Post-lab Acids and Bases (1212K)

Acids & Bases: Understanding Connections Between Descriptions if Weak Acid Dissociations For a certain acid pka is 3.58. Calculate the pH at which an aqueous solution of this acid would be 6.5% dissociated. Round your answer to 2 decimal places.    *Photo included below

Formic acid dissociates reversibly according to the following equation. [       /20] HCOOH(aq) ⇌ HCOO-(aq) + H+(aq) Write the law of mass action for this equilibrium.K = Is the equilibrium constant in (a) a Ka? Briefly explain. If a solution is initially 0.20 mol/L HCOOH and the equilibrium constant in (a) is 1.8 × 10-4, what is the concentration of hydrogen ions at equilibrium? Show your work.             Use the value obtained in (c) to find the solution’s pH and pOH at 25 °C. If you were unable to complete (c), you may assume a 0.0030 mol/L concentration of hydrogen ions. Would the addition of sodium formate (NaHCOO) to this solution increase pH? Explain.

Draw the Lewis structure of the 1:1 adduct that forms in the Lewis acid-base reaction between boron trifluoride (BF3) and dimethyl ether ((CH3)20). . Explicitly draw all H atoms. . Include all valence lone pairs in your answer. . Do not include charges in your answer. They will not be considered in the grading. . In cases where there is more than one answer, just draw one. O Q [ ] در ? Ⓡ ChemDoodle

If the concentration of an acid in solution is 2.2 times larger than the concentration of its conjugate base, and the pH of the solution is 3.5, what is the pKa of the acid? Include the answer to 3 significant figures

Use resonance structures to predict which is more acidic: phenol (C6H5OH) or ethanol (CH3CH₂OH). (Hint: phenol has a six membered carbon ring) Use the editor to format your answer

PLEASE PLACE THE ANSWERS IN A SQUARE BOXES SAME AS THE QUESTION. SO I COULD KNOW WHICH ANSWERS BELONGS TO THE RIGHT PLACE.

How do you determine which side the reaction favors in acid base equilibrium problems such as this one?  Subject: Organix Chemistry

in text form with proper workings and explanation for each and every part and steps with concept and introduction no AI no copy paste remember answer must be in proper format with all working!!!!!!!

Calculate the pKa value for each of the following acids: Remember to use the rules for significant figures in reporting your answer. a)  Phosphoric acid (H3PO4),   ??=4.5×10−4Ka=4.5×10−4     pKa =    b)  Propanoic acid  (HC3H5O2),  ??=1.3×10−5Ka=1.3×10−5     pKa =

Select the correct answers: “Ocean acidification is a process that occurs when atmospheric carbon dioxide dissolves in the ocean and is subsequently converted into (methane; carbonic acid; carbonate ions; sodium carbonite) . This then causes the pH of the ocean to (increase; decrease; fractionate; multiply) and become more acidic.”

Refer to the following ionization of hypochlorous acid: HOCI (aq) + H₂O (1) H3O+ (aq) + OCI (aq) a. The acid-dissociation constant, Ka, for hypochlorous acid, HOCI, is 3.5 X 10-8. Calculate the equilibrium concentrations of H3O+, OCI, and HOCI if the initial concentration of HOCI is 0.125 M. b. Calculate the pH and pOH of the above solution once equilibrium is established.

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CHEMISTRY RATE WILL BE GIVEN! NO LONG EXPLANATION NEEDED.  PLEASE ANSWER 47-52

Calculate at what pH about 80% of 2-naphthol (pKa = 9.5) will be found in the ionized form in aqueous solution. Write your answer in numerical form with one diciminal digit (e.g. 1.1) Answer:

For the Brønsted acid-base reaction shown below, determine the conjugate acid- base pairs. Then give the curved-arrow notation for the reaction in the left-to-right direction :0: :O: Нзс- H–Ö-H -> Нзс A D Fill in the blanks with the letters A,B,C, and D, representing the species in the reaction above. (It doesn't matter which pair you list first.) Pair 1: Pair 2: acid and its conjugate base acid and its conjugate base

14. In aqueous solution, hydrazine is a base that can accept two protons: N₂H4(aq) + H₂O(l) ≥ N₂H5†(aq) + OH-(aq) Kb1 = 8.5 x 10-7 N₂H5+ (aq) + H₂O(1) ≥ N₂H6²¹(aq) + OH-(aq) Kb2 = 8.9 x 10-16 a. What is the pH of a 0.015 mol.L-¹ hydrazine solution? | b. What is the concentration of N2₂H4, N₂H5†, and N₂H6²+ at equilibrium?

For the reaction below (the one you will be studying during this lab), write an expression for the reaction rate in terms of changing concentration over time for each species in the overall reaction (one is given as an example).  S2O82- (aq) + 3I- (aq) ⇌ 2SO42- (aq) +I3- (aq)   What does it mean if a concentration change over time is written as being negative? What does it mean if a concentration change over time is written as being positive?

Compare the two reactions with different Lewis bases and the same Lewis acid. include the kinetic aspect and thermodynamic aspect with detailed structural features and mechanisms.

Reaction: CrO42-(aq)+2H+(aq) <--> Cr2O72-(aq)+H2O(l)                 YELLOW                            ORANGE If sulfuric acid (H2SO4) is added to this solution, will a color change be observed? If so, how does the addition of sulfuric acid result in a color change? Explain your reasoning by showing the effect of the addition of H2SO4 on the equilibrium for the reaction.

