Chem1011GeneralChemistryII_TitrationforAceticAcidinVinegar_134692

What is the molarity of an aqueous solution that contains 0.0720 g C2H6O2 per gram of solution . The density of the solution is 1.04 g/mL X STARTING AMOUNT ADD FACTOR ANSWER RESET *( ) 1.04 62.08 6.022 x 1023 0.0720 1.21 x 10-3 4650 1.12 1000 1.21 1 0.001 g C2H.O2 mol C2H6O2 g C2H&Oz/mol g solution/mL mL solution g C2H6O2/g solution M C2H6O2 L solution g solution

Pre Lab Questions: (Each answer is to be written as a complete sentence) What is the reason for washing the precipitate with water in Step 9? Define precipitate. Define filtrate. In Step 2, what is the purpose for rinsing the stirring rod? read the Procedure to answer the questions  Using a balance, mass between 1.50 – 2.00 grams of sodium carbonate in a pre-massed 150mL beaker. Add 20 mL of distilled water and stir thoroughly to make sure all the crystals are dissolved. Rinse the stirring rod with a little distilled water after stirring. Using a balance, mass between 1.50 – 2.00 grams of calcium chloride dihydrate in a pre-massed 50 mL beaker. Repeat Step 2 for the solution in the 50 mL beaker. Pour the calcium chloride solution into the 150mL beaker containing the sodium carbonate solution and stir. Mass a piece of filter paper. Fold the filter paper and place it into the funnel. Wet it with a little distilled water to ensure that it is stuck to the sides of the funnel. Slowly…

3 Solid ammonium bromide is slowly added to 75.0 mL of a 0.283 M silver nitrate solution until the concentration of bromide ion is 0.0583 M. The percent of silver ion remaining in solution is %. Submit Answer $ 4 R F % 5 Use the References to access important values if needed for this question. Retry Entire Group 5 more group attempts remaining T G Cengage Learning | Cengage Technical Support ^ 6 MacBook Pro Y H & 7 U J * 00 8 1 ( 9 K O < ) O L P Previous Email Instructor + = Next Save and Exit

STARTING AMOUNT X = 0.1 A student dissolves 24.3 g Na2S₂O3 in enough water to make a 0.302 solution. How many mL solution did the student make? ADD FACTOR x( ) 0.302 24.3 509 1 DELETE 6.022 x 10²3 0.509 L solution g Na₂S₂O3 A 158.1 ANSWER 1000 0.001 1.965 0.01 M RESET 5 3.311 100 M Na2S₂O3 kg Na₂S₂O3 mol Na2S₂O3 mL solution 10

16 You need to make an aqueous solution of 0.237 M cobalt(II) fluoride for an experiment in lab, using a 250 mL volumetric flask. How much solid cobalt(II) fluoride should you add? grams Submit Answer Review Topics] [References] Use the References to access important values if needed for this question. Retry Entire Group 8 more group attempts remaining Cengage Learning Cengage Technical Support Previous Next> Save and Exit

Quantity Your Data 1.   Grams of vinegar sample used for your titration 25.000 g 2. Initial Buret Reading of Sodium Hydroxide solution 10.00 mL 3. Final Buret Reading of Sodium Hydroxide solution 28.00 mL 4. Amount of Sodium Hydroxide Solution used to neutralize the vinegar sample   5. Concentration of NaOH in the NaOH solution 0.050 g/mL 6. Grams of NaOH used to neutralize the vinegar   7. Grams of acetic neutralized by the amount of NaOH   8. Percent acetic acid in the vinegar   Hints:     For #4, The amount of NaOH used is the difference between the starting buret value and the ending buret value.   For #6, Once you calculate the amount of sodium hydroxide used, multiple that value by the concentration of NaOH in the NaOH solution.   For #7, Multiply the value obtained in number 6 by the number 1.5.  Remember, we learned that every 1 gram of NaOH neutralizes 1.5 grams of acetic acid.   For #8, Divide the grams of acetic acid by the grams of vinegar sample and multiply this value by…

