In a 1.7 mM aqueous solution of acetic acid (CH,CO,H), what is the percentage of acetic acid that is dissociated? You can find some data that is useful for solving this problem in the ALEKS Data resource. Round your answer to 2 significant digits. do 0% の

In a 1.7 mM aqueous solution of acetic acid (CH,CO,H), what is the percentage of acetic acid that is dissociated? You can find some data that is useful for solving this problem in the ALEKS Data resource. Round your answer to 2 significant digits. do 0% の

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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For acid solutions comprised of a moderately concentrated mixture of strong and weak acids, the [H+] concentration is approximately equal to the concentration of the strong acid (e.g. HNO3). This approximation applies to the acid rain experiment you are about to carry out. In your experiment, acid rain samples will involve the following reactions: weak acid : HNO2 H + + NO− strong acid : HNO3 ⎯ → H + + NO− From these reactions, you can recognize that the strong acid, nitric acid, completely dissociates into hydrogen ions and nitrate ions, whereas the weak acid, nitrous acid, is predominately in its molecular form, HNO2. B. The total acid concentration (nitric + nitrous acid) of the 10.0 mL solution of “acid rain” is determined by an acid-base titration method. You add 5.00 mL of the titrant sodium hydroxide with a concentration of 0.0114 M to reach the endpoint. i. What is the number of moles of hydroxide ions added? ii.Write one net ionic equation for the…
For acid solutions comprised of a moderately concentrated mixture of strong and weak acids, the [H+] concentration is approximately equal to the concentration of the strong acid (e.g. HNO3). This approximation applies to the acid rain experiment you are about to carry out. In your experiment, acid rain samples will involve the following reactions: weak acid : HNO2 H + + NO− strong acid : HNO3 ⎯ → H + + NO− From these reactions, you can recognize that the strong acid, nitric acid, completely dissociates into hydrogen ions and nitrate ions, whereas the weak acid, nitrous acid, is predominately in its molecular form, HNO2. A. One simple way to measure the [H+] is to measure pH. If a 10.0mL solution of “acid rain” is measured to have a pH=2.77, what is the concentration of strong acid, HNO3, formed? Hint: pH=-log[H+] and 10–pH= [H+], where [H+] is in molarity units.
Complete the following: 1. Random error, also called _________arises from the effects of uncontrolled variables in the measurement. 2. The ____________,measures how closely the data are clustered about mean. 3. The chemical equilibrium in which all the reactants and products are in the same phase are called____________. 4. Reaction that go to completion and never proceed in the reverse direction are said to be_____________ 5. The equation for buffer is the__________equation. 6. A ___________solution is one that resists changes in pH when small quantities of an acid or an alkali added to it. 7. __________is the pH of the pure, neutral and polyprotic
25.0 cm³ sodium hydroxide is neutralized by 15.0 cm³ sulphuric acid of concentration 0.10 mol dm-3. a. Write the equation for the reaction b. From the equation, determine how many moles of sulphuric acid will neutralize 1.0 mol of sodium hydroxide. c. Determine how many moles of sulphuric acid are used in the neutralization. d. Determine the concentration of sodium hydroxide.
Determine the pHpH of an HNO2HNO2 solution of each of the following concentrations. Part A 0.510 MM Express your answer to two decimal places. pHpH = nothing SubmitRequest Answer Part B 0.110 MM Express your answer to two decimal places. pHpH = nothing SubmitRequest Answer Part C 1.40×10−2 MM Express your answer to two decimal places. pHpH = nothing SubmitRequest Answer Part D In which cases can you not make the simplifying assumption that x is small? In which cases can you not make the simplifying assumption that x is small? only in (b) only in (a) in (b) and (c) in (a) and (b) SubmitRequest Answer Provide Feedback Next
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?
Q5 chapter 15 titration: multimedia activities Solve asap
Rainwater is naturally acidic due to the formation of carbonic acid from dissolved carbon dioxide (CO2)(CO2). Atmospheric sulfur oxides, produced when coal is burned for fuel, can cause rainwater to become even more acidic. In some locations, pH values below 5 have been measured. Results of the increasing acidity include increased ocean acidification, slowed coral growth, and damage to marble statues. Balance the equations related to the acidification of rain by inserting coefficients as needed. If the equation is already balanced, leave it as is. equation 1: S+O2⟶SO2S+O2⟶SO2 equation 2: SO2+O2⟶SO3
In this assignment, you will determine the mass % of an unknown sample of baking soda (NaHCO3) by titrating it with an HCl solution of known concentration. The laboratory will open with a beaker on the stir plate with 1.5000 g of impure solid NaHCO3 and with sufficient water added to make the total volume 25.00 mL. The buret will be filled with 0.3015 M HCl. Pouring HCI until pH is 2. The volume in the buret went from 0 mL to 43 mL Question 1: Calculate the moles of HCl transferred during the titration. (number and unit) (Keep four significant digits in all of the calculations.) Question 2: How many moles of NaHCO3 are present in the sample? Question 3: What mass of NaHCO3 is present in the sample? Question 4: What percent of the original sample mass was NaHCO3?
Aniline, abbreviated fNH2, where f is C6H5, is an important organic base used in the manufacture of dyes. It has Kb = 4.3 * 10 - 10. In a certain manufacturing process it is necessary to keep the concentration of fNH3+ (aniline’s conjugate acid, the anilinium ion) below 1.0 * 10 - 9 M in a solution that is 0.10 M in aniline. Find the concentration of NaOH required for this process.
it is time for the titration. You measure 15.0 mL of the H2C2O4 solution with a 100-mL graduated cylinder and add it to a 125-mL Erlenmeyer flask. Then you add two drops of the indicator, phenolphthalein, to the oxalic acid solution in the flask. You dispense the NaOH solution from the buret into the flask (while swirling the flask) until you reach the endpoint. At the endpoint, the solution in the flask turns light pink. You repeat the titration two additional times for a total of three trials. H2C2O4 (aq) + 2 NaOH (aq) --> Na2C2O4 (aq) + 2 H2O (l) (I) (II) (III) Volume of H2C2O4 used 15.00 mL 15.00 mL 15.00 mL Initial Buret Reading 0.00 mL 0.05 mL 0.10 mL Final Buret Reading 14.45 mL 14.38 mL 15.40 mL what Volume of NaOH is used ?
it is time for the titration. You measure 15.0 mL of the H2C2O4 solution with a 100-mL graduated cylinder and add it to a 125-mL Erlenmeyer flask. Then you add two drops of the indicator, phenolphthalein, to the oxalic acid solution in the flask. You dispense the NaOH solution from the buret into the flask (while swirling the flask) until you reach the endpoint. At the endpoint, the solution in the flask turns light pink. You repeat the titration two additional times for a total of three trials. H2C2O4 (aq) + 2 NaOH (aq) --> Na2C2O4 (aq) + 2 H2O (l) (I) (II) (III) Volume of H2C2O4 used 15.00 mL 15.00 mL 15.00 mL Initial Buret Reading 0.00 mL 0.05 mL 0.10 mL Final Buret Reading 14.45 mL 14.38 mL 15.40 mL Volume NaOH used ________mL ________mL ______mL Moles NaOH _______M ________M _________M…