Volume of sulfuric acid in sample (ml) Initial burette reading (ml) Final burette reading (ml) Total volume of 0.25 mol/L KOH added (ml) Average Volume of KOH added (mL) Trial 1 25.0 0.0 19.8 Trial 2 25.0 19.8 39.4 Trial 3 25.0 0.3 20.0
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A student wants to determine the unknown concentration of a sample of sulfuric acid.
She performs a titration between her sample of sulfuric acid and potassium hydroxide and collects the data below.
Determine the unknown concentration of sulfuric acid.
Step by step
Solved in 4 steps
- Sucrose solution for experiment 1: (Question a-c)Prepare a solution of sucrose by accurately weighing 9.0 – 9.25 g of sucrose into a 100mLbeaker / conical flask. Record the mass of the sample. Add 25 mL distilled water. Mix until allcrystals dissolve.NaCl solution for experiment 2: (Question d-f)Prepare a solution of NaCl by accurately weighing approximately 1.5 g of NaCl into a 100 mLbeaker / conical flask. Record the mass of the sample. Add 25 mL distilled water. Mix until allcrystals dissolve.MgCl2٠6H2O solution for experiment 2: (Question d-f)Prepare a solution of magnesium chloride by accurately weighing approximately 3.6 g ofMgCl2٠6H20 into a 100 mL beaker / conical flask. Record the mass of the sample. Add 25 mLdistilled water. Mix until all the crystals dissolveYou 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). Initial Burette Reading (mL) Final Burette Reading (mL) Vol Delivered (mL) Acid Concentration (M) Trail 1 0.15 19.47 ? ? Trail 2 0.18 17.3 Trail 3 0.17 18.05 State the volume delivered and acid concentration for just the first trail. Use significant digits.Please put your observations in data table part 2 and answer the post lab questions(1-5) AND 6 A AND B and for number 7 ONLY DO THE EQUATIONS FOR 11 12 AND 13 I MARKED ON THE WORKSHEET BUT ONLY DO EQUATION FOR HCI WITH CUSO4 AGNO3 AND FE2SO4 I KNOW I DID IT BUT I MAY BE WRONG
- Why is NaOH(s) to be taken out and weighed only when you are ready to make measurements? Group of answer choices NaOH does not need special treatment. NaOH reacts violently so is prepared last. NaOH is hygroscopic NaOH burns holes in the weighing paper.A student creates a calibration plot for serial dilutions of Cu(NO3)2. A graph of concentration in M (x-axis) versus absorbance (y-axis) gives a linear trendline of y = 0.345x - 0.11. Copper(II) nitrate has a solubility of 83.5 g in 100 g of water. Calculate the percent error in the student's concentration.Convert each "b" value from the three Graphs ln(Conc) to the Initial Concentration. Graph Two: y= -0.0048x -11.125 Graph Four: y= 161824x - 13.326 Graph Five: y= -0.0189x -10.903 **Note these are the y= mx-b equation from the linear graph, In(concentration) vs time. I don't know how to convert natural log value such as -11.125 to the initial concentration.
- Assignment: This is an individual activity. After studying the lesson and watching all the videos, answer the following questions. Answer in not more than 3 sentences per question. 1. Discuss the a) direct method of weighing b) indirect weighing using the analytical balance. 2. Explain how suction filtration is carried out in the laboratory. Give the important points that must be observed in doing the process. 3. Explain why it is important to wash the precipitate. Can distilled water be used to wash all types of precipitates? 4. Discuss how to use a desiccator. When should a desiccant be replaced?An environmental scientist obtained the following replicate concentration measurements of methane (CH4) gas at a landfill site: Replicate Measurements CH4 Concentration (mg/m3) 1.0 0.1571 2.2 0.2031 3.0 0.1914 4.0 0.2103 Calculate % error when the scientific community accepts 0.2102 as true value.Data obtained: Chips # of extractions Chips' weight (g) Fat weight (g) Regular 3 20.043 6.745 3 20.187 6.438 3 20.198 7.451 Low fat 3 19.456 3.982 3 20.072 4.547 3 20.192 4.589 Mass percent is a method of expressing the concentration of a substance in a mixture or element in a compound. It is calculated as the mass of the component divided by the total mass of the mixture and then multiplied by 100 to get the percent. The formula is: mass % of component= (mass of component / total mass) x 100% 1) Reproduce the following table, and use the data to determine the mass % of fat in the chips for each trial. 2) Show one example calculation. Chips Trial % by mass of fat Regular 1 2 3 Lowfat 1 2 3
- Which analytical separation method is best for recovering river bodies that are polluted by heavy metals and particulate matter. Explain your analytical process of choice.Part 1 – Preparation of CaCO3(s) The following is a procedure that was theoretically performed by a student. Read through the procedure and answer the questions below. A 10.0 mL graduated cylinder to measure 10.0 mL of a 1.00 M CaCl2 solution into an initially empty 50.0 mL beaker. A 50.0 mL graduated cylinder was then used to measure out 25.0 mL of 0.500 M K2CO3. This K2CO3 solution was then added to the beaker containing the CaCl2 The solution became cloudy, and the student concluded that a precipitate must have formed. Write a balanced chemical reaction below, including phases, and identify the chemical formula of the precipitate: Answer the questions below as part of Data Analysis. 1. What is the actual yield of the product? 2. Using stoichiometry, calculate the limiting reactant, and the theoretical yield (the mass of CaCO3 product) for the reaction. 3. Determine the percent yield of the reaction.You have finished two trials of the sample analysis for the experiment and you noticed that the burette is almost empty (~5 mL remaining). Should you add more titrant before the next sample analysis or not? Why or why not? Select one: YES. It will not affect the calculations and not cause error NO. It will affect the calculations and cause error Neither A nor B Cannot be determined