Tools Window Help View History Bookmarks ... 71% D Fri 3:25 PM A writing.citationmachine.net Editor 101 Chem101 Calculate the volume of CO, ga: X + e Share -> 8 https://app.101edu.co ate Sensitivit Question 13 of 13 Submit Gra Plag When excess water is added to a mixture of citric acid and sodium Expe bicarbonate present in a bath bomb, the following reaction takes place C6H&O7(s) + 3 NaHCO3(s) + H2O(1) → Na3C6H;07(aq) + 4 H20(1) + 3 CO2(g) Calculate the volume of CO2 gas collected over water at 38.0 °C when a mixture of 55.5 g of citric acid and excess sodium bicarbonate is added to a tub of water if the total pressure is 725 torr. The vapor pressure of water at 38.0 °C is 49.7 torr. L 4 6 C 7 8 +/- x 100 O Focus General 书 1263 words English (United States) 2450 word: Page 2 of 5 Page 1 of 7 Page 1 of 3 816 words tv NOV 19 MacBook Air DII F10 F9 80 888 FB F7 F6 F5 F4 esc F2 F3 | & 3. 1,

A student performed titration to find the concentration of acetic acid. Titrant was sodium hydroxide. He went beyond the indicator color change by adding too much titrant. How will his experimental error affect the calculated value for the concentration of unknown acetic acid? calculated value actual value. calculated value < actual value calculated value = actual value. more information is necessary this is not a source of error

1. Solubility Test Table 1. Results for the solubility test. OBSERVATION* INFERENCE SAMPLE Ethyl acetate ** Нехаne Methanol Water Coconut oil Vitamin E Beef fat Miscible (soluble) or immiscible (insoluble) ** polar or nonpolar Sudan IV Test Table 2. Results for Sudan IV test. OBSERVATION* INFERENCE SAMPLE Нехаne Ethyl acetate Methanol Water ** Coconut oil Vitamin E Beef fat Homogeneous or heterogeneous mixture ** polar or nonpolar

1. 500.0 mL 0.2 M KI2. 500.0 mL 0.2 M KCl3. 500.0 mL 0.1 M K2S2O84. 500.0 mL 0.1 M K2SO45. 500.0 mL 4.0 mM Na2S2O3 (from Na2S2O3∙5H2O)pls compelete the 2nd table given the data

A 21.47-mL sample of hydrochloric acid solution requires 35.00 mL of 0.109 M sodium hydroxide for complete neutralization. what is the concentration of the original hydrochloric acid solution? Submit Answer Try Another Version 2 item attempts remaining Previous Next Save and Exit Cengage Learning | Cengage Technical Support

Pre-lab question #8: Suppose you were dissolving a metal such as zinc with hydrochloric acid. How would the particle size of the zinc affect the rate of its dissolution? As the particle size of the zinc increases, the rate of dissolution AA (decreases/increases).

31 Name Date Lab Section Results and Discussion - Experiment 3 - Acids and Bases: Analysis A. Analysis of vinegar 1. Unknown vinegar number $1- 10716 feR=103.63 fl:112.2 f2=108.4 2. Mass of flask %3D 3. Mass of flask + 5.00 mL of vinegar %3D 4. Mass of 5.00 mL of vinegar 5. Density of vinegar Oo\M 6. Molarity of sodium hydroxide solution Titrations flask 1 flask 2 flask 3 41.7 7. Final buret reading 8. Initial buret reading 41.7 41.7 9. Volume of NAOH soln. 10. Moles of NaOH 11. Moles of acetic acid 12. Molarity of acetic acid 13. Average molarity of acetic acid in vinegar 14. Deviation of each molarity from average 15. Average deviation of molarity (see Expt. 4) 16. Mass percent of acetic acid in vinegar (show calculations below) O 2015 Cengage Learning. All Rights Reserved. May not be scanned, copied or duplicated, or posted to a publicly accessible website, in whole or in part.

