Final Burette Reading Initial Burette Reading Mass of flask + water (after adding aliquot) Mass of flask (before adding aliquot) Approx. 10 mL Aliquot 10.93 mL 0.84 mL 105.49 g 95.63 g Approx. 15 mL Aliquot 25.91 mL 10.93 mL 120.28 g 105.49 g What is the density of the approx. 10 mL aliquot, in g/mL? Report your answer to the correct number of significant figures and only report the numerical value (no units).

Final Burette Reading Initial Burette Reading Mass of flask + water (after adding aliquot) Mass of flask (before adding aliquot) Approx. 10 mL Aliquot 10.93 mL 0.84 mL 105.49 g 95.63 g Approx. 15 mL Aliquot 25.91 mL 10.93 mL 120.28 g 105.49 g What is the density of the approx. 10 mL aliquot, in g/mL? Report your answer to the correct number of significant figures and only report the numerical value (no units).

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Standardization of Sodium Hydroxide Mass, KHP, g 1.0128 g Initial volume of NaOH in the buret, mL 3.30 mL Final volume of NaOH in the buret, mL 8.30 mL Volume of NaOH added, mL 5.00 mL Unknown Concentration of Vinegar Trial 1 Trial 2 Volume of acid, mL 20.50 mL 20.00 mL Initial volume of NaOH in the buret, mL 9.70 mL 8.55 mL Final volume of NaOH in the buret, mL 30.30 mL 28.25 mL Volume of NaOH added, mL 20.6 mL 19.70 mL Use the equation shown to calculate the concentration of the sodium hydroxide from the standardization data. NaOH(aq) + KHP(s) → KNaP(aq) + H2O(l) 2. Calculate the concentration of your acetic acid sample for each trial. What is the average concentration?
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
Your lab group needs to make 25.0 mL of a 2.5 M Cu(NO3)2 solution, which piece of glassware should be used to accurately measure the 25.0 mL solution? 25.0 mL Volumetric Flask 25.0 mL Beaker 25.0 mL Erlenmeyer Flask 25.0 mL Graduated Cylinder
Q) A student misreads the directions and adds 4.0 g of benzoic acid instead of 0.4 g. What do you expect to happen? Would the experiment still be valid? Explain your reasoning. Pure Lauric Acid Lauric Acid + 0.4 g Benzoic Acid Lauric Acid + 0.5 g Benzoic Acid Mass of Lauric Acid 3.03g 3.00g 3.00g Mass of Benzoic Acid 0 g 0.40g 0.50g Freezing Point 43’C 39’C 38’C Freezing Point Depression * 4’C 5’C Molality of Benzoic Acid in Lauric Acid* 1.026 mol/kg 1.282 mol/kg Moles of Benzoic Acid * 0.003 moles 0.004 moles Experimental Molar Mass of Benzoic Acid * 133.3g/mol 125 g/mol Average Molar Mass * 129.15g/mol Percent Error * 5.75%
Q10: what is the correct answer choice
Sample 1 Sample 2 Sample 3 Mass of Erlenmeyer Flask (g) 24.33 24.37 24.44 Mass of Erlenmeyer Flask + Calcium Hydroxide Solution (g) (g)(lime water) 27.22 27.29 27.33 Mass of Calcium Hydroxide Solution (g) 2.89 2.92 2.89 Volume of Ca(OH)2 Density = 1.000 g/mL 2.89 2.92 2.89 Concentration of HCl (M) 0.1 0.1 0.1 Initial HCl Volume in Syringe (mL) 1.00+1.00 1.00+1.00 1.00+1.00 Final HCl Volume in Syringe (mL) .72 .66 .54 Volume of HCl Delivered (mL) 1.28 1.34 1.46 Moles of HCl Delivered Moles of OH- in Sample Moles of Ca2+ in Sample Molar Solubility (M) Calculated Ksp Average Calculated Ksp I am very confused how to solve the blank spots in the table. Everything including and after "Moles of HCl Delivered" confuses me. Please help me figure out how to solve the sections correctly. Also feel free to…
Equal volumes of Solutions 2 and 3 were mixed in the lab. Suggest a measurement that could be made in the lab to provide evidence that a chemical reaction occurred when Solutions 2 and 3 were mixed.
0.10 M formic acid (HCHO₂) Ka = 1.8 x 104 0.10 M sodium formate (NaCHO₂) 0.10 M acetic acid (HC2H302) Ka = 1.8 x 10¹5 0.10 M sodium acetate (Na C₂H30₂) 0.10 M carbonic acid (H₂CO3) Ka = 4.3 x 107 0.10 M sodium bicarbonate (NaHCO3) 0.10 M KOH 0.10 M HCI 0.10 M boric acid (H3BO3) Ka = 5.8 x 10-10 0.10 M sodium borate (NaH₂BO3) 4. Which reagents listed above should be mixed to result in a buffer of about pH 6-8?
Use sig figs
Part B A chemist has a bottle containing 0.57 M CuCl2. How many milliliters of this solution should the chemist use to add 2.0 grams of CuCl2 to her reaction? 3.5 mL 26 mL 13 mL 0.015 mL