Write the chemical equation for the reaction of carbonic acid (H, CO,) with water and identify the acid dissociation constant expression (acidity constant expression) for this reaction. STRATEGY 1. Write the formula for the conjugate base of carbonic acid. 2. Identify the reactants and the products. 3. Write the Ka expression for a generalized reaction. Steps 1 and 2: The reactants are carbonic acid, H, CO,, and water, H, O. The products are the hydrogen carbonate ion, HCO,, and the hydronium ion, H, O*. Step 3: Write the Ka expression for the generalized reaction aA(aq) + bB(1) cC(aq)+ dD(aq) Answer Bank K = [A] [D] [B]* [C] [B] [A]" [DF [C)

Find the value of the equilibrium constant for the following equilibrium HAsO42–(aq) + H2O(l) ⇌ H2AsO4–(aq) + OH–(aq) given the acid ionization constants for H3AsO4: pKa1=2.26, pKa2=6.77, pKa3=11.29.   A 1.8 x 10–12 B 2.0 x 10–3 C 5.9 x 10–8 D 5.5 x 10–3 E 1.7 x 10–7

3 PNW Fall 2023 CHM 11600-006 General Chemistry LEC = ACIDS AND BASES Interconverting Ka and pka acid A Complete the following table, which lists information about the measured acid dissociation constants of three unknown weak acids. Note: be sure each number you put in the table has the correct number of significant digits. B с Explanation Ka 0 2.8 × 10 Check 9 pKa 7.9 1.142 A ALEKS - Leticia Jimenez - Learn 0 relative strength (Choose one) (Choose one) (Choose one) x10 www-awa.aleks.com X b Answered: Complete the following table, which... | bartl... Ś 1/5 HOAPOS Staff Site Leticia V 09: 00. 18 18 © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility +

lem 10.10 -Enhanced - with Feedback Part A Enter the formula of the conjugate base for the acid H2PO4. Express your answer as a chemical formula. ΑΣφ a Xh 1L ↑

Formic acid dissociates reversibly according to the following equation. HCOOH(aq) ⇌ HCOO-(aq) + H+(aq) Write the law of mass action for this equilibrium.K = Is the equilibrium constant in (a) a Ka? Briefly explain. If a solution is initially 0.20 mol/L HCOOH and the equilibrium constant in (a) is 1.8 × 10-4, what is the concentration of hydrogen ions at equilibrium? Show your work.

Formic acid dissociates reversibly according to the following equation. HCOOH(aq) ⇌ HCOO-(aq) + H+(aq) Write the law of mass action for this equilibrium.K = Is the equilibrium constant in (a) a Ka? Briefly explain. If a solution is initially 0.20 mol/L HCOOH and the equilibrium constant in (a) is 1.8 × 10-4, what is the concentration of hydrogen ions at equilibrium? Show your work.  4.Use the value obtained in (c) to find the solution’s pH and pOH at 25 °C. If you were unable to complete (c), you may assume a 0.0030 mol/L concentration of hydrogen ions. 5.Would the addition of sodium formate (NaHCOO) to this solution increase pH? Explain.

Formic acid dissociates reversibly according to the following equation. HCOOH(aq) ⇌ HCOO-(aq) + H+(aq) Write the law of mass action for this equilibrium.K = Is the equilibrium constant in (a) a Ka? Briefly explain. If a solution is initially 0.20 mol/L HCOOH and the equilibrium constant in (a) is 1.8 × 10-4, what is the concentration of hydrogen ions at equilibrium? Show your work.         question 4, 5 need to be solved   4.Use the value obtained in (c) to find the solution’s pH and pOH at 25 °C. If you were unable to complete (c), you may assume a 0.0030 mol/L concentration of hydrogen ions. 5.Would the addition of sodium formate (NaHCOO) to this solution increase pH? Explain.

Compare the relative acidity of 1-molar aqueous solutions of the following acids.NH4Cl CH3COOH BrCH2COOH F3CCOOH H2SO4 HCl HBrpKa = 9.26 pKa = 4.74 pKa = 2.9 pKa = 0.2 pKa = -5 pKa = -7 pKa = -9

using the data in the table, indicate which direction the equilibrium will lie for each of the following acid/base reactions. Use an arrow to indicate the direction of the equilibrium

← → C view-source:https://... * Question Completion Status: esc blackboard.matc.edu/webapps/assessment/take/launch.jsp?course_assessment_id=_827 QUESTION 9 Choose all acids: ⒸH3PO4 Cu(NO3)2 ☐ Ca3(PO4)2 NH3 KF ! HCI C₂H5OH ☐ H₂SO4 со Li₂SO4 Click Save and Submit to save and submit. Click Save All Answers to save all answers. ← @ 个 #m с THE tA 78 % MD hp Ill & I

I need help with this problem. Compare the pH of propionic acid and nitric acid when they are dissolved in water at a concentration of 20 mM using the "Arrhenius Concept". Include:a balanced equation describing the acid-base reactions involvedThe calculation of the pKa for bothThe calculation of the two pH's (of propionic acid and nitric acid when they are dissolved in water at a concentration of 20 mM)and A calculation of the percent of dissociation of both propionic acid and nitric acid.The gibbs free energy ΔG are listed as the following:Nitric acid: -152 kJ/molPropionic Acid : -291 kJ/molPropionate: -361 kJ/mol

Complete the following table, which lists information about the measured acid dissociation constants of three unknown weak acids. Note: be sure each number you put in the table has the correct number of significant digits.