 PM Wed Mar 15 ... ap here or pull up for additional resources Question 74 of 75 A 25.0 mL solution of HNO3 is neutralized with 16.5 mL of 0.250 M Ba(OH)2. What is the concentration of the original HNO3 solution? 1 4 7 +/- 1 M 2 3 5 6 8 9 O LTE 32% Submit XC с x 100
o/index.html?deploymentld%=55750828934189288909969212&eiSBN=9781305657571&snapshotld%32199898&id%3... ☆ IDTAP Q Search this cou Use the References to access important values if needed for this question. The concentration of H3ASO3 in a solution is determined by titration with a 0.1945 M Ce+ solution. The balanced net ionic equation for the reaction is: 2Ce*(aq) + H3ASO3(aq) + 5H2O(1) 2Ce*(aq) + H3ASO4(aq) + 2H3O*(aq) (a) If 19.83 mL of the 0.1945 M Ce** solution are needed to react completely with 30.00 mL of the H3ASO3 solution, what is the concentration of the H3ASO3 solution? M (b) Which of the two solutions was in the buret during the titration? (c) Suppose at the end of the titration, the solution containing the Ce³* ion is transferred to a volumetric flask and diluted to 300. mL. What is the concentration of Ce3+In the diluted solution? Submit Answer 5 question attempts remaining
TITRIMETRIC DATA SAMPLE: CANE VINEGAR % acidity in label: 4.5% %purity of KHP: 99.80% FORMULA WEIGHT of KHP: 204.22 g/mol STANDARDIZATION OF NaOH SOLUTION TRIAL 1 TRIAL 2 TRIAL 3 Weight of KHP, g 0.1012 0.1004 0.09987 Initial volume of NaOH, mL 5.00 10.01 Final volume of NaOH, mL 4.95 9.99 14.93 Molarity of NaOH Average Molarity of NaOH ANALYSIS OF ACETIC ACID IN A VINEGAR SAMPLE TRIAL 1 TRIAL 2 TRIAL 3 Volume of vinegar, mL Initial volume of NaOH, mL 1.00 1.00 1.00 14.98 22.90 30.87 Final volume of NaOH, mL 22.84 30.77 38.75 Molarity of acetic acid Average molarity of acetic acid ANALYSIS OF CARBONIC ACID IN A SODA SAMPLE TRIAL 1 TRIAL 2 TRIAL 3 Volume of soda, mL 20.0 20.0 20.0 Initial volume of NaOH, mL 20.20 22.05 23.93 Final volume of NaOH, mL 22.03 23.89 25.8 Molarity of carbonic acid Average molarity of carbonic acid
UEid- base tit ration the Consentrat ion of ammonia Solution excess HCL was titrated ith o.07om Na, cO3 Solutian. The volume of Na, Coz Solution reguired was 15.50 ml using the following eguations: 2HCLem> + Na, COgcaps CO2 Cays + HzO1) t NaCL Calculate the concentration (molarity and ppm) of ammonia in the Original Solution.(MM of NHzis 17.031.9/4) 10.0 was by of o.10OMI HCE to Then
Help me please
A solution of HCl was titrated against sodium carbonate. What is the titer for Trial 1 in the given data? T2 0.3562 0.3479 0.3042 Weight (g) Initial V (ml) 0.80 1.60 35.20 36.70 39.80 Final V (ml) Vol HCI used (ml) 35.10 N of HC (eq/L) 0.1954 0.1870 Average N of HCl (eq/L) A
How many mL of 0.2315 M sulfuric acid are required to neutralize 38.00mL of 0.189 M CH3NH2? For the toolbar, press ALT+F10 (PC) or ALT+FN+F10 (Mac). B I US Paragraph Arial 14px ABC x? X2 T T -
3. Titration: Strong Acid / Weak Base. (I warned you to be ready!) Here's the cool chart! Analyte: 20.00 mL 0.100 M Hydrazine (N₂H4) Hd A: initial Vertical (Value) Axis Title 0 B: half equivalence C: equivalence 5 10 15 20 Titrant: mL of 0.100 M HCI added 25 20.00 mL of 0.100 M hydrazine (N₂H4, pKb = 5.77) is titrated with 0.100 M HCl. a) Find the initial pH (point A) and the pH at the equivalence point (point C). b) Find the pH at the half equivalence point (point B).