Experiment 1: Preparation and pH of Buffer Solutions Test Data: Mass of Sodium Acetate :4.0 g Volume of Sodium Acetate Solution: 100.00mL Acetic Acid Concentration (mass percent from label) :4.5% pH of Prepared Buffer Solutions Buffer Solution Acetic Acid; 4.5% Sodium Acetate Solution Recorded pH A 5.0 mL 5.0 mL 4.3 B 5.0 mL 1.0 mL 4.2 C 10.0 mL 1.0 mL 3.4 D 1.0 mL 10.0 mL 5.0 E 1.0 mL 5.0 mL 4.5 questions 1. Compare the calculated pH of buffers A, B, C, D, and E to the measured pH of each of these buffers in Experiment What did you notice? Describe what may have accounted for any variations in pH if you saw any variations.

Experiment 1: Preparation and pH of Buffer Solutions Test Data: Mass of Sodium Acetate :4.0 g Volume of Sodium Acetate Solution: 100.00mL Acetic Acid Concentration (mass percent from label) :4.5% pH of Prepared Buffer Solutions Buffer Solution Acetic Acid; 4.5% Sodium Acetate Solution Recorded pH A 5.0 mL 5.0 mL 4.3 B 5.0 mL 1.0 mL 4.2 C 10.0 mL 1.0 mL 3.4 D 1.0 mL 10.0 mL 5.0 E 1.0 mL 5.0 mL 4.5 questions 1. Compare the calculated pH of buffers A, B, C, D, and E to the measured pH of each of these buffers in Experiment What did you notice? Describe what may have accounted for any variations in pH if you saw any variations.

