ver 80 % industry area has reported acid rain due to harmful gases emissions. Josephine collected a rainwater sample from industry site and analysed it using pH meter. It was found that the sample recorded an average pH of 4.35. Calculate the amount of H* in rainwater sample. Suggest an alternative method to determine H* in unknown liquid samples

ver 80 % industry area has reported acid rain due to harmful gases emissions. Josephine collected a rainwater sample from industry site and analysed it using pH meter. It was found that the sample recorded an average pH of 4.35. Calculate the amount of H* in rainwater sample. Suggest an alternative method to determine H* in unknown liquid samples

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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esc A 0.2000M solution of hydroflouric acid is only partially ionized. Using measurements of the pH of the solution, [H+] was determined to be 3.184 x 10-2 M. Calculate the acid dissociation constant of hydroflouric acid. / 54°F Mostly clear 7.023 x 10-3 6.669 x 10-3 @ "// A 6.029 x 10-3 5.534 x 10-3 2 113 C W # 3 E 14101 $ O Search 4 % 5 R S DEL F 1 z 1 x || c || V || B T 161 G 6 Y 7 N 8 9 K M O P ? 1 prt sc 9:30 PM 4/23/2023 backspace C pause delete
Determine an unknown concentration or volume using an acid-base titration. Calculate the volume of 0.114 M calcium hydroxide required to neutralize 19.4 mL of a 0.240 M nitric acid solution. mL Alpha-numeric input field Check & Submit Answer Show Approach It is often important to have an accurate concentration of an acid or base solution. With standardization, another type of acid-bas titration, the concentration of an acid or base is determined accurately by the use of either a primary standard or another solution w concentration has already been determined. A primary standard is an acid or base that can be obtained in a very pure form, such a potassium hydrogen phthalate, KHC;H4O4 (often abbreviated KHP), or sodium carbonate, Na2 CO3. The steps involved in standardization calculations are very similar to other acid-base titration calculations, as shown in the following example. tv A hulu W 四)
Write the Henderson-Hasselbalch equation for a propanoic acid solution (CH₂CH₂CO₂H, pKa [HA] pH = = 4.352 || pH = 4.874 Answer Bank [A] + log Using the equation to calculate the quotient [A¯]/[HA] at three different pH values. [A-] [HA] [A-] [HA] - o = pka pH = 4.874).
BUFFER CAPACITY EXPERIMENT Part 1: Preparation and pH Meter Calibration Prepare 50 mL of 0.5 M acetic acid from a concentrated stock. Prepare 50 mL of 0.5 M sodium hydroxide from a solid. Part 2: Buffer Capacity Transfer 20 mL of 0.5 M acetic acid (Ka is 1.75*10-5), stir at a slow setting and measure the pH reading is stabilized. Add 1.0 mL of 0.5 M NaOH and measure the pH. Continue adding 0.5 M NaOH in 0.5 - 1.0 mL increments until a major spike in pH occurs. After the spike, add another two 0.5 – 1.0 mL increments of 0.5 M NaOH. Create a pH vs. Volume graph to determine the range of the buffer’s capacity. Compare the actual data (nonstandard conditions) with the theoretical data under standard conditions. I NEED HELP WITH CALCULATIONS AN SMALL RESULT INTERPRETATION DESCRIPTION PLEASE TO UNDERSTAND WHAT I DID AND WHY THANKS
A.) In the laboratory, a general chemistry student measured the pH of a 0.589 M aqueous solution of diethylamine, (C2H5)2NH to be 12.321.Use the information she obtained to determine the Kb for this base.Kb(experiment) =
4. Diprotic acid system. a. Plot the ionization fractions (do, ɑi, a2) as a function of pH (0-14) for the diprotic system malic acid (C4H6O5), which is found in fruits such as apples. pKa1 = 3.40, pKa2 = 5.20 b. At a typical pH for natural waters, which species in the malic acid system dominates?
