CHEMISTRY 3ThiChung Le

For acetic acid, justify the acidity values ​​in the three media below: - solvent: water (pka = 4.8) - solvent: 20% methanol - 80% water (pKa = 5.1) - solvent: 20% dioxane - 80% water (pKa = 5.3)

For each of the following acids or bases belowa) Label the following acids and bases as strong acid/strong base/weak acid/weak base.b) Write equations showing the dissociation of the following acids/bases (pay special attention towhich arrow you draw between reactants and products).c) Draw a molecular level diagram showing the beaker at the end of the reaction of acid/base withwater.1. HBrO4 2. HIO3 3.

Acid-Base Reaction A. Kremil-S and Vinegar 1. Dissolve a tablet of Kremil-S in a plastic cup with few amounts of water. Mix thoroughly. 2. Add one (1) tablespoon of vinegar to the mixture containing Kremil-S and observe the reaction. Take photos of the setup and the reaction. B. Baking Soda and Vinegar 1. Put at least five (5) tablespoons of baking soda inside the balloon using a funnel. 2. Add half a cup of vinegar to the bottle, and carefully stretch the opening of the balloon over the mouth of the bottle. 3. Drop the baking soda into the vinegar inside the bottle and observe the reaction. Oxidation-Reduction Reaction A. Vitamin C and Betadine 1. Dissolve one (1) Vitamin C tablet in a small amount of water in a cup. 2. Add dropwise amounts of Betadine while slowly stirring. Observe the reaction. B. Bleach and Betadine 1. Put a small amount of liquid bleach in a cup. If your bleach is in powder form, dissolve it in a small amount of water in a cup. 2. Add dropwise amounts of Betadine…

NaHSO3 is a salt, which ionized completely to give HSO3-  ion. the following equations show that this ion can act either as an acid or as a base.              HSO3- + H2O(l) <=> H3O+ + SO3-2             K1 = ?            HSO3- + H2O(l) <=> H2SO3 + OH-            K2 = ? (a) Knowing that for H2SO3:Ka1=1.4x10-2, Ka2 = 6.5x10-8, find K1 and K2. (b)Predict which reaction of the two is more important based on their K values. (c) What is the pH of 0.10 M NaHSO3

Hi. A couple of minutes ago my this same question was rejected and was said incomplete ...  But in my book like that only the question is there ... (Nothing, by the way, seems incomplete ) So I am sending a clear picture once again ..  So please respond to it now  ...' thank you  AND YOUR APP BARTLEBY IS THE BEST APP I HAD EVER MET ...  THANK YOU  and here is the question to be answered  ...   THE QUESTION IS FROM THE CHAPTER ACIDS, BASES AND SALTS

Each value represents a different aqueous solution at 25 °C. Classify each solution as an acid, base, or neutral. [OH−]= 3.0 × 10 − 6 [H+]= 8.1 × 10 − 13 pOH= 13.67 pOH= 7.00 [H+]= 5.3 × 10 − 3 [OH-]= 3.0x 10^-6 is a(n) Question Blank 1 of 5 , [H+]= 8.1 x 10^-13 is a(n) Question Blank 2 of 5 , pOH= 13.67 is a(n) Question Blank 3 of 5 , pOH= 7.00 is a(n) Question Blank 4 of 5 , [H+]= 5.3 x 10^-3 is a(n) Question Blank 5 of 5

Calculate the pH and fraction of dissociation (?) for each of the acetic acid (CH3COOH, p?a=4.756 ) solutions. A 0.00393 M solution of CH3COOH . pH= ?= A 1.93×10−12 M solution of CH3COOH . pH= ?=   (Please type answer no write by hend)

Calculate the concentration of a sulfuric acid solution (H2SO4) if 25.3 mL of concentrated acid (18.4 M) is diluted with enough water to make a 100.0 mL solution (to 3 sig figs).

What is N3− classified as? Group of answer choices strong acid weak acid strong base weak base salt negligible spectator

UPVOTE WILL BE GIVEN! PLEASE ANSWER ALL. THANK YOU! ANSWER IN 3 DECIMAL PLACES. CHEMISTRY! NO LONG EXPLANATION NEEDED.  Calculate the percent dissociation of the acid in each of the following solutions a.  0.50 M acetic acid  b. 0.050 M acetic acid c. 0.0050 M acetic acid

What mass of aluminum hydroxide can be dissolved in a solution whose pH is held at 11.20? (Ksp of aluminum hydroxide = 1.9x10^-33)

Rain with a pH below 5.6 is considered acid rain. The principal cause of acid rain is coal-burning electrical power plants (sulfurous and sulfuric acids are formed in the atmosphere from this). Any combustion reaction that produces high temperature can also produce acid rain (nitrous and nitric acid are produced in the atmosphere from this). Thus, automotive engines are also an important contributor to acid rain. Acid rain harms both living and nonliving things in a variety of ways. What solution/s can you propose to combat acid rain?

