8. The following titration data was collected in a lab. Based on the results, determine the concentration of the aqueous sulfuric acid acid. Concentration of NaOH used: 0.50 M Volume of NaOH used: 50.0 mL Indicator: phenolphthalein Endpoint color change: olorless to pale pink Table 1 Volume of sulfuric acid Required Burette reading (mL) Trial 1 Trial 2 Trial 3 Final reading 31.28 39.17 46.70 Initial reading 1.18 9.08 16.62 Volume H:SO4 used (mL)
Q: a. Assuming that the acid is a strong monoprotic acid, what is the molarity of the acid? b.…
A:
Q: Buffer 1: Using a graduated cylinder measure out 20.0 mL of 0.10 M acetic acid. Using a pipet, pipet…
A: For buffer 1, 20 ml of 0.10 M acetic acid mixed with 25 mL of 0.10 M sodium acetate in 100 ml beaker…
Q: Na2CO3 + HCl -> NaCl + NaHCO3 Na2CO3 served as the primary standard in a titration experiment. Find…
A:
Q: A titration was performed to find the concentration of hydrochloric acid and the following results…
A: Accuracy is defined as the closeness of a measured value to a standard or known value. Precision is…
Q: A 25.0 mL sample of a solution of a monoprotic acid is titrated with a 0.115 M NaOH solution. The…
A: Given , A sample of monoprotic acid is titrated with NaOH solution .
Q: 1. Dilution of NaOH Solution: Molarity of NAOH stock solution ..1000M wwwwwwww wwww www Volume of…
A: 1. Dilution of NaOH solutions : M1 = initial concentration of NaOH = 1000M V1 = initial volume =…
Q: In a test tube with 0.3 mL of N-methylaniline, 5 mL of 10% NaOH, 0.4 mL of benzene sulfonyl…
A: the solution is as follows:
Q: A 0.6423 g sample that might contain NaOH, Na₂CO₃, NaHCO₃, or a permissible mixture of the bases is…
A: NaOH is a strong acid, so first it will be completely neutralised by the strong acid HCl. The…
Q: Determine the pH at one-half of the equivalence point. Express your answer to two decimal places.…
A: The pH at the half of the equivalence point, at the equivalence point and the after adding 6.0 mL of…
Q: The flask contains 10.0 mL10.0 mL of HClHCl and a few drops of phenolphthalein indicator. The buret…
A: Given, The Volume of HCl = 10.0 mL. The molarity of HCl = x. The Volume of NaOH = 31.1 mL. The…
Q: Introduction to Volumetric Analysis A 0.095g sample of oxalic acid dihydrate is titrated with NaOH…
A: Given the mass of oxalic acid dihydrate, H2C2O4.2H2O(s) = 0.095 g Molar mass of oxalic acid…
Q: Use a primary standard to determine an unknown concentration using an acid-base titration. Potassium…
A: When KHP and barium hydroxide react with each other,then Following balanced Chemical Reaction…
Q: Calculate the pHpH at the equivalence point for titrating 0.240 MM solutions of each of the…
A:
Q: To plot the deformation curve resulting from 10 mL of 0.1 normal sodium hydroxide with 0.1 normal…
A: Equivalence point is the point of titration at which amount of titrant added totally neutralizes the…
Q: Consider the titration curve for aqueous 0.5M NaOH treatment of acid. The pH at the equivalence…
A: The above graph is showing weak acid vs strong base for simple identification here observe the lower…
Q: 8. A 25.00 mL HCl of unknown molarity was titrated against 0.8339 M NaOH. Based on the following…
A: Number of moles of solute present in 1L of solution is known as molarity of the solution. Molarity…
Q: how many moles of weak acid are present in this solution?
A: Given: volume=2.44000×101 mLmolarity=2.12000×10-1 M
Q: From the 3 trials, determine the average Molarity concentration of the H2SO4 to 3 significant…
A:
Q: Express the concentration of acetic acid in both samples as % by mass of acetic per 100mL of…
A: A numerical problem based on quantitative analysis, which is to be accomplished.
Q: Just fill out Table 1 by writing “+” if the compound is soluble/miscible in the solvent. Otherwise,…
A: "Like dissolves like" is the thumb rule for dissolution of solute in solvent. This means highly…
Q: Use a primary standard to determine an unknown concentration using an acid-base titration. Potassium…
A: The balanced chemical reaction between barium hydroxide and KHP is Ba(OH)2 + 2KHP → Ba(KP)2 + 2H2O
Q: Which of the following steps MUST be done prior to titration of an analyte? I. Prepare a…
A: Steps done prior titration.
