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 + H2O (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: a. H2SO4 + NaOH → Na2SO4 + H2O b. H2SO4 + 3 NaOH → Na2SO4 + 3 H2O c. H2SO4 + NaOH → Na2SO4 + 2 H20 d. H2SO4 + 2 NaOH → Na2SO4 + 2 H20

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 + H2O (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: a. H2SO4 + NaOH → Na2SO4 + H2O b. H2SO4 + 3 NaOH → Na2SO4 + 3 H2O c. H2SO4 + NaOH → Na2SO4 + 2 H20 d. H2SO4 + 2 NaOH → Na2SO4 + 2 H20

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

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 120CP: Another way to treat data from a pH titration is to graph the absolute value of the change in pH per...

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Similar questions

When might a pH meter be better than an indicator to determine the end point of an acid-base titration?
Another way to treat data from a pH titration is to graph the absolute value of the change in pH per change in milliliters added versus milliliters added (pH/mL versus mL added). Make this graph using your results from Exercise 61. What advantage might this method have over the traditional method for treating titration data?
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.
Students Mola and Rity were tasked to analyze the acidity of a 10.0-mL fermented milk sample diluted with water in a 250-mL volumetric flask. Mola obtained a 15.0-mL aliquot of this solution, diluted it to 50.0 mL, and then titrated this diluted sample. Titration data were given to Rity and she found out that the 50.0-mL diluted sample contains 0.21 mmol of lactic acid. MW: Lactic Acid (90.08) a. What is the lactic acid concentration (in M) of the titrated sample? b. Determine the lactic acid content (in M) of the 10.0-mL fermented milk sample. c. What is the lactic acid concentration (in %w/v) of the 10.0-mL fermented milk sample?
Why you should not start a titration with zero mL as an initial volume?
The table has data from the titration of four 10.0 mL samples of a solution containing hydrochloric acid, HCl(aq), using a 0.299 mol/L sodium hydroxide standard solution. Titration of 10.0 mL HCl(aq) with 0.299 mol/L NaOH(aq) Trial #1 #2 #3 #4 final burette reading (mL) 17.9 35.0 22.9 40.1 initial burette reading (mL) 0.3 17.9 5.9 22.9 volume of NaOH(aq) added (mL) colour at endpoint blue green green green a) Select the most consistent trials and calculate the average volume of titrantadded.b) Calculate the concentration of the hydrochloric acid solution.
A student titrates samples of a base with a standardised acid. The titration values obtained for each sample is given in Figure 5. What is the average titration value in cm³ that the student should use in further calculations? * Your answer
Volume of water sample used: 103 mL Initial buret volume: 0.45 mL Final buret volume: 16.92 mL HCl molarity: 0.020 M How many moles of HCl were used in this titration?
what glassware should be used to add the sodium hydroxide into the hydrochloric acid solution? A. Volumetric pipette b. Graduated cylinder c. Volumetric flash d. Erlyn mayer flash
Find the number of moles of HCl added. Concentration of HCl solution, M: 0.60 Initial buret reading: 0.35 ml Final buret reading: 5.65 ml Volume of titrant: 5.35 ml
Give typed solution A student analyzed a CaCO3 antacid tablet by neutralizing the base with an excess of .60 M HCL and back-titrating the excess with .50M NaOH. He recorded the following data: mass of tablet = 1.3g amount of active ingredient CaCO3 per label = 500 mg volume of HCl added: 25 mL initial buret reading : 34 mL final buret reading : 47.4 mL If the concentration of the provided HCl is actually higher than .60M, would the determined mass of CaCO3 in the antacid tablet be too high or too low?
This question is concerned with acid/base. The ionic product of water may be taken as 10-14 mol2dm-6. Aqueous solutions of a particular monobasic acid HX have the following pH values (see figure below). Concentration in moldm-3 PH Hydrogen ion concentration in moldm-3 Solution A 0.1 2.80 1.585 x 10-3 Solution B 0.001 3.85 Complete the table by calculating the hydrogen ion concentration of solution B. Write down the equation describing the dissociation of the acid HX in an aqueous solution.