H2NNH2 is a weak diprotic base.  Calculate [OH-], [H2NNH3+], [H3NNH32+] and [H3O+] in a 0.1M solution of H2NNH2].  Kb H2NNH2=8.5x10-7, and Kb H2NNH3+]=8.9x10-16.  This is all the information given by the instructor.  Can you do some of the problem?

Selected information about five solutions, each at 24oC, is given in each part.  Fill in the blanks in the missing information for each part.  See the example. For scientific notation values there are two fields:  the number  and then the power of 10 to which the number is raised. Example [?3?+][H3O+]:   1.3 × 10^−13 [??−][OH−]:   7.7 × 10^−2  acidic or basic:   basic  b) [?3?+][H3O+]:  4.2 × 10-6  [??−][OH−]:  X  10^ acidic or basic:  c) [?3?+][H3O+]:   X  10^ [??−][OH−]:  3.3 ×10-10  acidic or basic:

The generic equation for a weak base in water is: ?+?2?⟷??++??−B+H2O⟷BH++OH− A 0.0500 M solution of a base is 7.5% ionized.  Calculate the base ionization constant Kb Input the numerical answer.  Remember significant figures. Do NOT round until the final answer.  There are two fields in which to input the number.  The exponent will go after the 10^ Kb =  x  10^

Case Study Section 1 – pH Based on “The Case of the Mortified Mom: Acids, pH and Buffers” by Terry Platt (National Center for Case Study Teaching in Science)   The Patient: Paramedics were called to the home of the Mathews family because their 3-year old daughter, Molly, had gotten into the medicine cabinet and consumed a large number of aspirin tablets.  When the paramedics arrived Molly had vomited several times, with bits of undissolved tablets visible, but seemed sleepy, almost lethargic.  She was rushed to the nearest Emergency Room.  When she reached the hospital she was unarousable and was breathing rapidly and deeply.  She was examined and lab samples were obtained.     Above is the structure of aspirin, or acetylsalicylic acid, which is a weak acid with a pKa of 3.5.  The active, and toxic at high doses, form is the protonated form.      Under normal conditions this system functions to: Maintain blood pH near physiological pH. Remove excessive H+ generated during…

Case Study Section 1 – pH Based on “The Case of the Mortified Mom: Acids, pH and Buffers” by Terry Platt (National Center for Case Study Teaching in Science)   The Patient: Paramedics were called to the home of the Mathews family because their 3-year old daughter, Molly, had gotten into the medicine cabinet and consumed a large number of aspirin tablets.  When the paramedics arrived Molly had vomited several times, with bits of undissolved tablets visible, but seemed sleepy, almost lethargic.  She was rushed to the nearest Emergency Room.  When she reached the hospital she was unarousable and was breathing rapidly and deeply.  She was examined and lab samples were obtained.     Above is the structure of aspirin, or acetylsalicylic acid, which is a weak acid with a pKa of 3.5.  The active, and toxic at high doses, form is the protonated form.    Question 7: What is the purpose of the activated charcoal? Absorb the residual aspirin to prevent it from entering her bloodstream. Increase…

Case Study Section 1 – pH Based on “The Case of the Mortified Mom: Acids, pH and Buffers” by Terry Platt (National Center for Case Study Teaching in Science)   The Patient: Paramedics were called to the home of the Mathews family because their 3-year old daughter, Molly, had gotten into the medicine cabinet and consumed a large number of aspirin tablets.  When the paramedics arrived Molly had vomited several times, with bits of undissolved tablets visible, but seemed sleepy, almost lethargic.  She was rushed to the nearest Emergency Room.  When she reached the hospital she was unarousable and was breathing rapidly and deeply.  She was examined and lab samples were obtained.     Above is the structure of aspirin, or acetylsalicylic acid, which is a weak acid with a pKa of 3.5.  The active, and toxic at high doses, form is the protonated form.  Question 9: What would be the consequence(s) of lower than normal blood pH? Cause proteins to denature Decrease in enzyme activities Limit…