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.58QE

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Let's determine the concentration and the pH of a H2CO3 solution that was prepared by using standard NaOH solution with a concentration of 0.125 M using the following data. Trial 1 Trial 2 Trial 3 Volume of H2CO3 19.80 mL 20.05 mL 19.95 mL Initial volume of NaOH (mL) 1.90 16.88 31.98 Final volume of NaOH (mL) 16.88 31.98 47.00 What is the Molarity and the pH of the H2CO3 ?
Please help me fill out this table! Answering just one of the columns is good enough, thank you! Concentration of Standardized NaOH - 1.00 mol/L Mass concentration of acetic acid - 2.40 g/L Trial 1 Trial 2 Measured pH of the acetic acid solution 3.07 3.05 Mass of acetic acid solution taken for titration 20.0 g 20.0 g Initial buret reading of NaOH titrant 0.00 mL 0.00 mL Final buret reading of NaOH titrant 0.82 mL 0.79 mL Net volume of NaOH 0.82 mL 0.79 mL Millimoles of NaOH to end point of titration _?_mmol _____mmol Millimoles of acetic acid in sample _?_mmol ______mmol Molar concentration of acetic acid solution _?_mol/L ______mol/L
The data from my observations is given below: Concentration of Standardized NaOH - 1.00 mol/L Mass concentration of acetic acid - 2.40 g/L Trial 1 Trial 2 Measured pH of the acetic acid solution 3.07 3.05 Mass of acetic acid solution taken for titration 20.0 g 20.0 g Initial buret reading of NaOH titrant 0.00 mL 0.00 mL Final buret reading of NaOH titrant 0.82 mL 0.79 mL Net volume of NaOH 0.82 mL 0.79 mL Millimoles of NaOH to end point of titration 0.82 mmol 0.79 mmol Millimoles of acetic acid in sample 0.82 mmol 0.79 mmol Molar concentration of acetic acid solution 0.043 mol/L 0.041 mol/L Calculated molar mass of acetic acid g/mol g/mol Average molar concentration of acetic acid for the samples titrated: 0.042 mol/L Average pH: 3.06 Question: Calculate the corresponding [H3O+], compute the corresponding concentration of A- and HA, and calculate the dissociation constant Ka Thank you!
II. Titrating HCI Solution with NaOH Solution 1. Prepare a titration curve. Plot pH (on the y-axis) versus volume of NaOH solution added (on the x-axis). If your initial buret reading was not 0.00 mL, remember to subtract your actual initial reading from each of your subsequent buret readings before plotting the titration data.
File Edit View Insert Format Tools Add-ons He Introduction Procedure Observation Observations: 100% 1 2 I 3 I 4 Initial solution temperature (°C): 20.8°C Maximum solution temperature (°C):27°C Recall that the steepest point on the pH curve occurs at the equivalence point, that is, when the acid is exactly neutralized. Total volume of NaOH titrated to reach end-point or neutralization (steepest point on the pH curve):25ml 14 13 Mass of solution (g) = (Volume of NaOH titrated (ml) + Volume of HCl (ml)) x density Mass of solution = 76 g 34 32 31 30 29 Note: Assume a density of 1.038 for both NaOH and HCI 11 10 pH Heat released by neutralization: 27 Q = mcAT Q = 1.9 x 10^3 J 25 where m is the mass solution in grams, c = specific heat capacity of our solution (=4.184 J/°C g) and AT=T, max 23 22 21 20 Tinitial- Heat of Neutralization = Q/moles of limiting reactant Q/moles of NaOH titrated at neutralization Q/(Molarity of NaOH x volume of NaOH (in litres)) 10 15 20 25 30 35 40 45 %3D Volume…
Volume NaOH (added). pH of analyte 0.00 mL _1.00 10.00 mL 1.23 20.00 mL _1.54 30.00 mL _2.20 _33.33__ mL (at equivalence point) _5.22 35.00 mL _11.46 40.00 mL _12.04_ 9. Sketch your pH curve below. Place the pH on the y-axis and volume of NaOH added on the x-axis.
Table 1 Titration Data. Trial #1 Trial #1 (continued) Trial #2 Trial #2 (continued) Volume of Volume of NAOH added (mL) Volume of Volume of NAOH added (mL) pH NAOH added pH pH NaOH added pH (mL) (mL) 4.30 Iml 4.51 4.44 4,95 4..30 4.52 4.98 4.95 S.15 5.30 0.00 0.00 2. 2. 3. 5.28 S.S2 $,505.50 5.90 S.80 S, 8 6.04 6.20 16.50 T.16 10.10 7.6 10.20 8.32 1U.308.78 0.40 9.28 10.509.57 A0.21 1.08 So64 S,g6 6.07 6.64 4.5 8.0 8.3 16 12 a.s 10 12 14 169 4.62
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?
i need the Ka of an unknown acid please Vol of Observation NaOH added ml Total Vol of pH NaOH, ml %23 3.29 1.0 1.0 4.23 4.57 4.80 4.99 1.0 2.0 4. 1.0 3.0 1.0 4.0 1.0 5.0 6.0 7.0 5.16 1.0 1.0 5.33 5.50 8. 8.0 5.71 5.98 6.50 6.73 7.22 1.0 10 1.0 9.0 11 1.0 10.0 10.02 10.04 12 0.2 13 0.2 14 0.2 10.06 10.43 15 0.2 10.08 10.91 11.13 11.28 11.38 16 0.2 10.10 10.12 0.2 0.2 17 18 10.14 19 0.2 10.16 11.47 2///5670
13) Bromthymol blue (BTB) is a chemical indicator that is blue all alone. When combined with a basic solution, it turns green as a solution becomes more acidic it turns yellow in an acidic solution. Fill in what color you think bromthymol blue would be in each of the situations in the chart. If solution color is given, simply provide a logical, possible pH value based on the outcomes. Fill in the missing ions as well! Situation pH BTB color Ion present Water directly out of tap 7.2 pH after exhaled air is blown through a straw into water for 5 5.1 H+ min. 14 pH after a snail has lived in water for three days Very Yellow pH with 2mL of bleach added to the water Very Blue 5.0 pH with instant coffee added to the water pH after an aquatic plant is grown in water for three days in bright sunlight Light Blue OH- 14)Is BTB a chemical indicator? 15) What then does it "indicate"? 16) Based on the data above, why does drinking coffee cause stomach pain for some indivudals? 17) What effect does…
Data Table: (include units!) Unknown Acid # Your NaOH concentration 0.10 Trial 1 Trial 2 Volume of Acid (in mL) 17ml 15ml Initial Buret reading for 15.00ml 0.00ml your NaOH Final Buret reading for 39.06ml 21.23ml your NaOH Total volume of NaOH 0.024L 0.021L used in titration
Find the pH during a titration of 1.00 mL of 0.600 M analyte when a) 0.00 mL, b) 10.00 mL, c) 30.00 mL, d) 60.00 mL, and e) 120.00 mL of 0.0100 M titrant has been added. Then f) sketch a titration curve. a) 0.00 mL titrant added ANAlyte: KN3 TitrANT: HI b) 10.00 mL titrant added

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Buffer Solution	Acetic Acid; 4.5%	Sodium Acetate Solution	Recorded pH
A	5.0 mL	5.0 mL	4.3
B	5.0 mL	1.0 mL	4.2
C	10.0 mL	1.0 mL	3.4
D	1.0 mL	10.0 mL	5.0
E	1.0 mL	5.0 mL	4.5