1:06 1 | 5GE Question 22 of 25 Submit What is the molarity of an aqueous solution that contains 0.0720 g C2H,O, per gram of solution. The density of the solution is 1.04 g/mL STARTING AMOUNT ADD FACTOR ANSWER RESET *( ) 1.21 0.0720 g C2H,O2/mol 1 1.21 x 10-3 mL solution 1.12 g C2H,O2/g solution 4650 mol C2H,O2 62.08 g solution/mL 0.001 g solution 6.022 x 1023 M C2H,O2 1000 g C2H,O2 1.04 L solution

Determination of known acid concentration     Trial 1 Trial 2 Trial 3 Volume of acid used (mL) 25 mL HCl 25 mL HCl 25 mL HCl Initial buret reading (mL) 50 mL 50 mL 50 mL Final buret reading (mL) 30 .7 mL 31.1 mL 29.3 mL Volume of NaOH used (mL) 50 mL 50 mL 50 mL Molarity of NaOH       Calculated Molarity of HCl   Show a sample calculation of HCl molarity   Average concentration of HCl from Trials 1,2, and 3   The “true” concentration of HCl is 0.10 M. The calculated average concentration of HCl is ______________M. The % error is = (???? − ?????)/????? ? 100

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Based on the data given answer questions. 1,3, and 5 please ?? Question 2 is already answered to solved 1 and 3 1. Based on your three trials, discuss the precision of your data 2. The actual concentration of the unknown is 0.200 M. (Check with instructor to ensure that this value is accurate.) Calculate the percent error based on the average molarity of your three trials. Answer: Actual Molarity= 0.200M Mcalculated = 0.1755M % error = ( [actual - calculated value]/actual ) *100 Putting values; = ((0.200 - 0.1755)/0.200 )*100 = 12.25% 3. Based on your answer to (2), discuss the accuracy of your data. 5. 80.0 mL of 0.30 M NaOH and 80.0 mL of 0.30 M HCl are mixed together. What is the approximate pH of the solution —acidic, basic, or neutral? Explain.

Name Chem Section Data Sheet determination 23°C 23°C 25°C temperature of filtered KHT solution, °C 0.04m concentration of NaOH solution, mol L- 0.04 m 0.04m KHT solution 14.9 49-5 final buret reading, mL initial buret reading, mL 49.9 volume of KHT used, mL NaOH solution 28 final buret reading, mL 10 49.8 १.१ 49.7 initial buret reading, mL 50 40mL volume of NaOH used, mL number of moles of NaOH used 0014 0014 number of moles of HT titrated .04 [HT] in KHT solution, mol L- 1.42 1.142 1.142 [K*] in KHT solution, mol L-1 solubility of KHT, mol L-1 average solubility of KHT, mol L- Ksp average Ksp

1- 17.5 mL of a 0.1050 M Na,CO, solution is added to 46.0 mL of 0.1250 M NaCl. What is the concentration of sodium ion in the final solution? Select one: a. 0.165 M b. 0.148 M C. 0.119 M d. 0.205 M e. 0.539 M Previous p Chemistry 101 Exam Jump to.

Mg3(PO4)2 BaCO3 MgF₂ Most soluble Least soluble Fe(OH)3 Answer Bank

DATA AND CALCULATIONS Show all calculations neatly on an attached sheet. Trial 1 Trial 2 Trial 3 70.6849. 68.0749 2.61g 23.25ML O.65ML 22.6mL Mass of flask + vinegar Mass of empty flask Mass of vinegar used Final buret reading Initial buret reading Volume of NaOH used Moles of NaOH used 0.00226 mol Moles of açetic acid titrated Mass of acetic acid titrated Mass % acetic acid in vinegar 5.0%

Based on this student data, calculate the average molarity of the NaOH solution. Standard: KHP = potassium hydrogen phthalate, MM 204.4 g/mol Student Data Trial 1 E KHP mL initial: NaOH mL final: NaOH 2.02 0.57 19.25 Trial 2 2.05 19.25 39.80 Trial 3 1.99 1.65 20.75

L.O Page View Read aloud V Draw A Highlight Erase A chemist tries to dissolve a solid ionic compound called "X" in water at 25°C. He adds 100 mL of water to a beaker equipped with a stirrer on a balance. While slowly adding X to the beaker, he measures the mass of X added and, at the same time, carefully watches to make sure that everything he adds dissolves. Suddenly, when he has just added a total of 2 g of X, he sees that the mixture is no longer homogeneous (i.e. some of the X remains on the bottom of the beaker and won't dissolve). He divides the 2 g of X by the 100 mL of water and obtains the value 0.02 g X/mL water. This number répresents an important physical property of X. What is it uniquely called? A) the molarity of X in water at 25°C B) the concentration of X in water at 25°C C) the mass of X in water at 25°C D) the density of X in water at 25°C E) the solubility of X in water at 25°C How would you describe the solution that the chemist prepared in Question#1? A)…

