Lab 14 Handin done

light data and DID NOT round any intermediate calculations. In a 3.8M aqueous solution of benzoic acid (C6H, CO₂H), what is the percentage of benzoic acid that is dissociated? You can find some data that is useful for solving this problem in the ALEKS Data resource. Round your answer to 2 significant digits. 7.0 % GEE ola

1. Calculate the theoretical molarity of the NaOH solution you prepared. 2. Calculate the actual molarity of your .10 M NaOH solution. 3. Calculate the percent error between the two NaOH values you have.

How many milliliters of water have to be added to 122.5 mL of 0.50 M HCl to reduce the concentration to 0.10 M HCI? Vwater mL %3D eTextbook and Media Hint Save for Later Attempts: 3 of 15 used Submit Ans ост 14 tv MacBook Air 80 888 DD F1 F2 F3 F4 F5 F6 F7 F8 F9 F10 @ 23 2$ 4 7 OC

The buret reading is the amoung of NaOH i added 1. calculate the moles of NaOH required to neutralize the aspirin in each trial. 2. calculate the molarity of NaOH in each trial.

Calculate the moles of H+ delivered to eachsample based on your experimental dataand record these values in Data Table 1. 0.1M HCl = 0.1 moles HCl / 1 Liter solution Calculate the moles of OH- in each sampleand record these values in Data Table 1. H+ + OH- H2O Calculate the moles of Ca2+ in each sampleand record these values in Data Table 1.  Ca(OH)2 Ca2+ + 2OH . Calculate the molar solubility of Ca(OH)2for each sample and record these values inData Table 1. Molar solubility = moles / Liter . Calculate the Ksp for each trial and theaverage Ksp and record these values inData Table 1. Ksp = [Ca2+][OH-]2       Sample 1 Sample 2 Sample 3 Mass of Erlenmeyer Flask 25.47 25.47 25.47 Mass of Erlenmeyer Flask + Calcium Hydroxide Solution (lime water) 28.32 28.30 28.43 Mass of Calcium Hydroxide Solution 2.85 2.83 2.96 Volume of Ca(OH)2 Density = 1.000 g/mL       Concentration of HCl (M)       Initial HCl Volume in Syringe 1.0ml…

CHEMISTRY 1110L LAB REPORT: PROPERTIES OF SOLUTIONS Part One (Do calculations on the back of this sheet, prior to lab!) 1. In order to prepare 50.0 mL of 0.100 M NaOH you will add 2. In order to prepare 50.0 mL of 0.200 M 3. In order to prepare 50.0 mL of 0.150 M 4. In order to prepare 50.0 mL of 0.100 M HC₂H3O2 you will add mL of 1.00 M HC₂H₂O₂ to HCl you will add H₂SO4 you will add 5. In order to prepare 40.0 mL of 0.100 M NH3 you will add 6. In order to prepare 50.0 mL of 0.100 M NaCl you will add___ grams of NaCl to mL of water. 7. In order to prepare 50.0 mL of 0.100 M C12H22O11 (sucrose) you will add grams of C12H22O11 to mL of water. NOTE: The final volume is the sum of the concentrated solution plus the volume of added water. When making solutions from solids, since the solid dissolves in the water with minimal volume change, the volume of the final solution is the amount of water you need to use. Part Two 8. Measurement of Acidity a. 0.100 M NaOH b. 0.200 M HCI c. 0.150 M…

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1. The [H30"], in M, of 10.00 mL of 0.100 M NAOH after adding 10.00 mL of indicator solution. To enter exponential values, use the format 1.0e-5. Answer: 2. The [H30"], in M, of 10.00 mL of 0.100 M HCl after adding 10.00 mL of the indicator solution. To enter exponential values, use the format 1.0e-5. Answer:

I need help calculating the initial concentrations please.

Please help with explanation. (Gpt/Ai wrong answer not allowed)

L Moving to another question will save this response. Question 1 B A C D i litr OH L A Moving to another question will save this response. > НО. > Question 1 of 4 5 points E O Arrange the following compound based on decreasing water solubility. Use the letters assigned to each compound and place your answers to the space provided. Increasing acidity is >>> Save Answer Question 1 of 4 > >>

Each row of the table below describes an aqueous solution at 25 °C. The second column of the table shows the initial components of the solution. Use the checkboxes in the third column to explain the type of the initial solution. The fourth column describes a change in the solution. • Use the fifth column to predict how the change in the solution will change its pH. solution initial components initial type (check all that apply) change effect of change on pH (check one) acidic A H₂O basic add NaNO3 neutral acidic O pH higher pH lower pH the same O pH higher B H₂O, HCI basic add K Cl O pH lower neutral acidic C H₂O, HCI basic add KOH neutral acidic D H₂O basic add HNO3 Oneutral O pH the same O pH higher O pH lower O pH the same O pH higher O pH lower O pH the same 5

Find molarity of X and HX in beaker 1  X= 0.100M HX=0.100M

How many grams of hy

For propanoic acid (HC3H502, Ka = 1.3 x 10-5) Determine the percent dissociation of a 3.42 M solution. % Question Help: Message instructor Submit Question AUG 19 80 F3 000 000 F4 % 95 54 #3 ķ 649 119 F5 F6 F7 6 27 & 8

