Two trials made in the determination of the Molarity of NaOH solution gave the following results. Trial I: 0.0986M Trial 2: 0.0979M Calculate the: 1. Mean Molarity 2. Precision in ppt 3. Molarity of HCl solution if 23.00 mL of the NaOH solution is required to titrate 30.00 mL of HCl. Please provide a solution to all 3 :)

Two trials made in the determination of the Molarity of NaOH solution gave the following results. Trial I: 0.0986M Trial 2: 0.0979M Calculate the: 1. Mean Molarity 2. Precision in ppt 3. Molarity of HCl solution if 23.00 mL of the NaOH solution is required to titrate 30.00 mL of HCl. Please provide a solution to all 3 :)

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter4: Calculations Used In Analytical Chemistry

Section: Chapter Questions

Problem 4.24QAP

See similar textbooks

Similar questions

100ml of sodium hydroxide solution is required 20ml of 0.5 N sulfuric acid solution to neutralize it. Calculate the amount of sodium hydroxide or percent purity. (mwt of sulfuric acid is 98g/mole)
The following replicate molarities were obtained when standardizing a solution: 0.1067, 0.1071, 0.1066, and 0.1050 M. Assuming no determinate/systematic errors, within what range are you 95% certain that the true mean value of the molarity falls?
A commercial base solution, NH3 has a specific gravity of 0.898. Calculate the molarity of a 28.0 % (w/w) NH3 (17.02 g/mol) solution. (Assume specific gravity has the same units as that of density)
Submit a clean, dry, and properly labeled 50-mL reagent bottle for your unknown solution. Pipet 20.00 mL of the sample in 250-mL Erlenmeyer flask. Add 5 mL of buffer and 5 drops of indicator. Titrate the solution until it turns light blue. If the titration consumes more than 50 mL of the titrant, dilute the sample accordingly. Compute for ppm of CaCO3 using the following table. Mean Molarity = 2.487 x 10^-3 MBlank correction = 0.015 Formula = V (mL) titrant x Mean Molarity of Titrant x Molecular weight of CaCO3 x 1/V (L) sample
Complete the table by entering the molarity of B2- for each standard solution. Show an illustrative calculation for tube ‘A’. Use the dilution formula and express each result to one more digit than allowed by applying the rules of significant figures. Standard Volume of stock B2- solution taken, mL Molarity of dilute B2 Construct a graph of Absorbance vs. molarity of B2- in Excel using the data in the preceding table. Make certain to title the graph and include axes labels with proper units. Absorbance is dimensionless (has no unit). Add a linear trendline to the graph but do not set the y-intercept to zero Solid M2B is added to 25 mL of water, the resulting mixture is continually stirred for 1 hour. At this point, it is assumed that equilibrium (eqn 3) has been established. The mixture is transferred to a test tube, and the test tube is centrifuged to assure that any residual solid M2B is fully settled out. A portion of the supernatant in the test tube is carefully…
How much amount of solids (in grams) do you need to prepare the following solutions? Preparation of SolutionsPrepare the following solution quantitatively using boiled distilled water per class:1. 250.0 mL 1.0 M stock HCl solutionNOTE: Use the 3.0 M HCl solution from Solution Preparation experimentPrepare the following solution quantitatively using boiled distilled water per group:1. 250.0 mL 0.0500 M standard HCl solution from 1.0 M HCl
What molarity of HCI stock solution is needed so that 2.5mL of this stock solutiondiluted to 0.025L will yield 25mM?
A metal, M, of atomic mass 56 amu reacts with chlorine to form a salt that can be represented as MClx. A boiling point elevation experiment is performed to determine the subscript ?, and therefore, the formula of the salt. A 35.5 g sample of the salt is dissolved in 100.0 g of water and the boiling point of the solution is found to be 377.45 K. Find the formula of the salt. Assume complete dissociation of the salt in solution.
42.5 mL of 1.3M KOH are required to neutralize 50.0 mL of H2SO4. This sulfuric acid is further used to standardize NaOH solution. 20mL aliquot of the NaOH solution is obtained and 2 drops of phenolphthalein is added. The initial reading on the buret is 13.2 mL. After the titration, the exact normality of the NaOH solution is found to be 1.254N. (a) What is the molarity of H2SO4? (b) How much of the sulfuric acid is used? (c) What is the final reading on the buret?
In which situation(s) is it necessary to use a volumetric flask for maximum accuracy? to prepare a 0.150M solution of sodium chloride to measure ~25mL of water to prepare 0.1M HCI from 36-38% HCI a and c all of the above (Please type answer no write by hend)
The total cation content of natural water is often determined by exchanging the cations for hydrogen ions on a strong acid ion-exchange resin. A 25.00 mL sample of a natural water was diluted to 100.00 ML with distilled water, and 2.06 g of a cation - exchange resin was added. After stirring, the mixture was filtered and the solid remaining on the filter paper was washed with three 15.00 mL portions of water. The filtrate and washings required 16.30 mL of 0.0282 M NaOH to give a bromocresol green end point. a) Calculate the number of millimoles of cation present in exactly 1.00 L of sample. b ) Report the results in terms of milligrams of CaCO3 per liter. Only typed solution.
Identify if there are any errors in the solutions, and state what they are. Thanks