Determination of unknown acid concentration     Trial 1 Trial 2 Trial 3 Unknown Acid number Volume of acid used (mL) 25 mL 25 mL 25 mL Initial buret reading (mL) 50 mL 50 mL 50 mL Final buret reading (mL) 14.8 mL 15 mL 14.5 mL Volume of NaOH used (mL) 50 mL 50 mL 50 mL Molarity of NaOH       Calculated molarity of HCl (M)               Show a sample calculation of HCl molarity   AVERAGE MOLARITY OF Unknown HCl Show a sample calculation of NaOH molarity

Titration of Acetic Acid CH3COOH 1) Record the exact Molarity of the freshly prepared solution of NaOH by reading the label on the bottle, include all digits provided. This is the solution that will be in the buret. MB 0.0500 M 2) Record the exact volume of acid CH,COOH that was pipetted into the Erlenmeyer 10.00 aak mL. Note the concentration is unknown and what you will solve for. (This was diluted with 50 mL of water in the Erlenmeyer flask) Trial 1 Trial 2 Trial 3 Final base (mL) 30.46 30.98 29.88 Initial basc (mL) 0.45 0.05 0.04 Total base (mL) *Molarity (M) HOOD HO "Use atoichiometry to determine the molarity of your CIHCOOH solution fromn each of trial. Show all work Including units for one. Caleulate Average Molarity

In the experiment, the amount of acetic acid in vinegar was determined by titrating with 0.1 M NaOH solution. In the analysis, three trials were performed to obtain more precise result. The table shows the initial and final burette readings for three titrations:     Initial Burette Reading (mL) Final Burette Reading (mL) Trial 1 2.9 10.6 Trial 2 10.6 18.1 Trial 3 18.1 25.7   According to the given data, calculate molarity of acetic acid in the commercial vinegar. Please be sure that your answer includes followings; a) moles of NaOH for each trial                                              b) average mole of NaOH                                                         c) average mole of acetic acid in 50 mL solution                     d) average mole of acetic acid in 250 mL solution                   e) molarity of acetic acid in vinegar.

[References] Use the References to access important values if needed for this question. You need to make an aqueous solution of 0.208 M chromium(II) acetate for an experiment in lab, using a 500 mL volumetric flask. How much solid chromium(II) acetate should you add? grams Submit Answer Try Another Version 1 item attempt remaining DELL

Lab report – investigating solubility of solids in water and interpreting the solubility curves. - Solubility Curves 150 140 130 120 NANO KNO: 110 100 90 80 HCI 70 NH,CI 60 KCI NH 50 40 NaCl 30 KCIO, 20 10 SO2 10 20 30 40 50 60 70 80 90 100 Temperature °C Use the above graph to answer the following questions. 1.What is the solubility of KCI at 80 degree С?.... 2Which solvent is used in this experiment?.. 3. What is the solubility of NH3 at 10 degree C?... 4.Which two solutes have same solubility at 60 degree C?. 5.At 90 degree C, 10 g of NH3 is dissolved in 100 g of water. Is this solution saturated , unsaturated or unsaturated ? 6.Which term is used to represent a solution in which more solute can be dissolved?... 7.--- + = solution 8.Which is the most soluble solute at 20 degree C?. 9.Identify the solute which is a gas ?. 10. What happens to the solubility of solids when temperature increases?.. Grams of solute /100 g H,O

7 Solid lead (II) nitrate is slowly added to 125 mL of a 0.190 M potassium hydroxide solution until the concentration of lead ion is 0.0547 M. The percent of hydroxide ion remaining in solution is %. Submit Answer $ 4 R LLO % 5 [Review Topics) [References Use the References to access important values if needed for this question. Retry Entire Group T Cengage Learning | Cengage Technical Support ^ 6 * 8 more group attempts remaining MacBook Pro G H 2 & 7 A J * 0 8 ( 9 UD U K F 0 ) O ◆ P | Previous Email Instructor { [ + 11 = Next> Save and Exit } ]

