Use the exact values you enter to make later calculations.Experiment 4: Titration of AcidsHCl(aq) + NaOH(aq) →>>NaCl(aq) + H2O(1)Complete the following tables. (Enter all measured volumes to the nearest 0.1 mL. Enter concentrations in M to 3 significant figures. If you did not do a third trial,enter "0" for each of the Trial 3 column responses. Do not include units in your answers. Enter computed values to the correct number of significant figures.)Analyte & Titrant Known ValuesVolume of HCI10.00 ± 0.02 mLConcentration of NaOH 4.0 0.1027MTitration of Hydrochloric acid (HCI) with Sodium Hydroxide (NaOH)Trial 1Trial 2initial buret reading (mL)4.004.004.00final buret reading (mL)4.010.14.04.09.49.5volume of NaOH added (mL)4.04.04.09.99.39.4moles of NaOH (mol)4.01.0274.04.0molarity of HCI (M)average molarity of HCI (M)4.04.04.04.0Trial 3

Step 1: GivenVolume of HCl, VHCl = 10.00 mLMolarity of NaOH, MNaOH = 0.1027 M HCl (aq) + NaOH (aq) →…

Answered: Use the exact values you enter to make…

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...

See similar textbooks

Similar questions

Hi I am having trouble finishing and finding the rest of the data for my Titration lab. I've already imputed the given data and just need to find the rest of the excel boxes using those data, thank you.
Please help me how to calculate this. All about titration. even the trial 1 will do I can do trial 2 and 3. I just need to learn how to do it. thanks
Please answer all parts.
Consider a titration experiment of a NaOH solution from a burette is being added to an Erlenmeyer flask containing HCl solution. All your final answers should be reported to 4 significant figures. Calculate the concentration of 25.0 mL HCl that required 24.6 mL of 0.142 M NaOH titrant to reach the indicator endpoint. Calculate the concentration of 40.0 mL HCl that required 38.6 mL of 0.205 M NaOH titrant to reach the indicator endpoint.
The following tabulated data is provided to answer this question and the remaining questions in the quiz. The post lab data will appear each page so that you can refer back to this data, as needed. Review the data, then answer the first question below. The equation is H2SO4 + NaOH → Na2SO4 + H20 (note, this equation is unbalanced) The last two rows are left blank because they will be filled in by your calculations. Titration Lab Trial 1 Trial 2 Trial 3 Volume of Acid Used 20.0 mL 20.2 mL 20.8 mL Molarity of Acid Used 0.05 M 0.05 M 0.05 M Initial Buret Reading 0.00 mL 0.00 mL 0.00 mL Final Buret Reading 20.7 mL 21.0 mL 21.5 mL Volume of NaOH Used Molarity of NaOH Solution What is the correct balanced equation for the neutralization reaction? Select one: O a. H2SO4 + NaOH → Na2SO4 + H2O O b. H2SO4 + 3 NaOH → Na2SO4 + 3 H2O c. H2SO4 + NaOH → Na2SO4 + 2 H20 O d. H2SO4 + 2 N2OH → N22SO4 + 2 H2O
Complete the chart using the information provided in the second image. Show setup for the calculation of the molarity of the HCI for Trial 1 and also show the setup for the Calculation of the percent HCI in the solution.
Chem. 1A: Acid-Base titration : to determine molar mass of a diprotic ACID : H2A Put a weighing paper on the pan of balance and tare it. Then add 0.1482 g of an unknown diprotic acid. Transfer the acid to a Erlenmeyer flask add 35.0 mL. water and 4 drops phenophethaleine. The color of solution is colorless. Set up a 50.00 mL. buret: wash the buret with tap water twice, with deionized water twice and and the 0.1029 M NAOH(aq). Fill the buret with 0.1029 M NaOH(aq), remove the air bubble and adjust the initial buret reading to 0.00 mL. Put the Erlenmeyer flask containing the acid and the phenolphethaleine below the buret with 0.1029 M NAOH(aq). Add NaOH(aq) from buret to the Erlenmeyer flask containing the diprotic acid and phenolphethaleine , until the color of the solution turn to pink by adding one or two drops of NaOH(aq). Then stop adding NaOH(aq) from buret and read the final volume of NaOH(aq). Acid-base titration: buret base of known concentration + stopcock acid of unknown…
Make sure has a correct significant dig
Please don't provide handwritten solution ....
Consider the titration of 100.0 mL of 0.100 M NaOH with 1.00 M HBr. Find the pH at the following volumes of acid added. See the picture below. Kindly answer all the questions, thanks!
What is the pH at the equivalence point in the titration of 60.00 mL of 0.200 M HA (a generic acid with K, = (2.26x10^-5)) with 0.400 M NaOH? Enter your answer in scientific notation with 3 sig figs. Do not include any units in your answer. Do not round any intermediate calculations. Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: x10 Answer
Vinegar? required to neutralize the acetic acid in each sample of vinegar, 16. Complete the calculations to find the molarity and percentage of acetic acid in vinegar. Convert the average volume of NaOH required to reach endpoint from mL to L Average volume of NaOH required to reach endpoint in mL 15. Subtract the initial volume from the final volume to calculate the volume of NaOH I DATA 269 12.55 TITRATION DATA (REPORT YOUR VOLUMES TO 1/100TH MI TRIAL 1 TRIAL 2 Initial base buret reading Final base buret reading Volume of sodium hydroxide (NaOH) required to reach endpoint in mL Volume of vinegar used O15 12.55 TRIAL 3 12:55 24.11 EXTRA TRIAL 24.11 35.39 11.78 12.05 11.56 15.00 mL 15.00 mL 15.00 mL 15.00 mL (Show calculations here.) 12.05711-56+1178 -27.54 27.54ML (Show calculations here.) a7.54ML X IL 0-02754L :0.02754L nd bon 1600 Molarity of NAOH (recorded from the standard solution bottle) 0.1 I CALCULATIONS FOR MOLARITY OF ACETIC ACID IN VINEGAR 1. Using the known molarity of…

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry

ISBN:

9781305957404

Author:

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

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

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

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Organic Chemistry

Chemistry

ISBN:

9780078021558

Author:

Janice Gorzynski Smith Dr.

Publisher:

McGraw-Hill Education

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Elementary Principles of Chemical Processes, Bind…

Chemistry

ISBN:

9781118431221

Author:

Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard

Publisher:

WILEY

SEE MORE TEXTBOOKS