2)1.Februurg 2, 2022Lyonel TanisCHM-0ILSection: C16130)Name:Date:Report Sheet: Characterization of a Weak Acid.UNKNOWN NUMBERA. Standardization of NaOH SolutionTRIAL[HCI]VolumeMolesMolesVolume[NAOH]HCINaOHNaOH24.6525.750.100225.8925.73Average [NaOH].B. Identification of the Unknown Acid8.Determination of Molecular WeightTRIAL[NaOH]VolumeMolesMolesGramsMoleculaUnknownHOBNUnknownr Weight(g/mol)NaOH0.2947Lohe24.071.0.29432.3Average Molecular Weight(g/mol)

Answered: Image /qna-images/answer/9134e769-347d-4290-8ae3-7fa16d57cfef.jpg

A. Standardization of NaOH Solution TRIAL [HCI] Volume Moles Moles Volume [NAOH] HCI НОEN 25.75 IOH HOBN 0.1002 25.89 25.73 2. Average [NaOH]. B. Identification of the Unknown Acid Determination of Molecular Weight Volume Moles Moles Grams Unknown TRIAL [NAOH] Molecula HOBN Unknown r Weight (g/mol) HOBN 0.294 7 Lo'he 24.07 1. 0.2943 2. 3. Average Molecular Weight. (g/mol)

A. Standardization of NaOH Solution TRIAL [HCI] Volume Moles Moles Volume [NAOH] HCI НОEN 25.75 IOH HOBN 0.1002 25.89 25.73 2. Average [NaOH]. B. Identification of the Unknown Acid Determination of Molecular Weight Volume Moles Moles Grams Unknown TRIAL [NAOH] Molecula HOBN Unknown r Weight (g/mol) HOBN 0.294 7 Lo'he 24.07 1. 0.2943 2. 3. Average Molecular Weight. (g/mol)

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter16: Acids And Bases

Section: Chapter Questions

Problem 19QAP: . How is the strength of an acid related to the fact that a competition for protons exists in...

See similar textbooks

Similar questions

. How is the strength of an acid related to the fact that a competition for protons exists in aqueous solution between water molecules and the anion of the acid?
Q3- The acid-dissociation constant for chlorous acid, HCIO,, at 25C is 1.0x10. Calcul the concentration of H+ if the initial concentration of acid is 0.100 M. d Q4- How many grams of sodium hydroxide (M.wi=58.5) can be added 0 2.5 liter of a solution mixture of 0.3M ammonia and 0.15M ammonium chloride without changi POH by more than lunit? Ky=1.8x 10°? w
A 250 cm3 volumetric flask contains exactly 200,0 cm3 of a 0,025 mol.dm3sulphuric acid solution. Thereafter ten (10) sodium hydroxide pellets, eachof mass 0,1 g are dropped into the flask. After the pellets have dissolvedcompletely, the flask is topped to the 250 cm3 mark with water and thecontents are thoroughly homogenised. Determine the pH of the resultingsolution.
The pH and Kh of 0.1N NH4CI solution, if Kb for NH4OH at 25°C is 1.8x10-5 :will be respectively equal to
p Please don't provide handwriteen solution
Prepared buffer solution GivenAmmonia Volume = 68 mL | Ammonia Concentration = 0.17 MAmmonium Chloride Volume = 42 mL | Ammonium Chloride Concentration = 0.13 MDissociation Constant of Ammonia: 1.8x10-5What is the final concentration of the base
Hi hlo Expert Hand written solution is not allowed. Give proper explanation of the answer please.
please answer number 1 and 2 (if possible pls answer #3 too) with solutions
We have assumed [CO32-] << [HCO3] in our precedent calculation and accordingly ignored the [CO3²-] contribution. Explain why it is a good assumption to make for most natural waters. Note: the common pH range in natural waters is 5.5 to 8.5. (Hint: either use the second acid dissociation constant expression, or a quick sketch of the carbonate system Bjerrum plot to demonstrate your
Present clear legible solutions and answers thank you
From the fact that acetic acid (CH3COOH) is 1.30% ionized in 0.10M of aqueous solution, calculatea. Ionization constant of acetic acidb. Percentage ionization in 0.20M solution
How to write the methodology? I have a practical of the MEASUREMENT USING PH METER, I don't know how to write the methodology. Here is the introduction: A pH meter is an electronic device mainly used for qualitative measurement, for thedetermination of acid and the basic value of a solution. Generally, it measures thehydrogen ion concentration/activity [H+] in a solution. It is denoted as:pH = - log10 [H+]In a pure water solution, the concentration of [H+] and [OH-] ions, respectively, rangefrom 1.0 x 10-1 M to 1.0 x 10-14 M. When [H+] is equal to [OH-] as when pure waterdissociates, the hydrogen ion concentration of pure water is equal to 1.0 x 10-7 M orpH = 7.00, defined as a neutral solution at 25°C, to be of temperaturedependent/endothermic dissociation.[H+] = [OH-] = 1.0 x 10-7 MWhen an ionic or polar substance is dissolved in water, it may change the relativenumbers of H+ and OH-. The higher the pH number, the lower the hydrogen ion concentration, and vice versa. Solution with an…