Q: 14 9 Hd 7 A pka of the indicator D C B negligible volume difference Vbase Titration of a Strong Acid…
A: A titration curve is drawn by taking Volume of titrant added on X axis and pH on Y axis.
Q: A substance contains 0.5 g of magnesium hydroxide as the only basic ingredient . The sunstamce is…
A: Given: Mass of magnesium hydroxide i.e. Mg(OH)2 in 1 tablet = 0.5 g Concentration of stock HCl…
Q: The graph shows the titration of the aqueous solution containing 0.138 g of unknown monoprotic acid…
A: For a monoprotic acid and NaOH , first we right a balanced reaction. At equivalence point , acid and…
Q: Calculate the volume in milliliters of 0.362 M KOH necessary to titrate 28.38 mL of 0.279 M diprotic…
A: Chemical reaction between KOH and H2SO4: 2KOH + H2SO4 → K2SO4 + 2H2O From…
Q: t is time for the titration. You measure 15.0 mL of the H2C2O4 solution with a 100-mL graduated…
A: The titration is carried out between oxalic acid solution and sodaium hydroxide solution. The…
Q: The correct indicator was added to 25.00 mL of a 0.1340 M solution of pentanoic acid (CH3(CH2)3CO0H)…
A: Pentanoic acid is titrated with NaOH.
Q: The following titration data was collected by a students in CH1031. Based on the results, determine…
A: Data given: The concentration of NaOH used, M1 = 0.25 M The volume of NaOH used, V1 = 25.0 mL
Q: 4. In an experiment to determine the concentration of an HCCI sample of unknown concentration, 0.1 M…
A: The concentration of unknown solutions is calculated by using the process of titration. The…
Q: 50 mL sample solution containing Na2CO3 and NaOH is titrated with 0.2 M HCl solution. In the…
A: In the presence of phenolphthalein, NaOH is titrated by hydrochloric acid whereas in the presence of…
Q: it is time for the titration. You measure 15.0 mL of the H2C2O4 solution with a 100-mL graduated…
A: The addition of solution of a known concentration to a solution having unknown concentration of…
Q: only SELECT correct respomses 1) Titrations of different forms are often employed to quantitate…
A: Correct responces are 1 2 3 5 6 7 8 9 11
Q: 25.0 mL aliquots of acidified tin(II) iodide are titrated with 0.396 mol/L of potassium dichromate.…
A: Working formula: volume*Molarity = no of mmol the balanced chemical reaction is as follows: 2…
Q: researchers titrated a 100mL solution of 0.1M glycine at pH 1.72 with 2 M NaOH solution. She then…
A:
Q: A 125.0 mg sample of an unknown, monoprotic acid was dissolved in 100.0 mL of distilled water and…
A: The graph point where slope will be zero then point will be the equivalence. The pH value is…
Q: measured pH of 0.100 M maleic acid with an initial volume of 25.00 mL as it is titrated with a…
A: Given: Maleic acid= 0.100 MMaleic acid initial volume = 25.00 ml titrated with strong base 0.100 M…
Q: olphthalein (9.9) Resazurin (5.1) Phenol Red (7.4) This is a lab where strong acid is titrated by a…
A: Indicators are used for indicating the pH changes that occur in the substances upon addition of…
Q: A different titration experiment using a 0.122M standardized NaOH solution to titrate a 26.48 mL…
A: Molarity of trial 1 = 0.0345 M Molarity of trial 2 = 0.0334 M Molarity of trial 3 = 0.0381 M Average…
Q: Buffer 1: Using a graduated cylinder measure out 20.0 mL of 0.10 M acetic acid. Using a pipet, pipet…
A: A buffer is an aqueous solution that resists change in pH value on addition of small amount of acid…
Q: The following titration data was collected by a students in CH1031. Based on the results, determine…
A: Given that :
Q: (4). A buret in the “The soluble chloride determination by gravimetry” lab is employed as ____…
A:
Q: In a test tube with 0.3 mL of Aniline, 5 mL of 10% NaOH, 0.4 mL of benzene sulfonyl chloride. Add a…
A: the answer is as follows:
Q: An 20.00 mL unknown solution required two indicators for titration. The first indicator reaches its…
A:
Q: From the graph find equivalence point, determine pH at half-equivalence point. Calculate Ka value of…
A:
Q: An 20.00 mL unknown solution required two indicators for titration. The first indicator reaches its…
A: As per the given problem, 20.00 mL of the unknown solution requires two indicators for titration.…
Q: Calculations for Acetate Buffer Solutions 2. Molarity of sodium acetate in acetate buffer. 2.…
A: Molarity is defined as the moles of solute present per unit volume of solution. It is a way of…
Q: 50 mL sample solution containing Na2CO3 and NaOH is titrated with 0.2 M HCl solution. Acid…
A: In the presence of a strong base (NaOH) in the mixture of Na2CO3 and NaOH, HCl first reacts with…
Step by step
Solved in 3 steps
- A 10.00-mL aliquot of a known HCl solution (3.800 g/L) was titrated with a 4.100 g/L NaOH solution. Calculate the range of the blank corrected titration volumes using the titration data below: Blank Trial 1 Trial 2 Trial 3 Initial Volume (mL) 12.50 0.50 12.30 34.75 Final Volume (mL) 13.10 10.45 22.35 45.27100 mL water sample was subjected to DO analysis using the Winkler method. The initial reading of the titrant (0.025 M Na2SO3) in the buret was 2.51 mL. The endpoint was obtained and the final reading was 7.07 mL. A blank was also titrated and 0.75 mL of the titrant was consumed. Compute for the amount of DO (mg/L) in the sample.A50.0 mL aliquot of solution contairing 0.450 g of MgSO4 [FM 120.27) in 0.500 L required 376 mL of EDTA solution for titration. How many miligrams of CaCO3 (FM 106.09) will react with 100 mL of this EDTA solution?