A) Please fill in the first blank with the word "acidic", "basic" or "nearly neutral". B) SHOW ALL WORK FOR THE pH QUESTION. WRITE YOUR FINAL NUMERICAL RESPONSE IN THE SPACE PROVIDED BELOW. Hint: IF you need Kb to solve this problem, you must calculate it from the information provided below. When 0.65 M potassium acetate salt hydrolyzes in water, the solution will be with a pH = Ka (CH3COOH) = 1.8 x 10 5 %3D
Ranking lonic Solutions: modified MC ChemlB Spr21 Page | 5 DI Predict the ranking of the pH for the solutions. 8) Fill in Table ID. Do this before performing the experiment with Beyond Labz Middle column: Identify cach solution as one of the following: Strong acid Weak acid Strong base Weak base Acidic salt Neutral salt Basic salt Last column: predict the pH ranking for the following 0.1 M solutions in order of expected increasing pH: rank of 1 will be for the strongest acid and the rank of 14 will be for the strongest base. Table 1D: Predicted Rank (1 most acidic and 14 most basic) Solutions (0.1IM) Identification NH,CI NaHCO3 KNO, NH3 H2SO4 NaC,H3O2 (NaAc) HCI H2SO3 HC2H3O2 (HAc) HCN NaOH NaCN H3PO4 Na PO4
(1) YouTube ns m/StudentFunctions/Interface/acellus_engine.html?Classi9=1129437624 Friday Night Funkin.... Mbku Friday Night Funkin... uru 4) U Find College Schola... N 3 E D A ght 2003-2022 International Academy of Science. All Rights Reserved. $ 1410 A buffer solution is prepared by adding NH4Cl to a solution of NH3 (ammonia). NH3(aq) + H₂O(1) ⇒ NH4+ (aq) + OH-(aq) What happens if HCI is added? 4 + shifts to reactants R F % 5 O Search T 6 B G shifts to products B Y 4 & hp 7 H fo * U N 8 remains the same ( - 9 ☆ ESA Amazon.com Shop... (Cloud Silver Shark F.... M fe93157t7ut7uttButt... M fo K 11 O O P + { = [ 1 D insert ? $ O 10:48 AM 12/24/2022 prt sc 1 4 X >> Help Resources Skip pause backspace delete he
3 Part A When 200. mL of 1.50 x 10-4 mol L-1 hydrochloric acid is added to 135 mL of 1.75 x 10-4 mol L-1 Mg(OH)2, the resulting solution will be O basic. O neutral. acidic. It is impossible to tell from the information given. Submit Request Answer Provide Feedback % 5 Search or type URL 6 & 7 * 8 1
The following results were obtained in the titration of an unknown monoprotic acid (Use data from table). Students identified the acid as benzoic. Copy VNaOH (no first raw), then pH(all values) into your Lab Report template. Use the data you obtained to fill in the table below. Concentration of NaOH used, M 1.164 x 10-1 Mass of unknown aid used, g 0.3840 1) Find: a) Equivalence point, mL. b) Half equivalence point, mL. c) pKa d) Ka e) pKa from literature f) Percent Error g) Number of moles of NaOH, mol. h) Number of moles of acid titrated, mol. i) Molar mass of acid g/mol. j) Molar mass of acid, g/mol from the literature k) Percent error
Time (sec.) pH of distilled water pH of buffered solution 20 7.99 8.61 40 7.46 8.43 60 7.15 8.31 80 6.75 8.22 100 6.54 8.16 120 6.39 8.10 140 6.22 8.05 160 6.11 8.01 180 6.03 7.97 Conclusion Explain your observations from the data table. Which resists a change in pH the most, water or the buffered solution? Give reasons. When you blow into the water, the pH goes up. Is the solution becoming more basic or acidic? A buffer is usually made of a weak acid and a weak base. When you blow into a buffer the pH doesn’t change. What do you think is happening?