Calculate the molarity of the original vinegar solution and its concentration in gdm-3, given that it reacts with NaOH in a 1:1 ratio. 7. 2.5 g of a sample of ethanedioic acid, H2C2O4.nH2O, was dissolved in water and the solution made up to 250 cm3. This solution was placed in a burette and 15.8 cm3 were required to neutralise 25 cm3 of 0.1 moldm-3 NaOH. Given that ethanedioic acid reacts with NaOH
Section 3: The titration of an unknown concentration of HCl with the standard solution of NaOH. Section 4: Use the HCl solution titrate a commercial basic product and determine the quantity of active ingredient. -Section1: Preparation of a Standard Sodium Hydroxide Solution Materials 250-mL volumetric flask Weigh scale Weighing bottle, or watch glass for NaOH sample, Glass funnel Dropper pipette 100 ml beaker Deionized water NaOH solid Procedure 1. Weigh approximately 1 gram of NaOH in a weighing bottle. Record the actual mass (1.01 grams weighed) in the results table.
In the first part, five 100 mL flasks of 5 mL ligand solution, 5 mL 2 M sodium acetate, 4 mL 3 M NH2OH, and 1-5 mL Fe2+ solution are diluted with water. The absorption spectrum for varying concentrations of Fe2+ are measured using a spectrophotometer and the data is graphed in Excel. The slope of the line is ε in the Beer-Lambart equation A = εcl. In the second part of the experiment, eleven flasks containing diluted stock solutions of Fe2+ and ligand are mixed with 5 mL 2 M sodium acetate and 4 mL 3 M NH2OH and diluted with water. The absorption spectrum is measured using a spectrophotometer and the data is graphed in Excel.
20. mol H2 reacts with 8.0 mol O2 to produce H2O. Determine the number of grams reactant in excess and number of grams H2O produced. Identify the limiting reactant. 8.1 g H2 , 2.9 x 102 g H2O 17. How many litres of O2 gas are required to produce 100. g Al2O3?
Percent H2O in Hydrate is equal 0.34/2.33=14.6% 3. The general formula of barium chloride hydrate is BaClg-nHZO, where n is the number of water molecules. Calculate the theoretical percent water for each value of n—divide the sum of the atomic masses due to the water molecules by the sum of all the atomic masses in the hydrate, and multiply the result by 100. Complete the table. | BaCl2 | BaCl2•H2O | BaCl2•2H2O | BaCl•3H2O | Sum of atomic masses (BaCl2) | 208.23 | 208.23 | 208.23 | 208.23 | Sum of atomic masses (nH2O) | 0 | 18.02 | 36.04 | 54.06 | Sum of atomic masses (hydrate) | 208.23 | 226.25 | 244.27 | 262.29 | Percent water in hydrate (theoretical) | 0% | 7.96% | 14.75% | 20.61% | In this lab we used a Balance, centigram
* 3. 3.0 ppm standard: * 3.00 mL of 10.0 ppm phosphate solution was placed in a 25 mL graduated cylinder and diluted to exactly the 10 mL mark with distilled water then poured into a plastic cup labeled 3. Cylinder was rinsed with distilled water. * * 4. Zero standard: 10 mL of distilled water was poured into a plastic cup labeled 0.
Solution Stoichiometry and Gas Law Problems Problem 1 In flask A, 1.500g of silver nitrate solid is dissolved in 50.0mL of water, while in flask B, 0.500g of potassium carbonate is dissolved in 25.0mL of water. The two solutions are then mixed together. a) Before mixing, what is the molarity of each solution? b) Write the balanced molecular equation, the complete ionic equation, and the net ionic equation for the reaction. c) If the percentage yield is 85.0%, what mass of precipitate is actually produced?
The resulting product was [Co(NH3)5Cl]Cl2 and yield was 4.453g (.017 mol, 84.8%) Distilled water (25mL) was added to concentrated ammonia (5mL) in a 125mL Erlenmeyer flask. The reaction was heated and stirred, then [Co(NH3)5Cl]Cl2 (.0060 mol) was added to the solution. The reaction mixture was vacuum filtered, and the filtrate was cooled in an ice bath. 6M HCl was then added until the solution was neutral to litmus. NaNO2 (.0217 mol) was added to the solution and was allowed to react for five minutes.
CaCO3 + 2HCl -----CaCl2 + CO2 + H2O ( Volume of acid added (L) ) (1.0mol/L) = moles acid added. Moles acid added - moles base added = moles acid that reacted. Moles of acid that reacted / 2 = moles CaCO3 present in sample. Final answer % CaCO3 3. Put exactly 5.0 mL of water in the 10.0 mL graduated cylinder.
The mechanism for the reduction of a ketone by sodium borohydride: (1) Method (Based on Chemistry Laboratory Manual): 1. 0.4510g of benzophenone was dissolved in 5 cm3 of ethanol in boiling tube containing a magnetic stirrer bar. 2. O.1249g of sodium borohydride was added and left for 30 minutes. 3.