As part of this experiment you will need to determine the concentrations of Fe* and SCN ions present in test tubes 1-9. These values can be calculated using the volumes and concentrations provided in Tables 1 and 2 of the Equilibrium Lab - Procedure and the dilution equation (M,V1 = M2V2). Note: the solutions provided in the lab, and therefore the tables in the lab document, are the compounds used to prepare the solution. You must determine the concentration of the ions based on how these compounds díssociate in solution Complete the following table by filling the the calculated initial concentrations of each substance. Be sure to: Pay attention to significant figures • Round appropriately Use decimal notation (not scientific) Do not include units Test Initial [Fe3*] (M) Initial [SCN'] (M) Tube 1 3 4. 6. 7 8. 2.

y/ h VG y² ki tions/Interface/acellus_engine.html?ClassID=329083093# News Share files over Blu... FL-CA - Student Inf... Aar $ All Copyright © 2003-2022 International Academy of Science. All Rights Reserved. % 8 15.0 mL of 4.0 M HCI is added to 85.0 mL of water. What is the final concentration of the acid? A .706 F6 * & F7 [?] mol HCI 8 3) Thomas Jefferso... F8 MHCI DELL prt sc apush chapter 7 ma... F10 Enter home F11 end F12 Just Short Answer q... insert y g 4 delete

Based on the analysis of a vinegar solution via titration with 0.1 M NaOH. Results are as follows: Trial 1 Volume of vinegar solution used (mL) 5.00 Final burette reading (mL) 44.20 Initial burette reading (mL) 0.00 Determine the percentage mass of acetic acid in vinegar for Trial 1. The density of vinegar is 1.01 g/mL and molecular mass for acetic acid is 60 g/mol.

I had 500 mL solution of 0.300M HCI that I left on the bench. WhenI got back to lab the next day, the concentration of the solution was 0.5M. What volumne of my solution evaporated? 200 mL 300 mL 125 mL 500 mL 225 mL

Hello, I'm having issue with this question: "Set up the factor label (dimensional analysis) calculation required to determine the concentration of the NaOH solution via titration of a given amount of KHP. Include all numbers except the given mass of KHP. Use “Mass of KHP” in place of your given mass" I started by converting the mass of KHP to moles,  but I'm going wrong somewhere and not getting a correct answer because I think I'm missing numbers somewhere, but I'm not entirely sure. A picture of the titration I'm working from is also attached.

CALCULATOR COLOR THEME O ZOOM ADD NOTE QUESTI 9. How many mL of stock NH, is needed to make 100.0 mL of 1.00 M NH, if your stock solution is 14.8 M? 1.48 mL 6.76 mL 67.6 mL 1480 mL CLEAR ALL Answered 13 14 NEXT > 10 11 12 ... 6. 7 8. 3. ( PREVIOUS O Type here to search 40 5.

Based on the following SAMPLE 2 data, calculate the concentration (M) of NaOH. Report answer with FOUR decimal places. Do not include units in response. REPORT FOR EXPERIMENT 22 Neutralization-Titration I Data Table Sample 1 Sample 2 Mass of flask and KHP 94.7994 g 95.3800 g Mass of empty flask 93.6616 g 94.2144g Mass of KHP Final buret reading 18.25 mL 36.94 mL Initial buret reading 0.15 mL 18.24 mL Volume of base used

K Question 13 of 43 > General Chemistry 4th Edition McQuarrie Rock Gallogly University Science Books presented by Macmillan Learning How many milliliters of 11.5 M HCI(aq) are needed to prepare 255.0 mL of 1.00 M HCl(aq)? V = mL > TOOLS x10 Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemsitry Publisher: University Science Books A étv Aa MacBook Air 80

The following volumes of 0.000300 M SCN- are diluted to 15.00 mL. Determine the concentration of SCN- in each sample after dilution. These values will be used during the experiment.  Sample 0.000300 M SCN- (mL) [SCN-] (M) 1  1.50   2 3.50   3 7.00   4 10.00