Titration of 15.00 mL of a weak, monoprotic acid solution requires 22.84 mL of a 0.09837M standardized NaOH solution. What is the molarity of the acid solution? (Show your work.)
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Titration of 15.00 mL of a weak, monoprotic acid solution requires 22.84 mL of a 0.09837M standardized NaOH solution. What is the molarity of the acid solution?
(Show your work.)
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- You are working with 1.00 M NaOH. Your unknown monoprotic weak acid has a concentration of 1.960 g/L, and you are titrating 20.0 g (assume the density of the solution is 1.00 g/mL), so you have 20.0 mL of unknown acid. It takes 0.376 mL to titrate this acid to its equivalence point.1. A. How many millimoles of NaOH were delivered during this titration?Titration of 15.00 mL of a strong, diprotic acid requires 34.79 mL of a 0.1648 M standardized KOH solution. What is the molarity of the acid solution? What is the formula of the acid?(Show your work.)A different titration experiment using a 0.122M standardized NaOH solution to titrate a 26.48 mL solution with an unknown Molarity concentration (M) of sulfuric acid (H2SO4) gave the following molarities for 3 trials. Initial Burette Reading (mL) Final Burette Reading (mL) Delivered vol (mL) Acid Concentration (M) Trial 1 0.0345 Trial 2 0.0334 Trial 3 0.0381 From the 3 trials, determine the average Molarity concentration of the H2SO4 to 3 significant digits. Don't include a unit.
- You collected the following data from a titration experiment using a 0.118M standardized NaOH solution to titrate a 26.65 mL solution with an unknown Molarity concentration (M) of sulfuric acid (H2SO4). Find molarity Initial Burette Reading (mL) Final Burette Reading (mL) Vol Delivered (mL) Molarity Trail #1 0.15 19.47 19.32 ?This question is about acid base titration: Osama a student, performed an acid base titration involving a standard solution of Sodium hydroxide (NaOH) (RMM = 40) against unknown HCl solution and obtained the following results. Mass of Sodium hydroxide (NaOH) dissolved in 250 ml volumetric flask = 3.6 g 2.Volume of Sodium hydroxide used in the titration = 23 ml 3.The mean volume of HCl titrated with 25 ml Sodium…A different titration experiment using a 0.127M standardized NaOH solution to titrate a 27.67 mL solution with an unknown Molarity concentration (M) of sulfuric acid (H2SO4) gave the following molarities for 3 trials. Initial Burette Reading (mL) Final Burette Reading (mL) Delivered vol (mL) Acid Concentration (M) Trial 1 0.0358 Trial 2 0.0341 Trial 3 0.0331 From the 3 trials, determine the average Molarity concentration of the H2SO4 to 3 significant digits. Don't include a unit. From the 3 trials, determine the standard deviation of the Molarity concentration of the H2SO4 to 3 significant digits. Don't include a unit.From the 3 trials, determine the relative standard deviation of the Molarity concentration of the H2SO4 to 3 significant digits. Don't include a unit. Do you think the above experiment was accurate? Precise? Explain your answer using supporting values.
- You used the back-titration method to experimentally determine the amount of CaCO3 in an Ultra Strength Tums antacid tablet. You calculated that you used 21.5 mmol HCl to complete the titration of a 2.139 g Tums tablet. What is the mass (in mg) of the active ingredient in the Tums tablet? (CaCO3 = 100.1 g/mol)Use some or all the data below to calculate the concentration of acetic acid (in M) in the Walmart bottle. Remember 1 molecule of NaOH neutralizes 1 molecule of acetic acid. Assume you titrated a 100.00 mL solution containing 1.00 mL of the Walmart vinegar. Data: Concentration of NaOH: 0.08467 M Titrant initial buret reading: 30.21 mL Final buret reading: 38.37 mLYou have a solution of a standardized titrant of 0.01254 M and a sample that approximately has a molarity of 0.48 M. What dilution do you have to do to spend approximately 15 mL of titrant if you have 25 mL and 10 mL pipettes to take the diluted sample and value it ? Solution: With the 10 mL pipette, the sample should only be previously diluted 1:25, with the 25 mL one 1:64. Therefore, 10 mL of the sample can be taken and made up to 250 mL.
- During a titration involving 1.852 g of KHP powder, the amount of NaOH in a buret started at a reading of 3.56 mL & ended at a reading of 28.13 mL. Part B: Using the molar mass of KHP from Example 1 in the lab manual, how many moles of KHP were used in the titration?In an acid base titration lab, a student determined that a NaOH solution was 0.1885 M. The student then used this NaOH solution to titrate with an unknown H2SO4solution. 25.00 mL of the unknown H2SO4solution was pipetted into an Erlenmeyer flask. This acid required 32.55 mL of the NaOH titrant to reach the endpoint. What is the molarity of the H2SO4?H2SO4+ 2 NaOH →Na2SO4+ 2 HOH1. As the acid solution is titrated the pink color forms where the drop first enters the solution but disappears as the solution is mixed. Explain why this happens. 2. You want to standardize am NaOH solution. A buret containing NaOH solution has an initial volume reading of 0.14 mL. 25.00 mL of a 0.1000 M HCl solution is titrated to an endpoint, which occurs at a final buret reading of 27.16 mL NaOH. What is the molarity of the NaOH titrant?