- concentration of I3- : 0.002M d. Titration data: Final volume: 29.05 mL Starting volume: 38.10 mL Delivered volume: 25.15 mL How do you calculate g?. 100 ml boiled cooled and filtered water sample takes 9.6 ml of M/50 EDTA in titration. The Permanent hardness of the water sample in terms of ppm of CaCO3 equivalent isA dilute peroxide solution was prepared by quantitatively diluting 10 mL stock H2O2 (MW = 34.0147) to 250mL using a volumetric flask. 50 mL aliquot of the diluted peroxide solution was titrated using the previously standardized KMnO4 in problem 1. Titration of the sample required 29.00 mL titrant and the blank containing 50 mL 1:5 H2SO4 required 0.75 mL of the standard KMnO4. Calculate the concentration in %w/v of the stock H2O2. (Hint: H2O2 produces O2 under acidic condition). Follow sig. Fig
- Determine the relationship between the observed/apparent value (EX) VERSUS that of the true value (ET) for the quantity being sought by writing either <, >, or = on the space provided Determination of water hardness using complexometric titration. During sample analysis (ppm CaCO3), the volume for blank correction was not subtracted to the volume of titrant. EX Blank 1 ET7. For aldehydes, a common quantification method is: A) Polarimetry B) Iodometry (back titration) C) Iodometry (direct titration) D) Alkalimetry after preliminary acid hydrolysisWhat is the concentration of Mn2+ in a solution with an analytical MnY2- concentration of 0.025 M at pH7? Kmny = 6.2 x 1013 a4 = 4.8 x 10-4 A 9.2 × 10-7 M B 8.4 × 10-13 M C 4.0 × 10-16 M D 2.0 × 10-8 M
- H8. a 10 ml sample containing Ni was back titarted againat 0.0575 M EDTA. 10 ml concentrated amonia was added to the sample and 100 ml of water with 0.02 indicatore. the averge of 3 titration is 14.76667 ml. what is the Ni content g/L?If a 1.065 g sample of magnesium oxide of 84.736% were treated with 50 mL of 1.017 N sulfuric acid, what volume of 1.103 N sodium hydroxide would be required in the back titration? 1. What specific type of titration is involved? * A. Direct Acidimetry B. Direct Alkalimetry C. Residual Alkalimetry D. Residual Acidimetry 2. Which is the analyte in the problem? A. Magnesium Oxide B. Sulfuric Acid C. Sodium Hydroxide 3. What is the analyte-titrant chemical reaction involved? Weak Acid + Strong Base Weak Base + Strong Acid Strong Acid + Weak Base Strong Base + Weak Acid1) Calculate the total hardness for the first sample (Sample Volume,V : 50 mL,Volume of EDTA titrant used for the sample, A:9.6 mL) 2)Calculate the calcium and magnesium concentrations for the first sample in the video in meq/L and mg CaCO3/L.(Sample Volume= 50 mL, Magnesium hardness titrant volume = 0 mL, Calcium hardness titrant volume:2,6 mL) 3)Assuming the pH and alkalinity of the first sample in the video are 7.5 and 100 mg CaCO3/L, respectively, calculate the temporary and permanent hardness values for this sample 4How much CaCL2 in meq/L should be added to the sample to equalize calcium and magnesium hardness? Which hardness level (soft, medium, hard, very hard) does the sample belong to after this addition?