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...

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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
1
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…
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The following table shows data from the titration of four 10.0 mL samples of a solution containing hydrochloric acid, HCl(aq), using a 0.242 mol/L sodium hydroxide standard solution. Bromothymol blue is used as an indicator to detect when the endpoint is reached. Titration of 10.0 mL HCl(aq) with 0.242 mol/L NaOH(aq) Trial final burette reading (mL) initial burette reading (mL) volume of NaOH(aq) added (mL) colour at endpoint #1 #2 #3 #4 17.9 35.0 22.9 40.1 0.3 17.9 5.9 22.9 blue green green green a) Select the most consistent trials and calculate the average volume of titrant added. b) Calculate the concentration of the hydrochloric acid solution. Hint: Write a balanced chemical reaction first. You MUST show your work in the space provided. Then, record your final answers with the correct number of significant digits and the proper units.
Make sure has a correct significant dig
Determine the concentrations of all major species in a solution of 1.14 M chromic acid, H2CrO4(aq). For this acid, Ka1 = 0.18 and Ką2 = 3.2 x 10-7. [H2CrO4(aq)] = i M [HCRO4 (aq)] = i M [CrO,2(aq)] = i M [H3O*(aq)] = i M pH = i
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…
4. How does the pH of each of the following solutions change when 5.0 mL of 1.0 M NaOH (a strong base) is added? Fill in the table. Give your answers with 2 decimals. Initial pH Final pH after adding NaOH Solution (a) 100.0 ml water (b) (c) 100.0 mL 0.150 M HNO2 (a weak acid) (Given: Ka = 4.5 × 10-4) 100.0 mL solution of 0.150 M HNO2 and 0.100 M NaNO₂

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