Calculate the number of moles of acetic acid in 100mL of both samples of vinegar accurately titrated. given: NaOH vs CH3COOH Burette solution is NaOH and the pipette solution is 5.0 mL of Vinegar Titration Initial burette reading Final burette reading Volume of NaOH consumed Average volume of NaOH Approximate  0.0 mL 20.1 mL 20.1 mL 20.3 mL Titration 1 0.0 mL 20.9 mL 20.9 mL Titration 2 0.0 mL 20.0 mL 20.0 mL To find the average volume  Average volume = 20.1 mL + 20.9 mL + 20.0 mL320.1 mL + 20.9 mL + 20.0 mL3                            = 20.3 mL Concentration of Vinegar = Volume of NaOH * Concentration of NaOHVolume of vinegarVolume of NaOH * Concentration of NaOHVolume of vinegar                                           = 20.3 mL * 0.0647 M5.0 mL20.3 mL * 0.0647 M5.0 mL                                           = 0.2627 M Concentration of NaOH = Volume of H2SO4 * Concentration of H2SO4Volume of NaOHVolume of H2SO4 * Concentration of H2SO4Volume of NaOH…

Suppose a student performed a similar standardization titration experiment. Below is the calculated concentration of NaOH from each of their titrations.   Titration #1 Titration #2 Titration #3 Concentration of NaOH (M) 0.9554 0.9540 0.9551 Using the 3 concentrations, calculate the average concentration of the student's NaOH solution and calculate the ± error in parts per thousand (ppt). Show the complete calculation. Express your final answer in the form of average (with units) ± error in ppt. use the right significant figures

How to solve for grams of KHP and the percent of KHP?

Find the [H2L*] concentration in a 0.005 M leucine hydrochloride aqueous solution (H2L* ), H2L*, Kaj = 4.70 x 10-3, Kaz = 1.80 x 10-10 %3D O a. 0.004M O b. 4.8x10-3M O c. 22.2x10- O d. 1.5x10-4 M

Data of HCl Trial 1: volume of HCl =0.82l Volume of NaOH =22.1ml Trial 2: volume of HCl=0.821ml Volume of NaOH = 22.2ml Trial 3: volume of HCl= 0.821ml Volume NaOH = 22.7ml 1) calculate the molarity of HCl for each trial and find the average molarity.

This is about determinition of acid content in vinegar through titration, please answer the questions. Please answer only the items nummber 4-5. i only put other questions for guide. 1. What is the purpose of standardization? 2. What is the primary standard used (name and formula)? ANS: KHP 3. Suppose that the KHP is not completely dry. Will the reported molar concentration of the sodium hydroxide solution be higher, lower, or unaffected? Explain. 4. In preparing the buret for titration the final rinse is with the NaOH titrant rather than with distilled water. Explain. 5. The procedure suggests the addition of only 2 drops of phenolphthalein. What will be the effect to the analysis if larger amount of phenolphthalein is added?

Question 16 I want a detailed explanation thanks

Solve question 12

Questions 11-14 refer to the same strong base/strong acid (SB/SA) titration. A 15.00 mL solution of 0.100 M sodium hydroxide (NaOH) is being titrated with 0.250 M hydrobromic acid (HBr). What is the solution pH before the titration begins? (Two decimal places) Type your answer...

10.0 mL 0.5 M HCl neutralizes ________ mL 0.1 M NaOH.

Calculate the accurate molarity of the sodium hydroxide solution using date from each titration to determine two values for the molarity. Calculate the average molarity of the sodium hydroxide solution from the individual values, and use the average in subsequent calculations. Given: Molarity of sulfuric acid:0.205 M (Sodium hydroxide with sulfuric acid)Approx Titration- initial buret reading : 0mL final buret reading : 31.8mL titration 1- initial buret reading : 0mL final buret reading : 31.5 mL titration 2- initial buret reading: 0mL final buret reading : 31.7mL Analysis of vinegar Approx titration - initial buret reading : 0mL final buret reading : 20.1 mL titration 1-  volume of vinegar solution:5mL initial buret reading : 0mL final buret reading : 20.9mL titration 2- Volume of vinegar solution :5mLinitial buret reading : 0mL final buret reading : 20.0mL

help please answer in text form with proper working and explanation for each and every part and steps with concept and introduction no ai no copy paste remember answer must be in proper format with all working

Each row of the table below describes an aqueous solution at 25 °C. The second column of the table shows the initial components of the solution. • Use the checkboxes in the third column to explain the type of the initial solution. The fourth column describes a change in the solution. • Use the fifth column to predict how the change in the solution will change its pH. solution initial components initial type (check all that apply) change effect of change on pH (check one) O acidic A H₂O, KOH basic ○ pH higher add KI O pH lower neutral acidic B H₂O basic add H CIO4 O neutral ☐ acidic C H₂O ☐ basic add Na CIO O neutral acidic O pH the same O pH higher O pH lower O pH the same O pH higher O pH lower O pH the same O pH higher D H₂O, KOH basic add HI O pH lower Oneutral O pH the same