2. Measurement of the pK, of Acetic Acid by the Half-Neutralization Method 1,00 Concentration of standardized NAOH titrant mole/L Trial 1 Trial 2 Trial 3 Mass of acetic acid solution 20.0 20.0 Volume of NaOH added to half-neutralize the acetic acid 0.40 mL 0.40 mL ml Measured pH of half-neutralized solution 4.68 4.66 28-7 Average pH value. pk, K,- Calculate the [H,0*] and the concentrations of A and HA, in the half-neutralized solution (Note: In this solution, (H,O] (A ].)

2. Measurement of the pK, of Acetic Acid by the Half-Neutralization Method 1,00 Concentration of standardized NAOH titrant mole/L Trial 1 Trial 2 Trial 3 Mass of acetic acid solution 20.0 20.0 Volume of NaOH added to half-neutralize the acetic acid 0.40 mL 0.40 mL ml Measured pH of half-neutralized solution 4.68 4.66 28-7 Average pH value. pk, K,- Calculate the [H,0*] and the concentrations of A and HA, in the half-neutralized solution (Note: In this solution, (H,O] (A ].)

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

K2HPO4-KH2PO4 buffer solution with water, vinegar, 0.85 M Na2CO3 sodium carbonate K2HPO4-K3PO4 buffer solution with water, vinegar, 0.85 M Na2CO3 sodium carbonate For each buffered solution from above: A.) Describe how the pH changed for added vinegar relative to cabbage indicator. B.) Describe how the pH changed for added sodium carbonate relative to cabbage indicator. C.) Describe the pH of the three solutions (using numbers from tabs and color chart). D.) Calculate the pKa of each buffered solution. E.) Compare the pKa calculated to the pH found using the tabs (close, very different?) I am having trouble understanding this problem if someone can help me walk it through. thank you very much
3. Use a titration between an acid and a base to answer the following: a. Mole to mole ratio of acid and base at the equivalence point: b. Describe how to find the equivalence point from a titration graph: and /150ml C. The equivalence point of a titration with 23 mL of 0.15M NaOH is used with 25mL of unknown HCI. What is the concentration of HCI? Jent ebxoibyvd muiboe to noits uov to aeogaib uDy bluone nonk
Which of these apply to the Image (attached)? There should be 4 total answers: A. High End pH B. High Initial pH C. Vertical Line with Equivalence Point Tall D. Equivalence Point Not at pH 7 E. Equivalence point at pH 7 F. low end pH G. low initial pH H. Vertical Line with Equivalence Point Short Using the info identified above, what type of analyte and tirant combo are in the image. Options for Analyte and Titrant: - Weak base - Strong Acid - Strong Base - Weak Acid
The pH of the buffer solution is 4.0 while the pKa of the weak acid is 3.0. Compute for the molar part of the acid component 1 part 10 parts 0.1 part 0.01 part
Endpoints in titrimetric procedures employing neutralization reactions are determined by:I. PotentiometerII. Visual Inspection III. Indicators III only II & III I & II I, II & III I & III
To prepare 1 liter of 0.10 M acetate buffer at PH 5.20.I need to mix _____g of CH3COONa molecular weight 82.03 g/mol with ______ml of 6.0 moler HCL and dilute the solution to the volume of 1 liter .pKa of acetic acid is 4.76..fill in the above blanks.??.
Titration Curve for Unknoówn A 12 11.49 10.04 10 2.85 10 15 20 25 30 35 ml levels pH levels
Select Weak Acid as the analyte in the titration interactive. Analyte, 25.0 ml. Weak Acid, 1.0.. Determine the pK, of this weak acid. colortess Indicator No Indicator 14 13.83 pK, = Incorrect pH=2.50 25 50 Titrant Added (mL) Titration Curve Concentration Chart Titrant: Strong Base, 1.0 M MOH 50 0.0 ml + Hd
need both 2 parts soon in detail don't copy I. will downvote
BURETTE READING SAMPLE Pp Mo A 12.4 25.0 6.2 6.2 9.2 16.8 D. 0.0 5.3 Use the table below to identify the basic compound C: *Note that double indicator titration for each compound was done using a standard acid solution with 0.0 mL as initial reading. O NaHCO3 O NaOHANazCO3 O NaOHANaHCO3 O Nazco3
I. Preparation of acetate buffer solutions with different pH values 1. Calculate the salt and acid volumes required to prepare 10 ml of the acetate buffer with the following ratio of sodium acetate and acetic acid: Test tube #1: Ratio - 1:9 Salt volume Acid volume ml ml
he X - OWLV2 | Assigr x : OWLV2 | Online X y! google - Yahoc X e Registration - L X O selfserve.una.e X Irn/takeAssignment/takeCovalentActivity.do?locator=assignment-take [Review Topics] [References) Use the References to access important values if needed for this question. A buffer solution is 0.478 M in H2SO3 and 0.380 M in KHSO3. If K for H2SO3 is 1.7 x 10-2, what is the pH of this buffer solution? pH = Submit Answer Retry Entire Group 9 more group attempts remaining 5:05 P 11/2/20 Cop fi2 ort sc delete home ho backspace num Iock