Post-lab Acids and Bases (1212K)

Determine the dissociation constants for the acids. Express the answers in proper scientific notation where appropriate. Acid A: pKa = 5.0 K₂ = a Acid B: pKa = 8.60 Ka = Acid C: pKa = -2.0 Ka =

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

. Give an example of a Lewis acid-base pair and a frustrated Lewis acid-base pair. What is the difference between these two systems? What is the mechanism for the reaction with H2?

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

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

9:33 Time's Up! Submit Construct the expression for Kb for the weak base, N2H4. N2H4(aq) + H20(1) = OH (aq) + N2H;*(aq) 1 Based on the definition of Kb, drag the tiles to construct the expression for the given base. Kp = 5 RESET [H,O] [H;O*] [OH] [N2Hs] [N;H4] [N;H;] 2[H,O] 2[H,O*] 2[OH] 2[N2H5°] 2[N¿H«] 2[N2H3] [H,O]? [H,O*]? [OH]? [N;Hs']? [N;Ha]? [N2H3 ]? Tap here or pull up for additional resources

How do I know if I use the small x approximation or not? There’s an answer for small x approximation and the answer if we don’t use small x approximation.

For the acid-base reactions below, fill in the boxes by providing the structure of the conjugate base or conjugate acid, and estimating the value of the equilibrium constant, Keq. ' + SH 요 요 ее в осно + Kea но = Kea = Keq = рказ = 5 + CH3OH + H₂ + pka = 35

Write the equilibrium-constant expressions and obtain numerical values for each constant in the basic dissociation of aniline, C6H5NH2. the acidic dissociation of hypochlorous acid, HClO.

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

Q25 P2

help please answer 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 pH of a 0.12 M solution of hydrocyanic acid (HCN), which has a pKa of 9.31. Your answer should have 3 significant figures (i.e. 9.99).

What is the acid dissociation constant (Ka) expression for the following reaction? CH3COOH+H2O=CH3COO-+H3O

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 =

Write the acid dissociation constant expression (Ka ) for the dissociation of HCN.

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.

Due to the pandemic Covid-19, the uses of hand sanitizers are very important among us. Predict and explain the colour of the solution and pH value when red cabbage indicator was added to the hand sanitizers.

Please don't provide handwritten solution ....

The acid dissociation constant K, of hypobromous acid (HBRO) is 2.3 x 10 D. Calculate the pH of a 3.3 M solution of hypobromous acid. Round your answer to 1 decimal place. pH = %3D Continue

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

will hc2h2o4 (not its conjugate) act as an acid or base- pick one of these rationales: because the first proton was already removed leaving a basic molecule behind, because the first proton's pkb value is a larger value, or because the second proton is still acidic based on the second pka being below 7

For relative strength, please rank 1 (strongest) to 3 (weakest).

Calculate the concentration (M) of the anion Z2- for a 0.100 M solution of H2Z  given the acid ionization constants for the acids below. Report your answer to the tenths place using scientific notation and do not include units. (ie. 1.1e+9, 1.1e-9) H2Z(aq) Ka = 7.8 x 10-2 HZ-(aq) Ka = 7.0 x 10-9

The equilibrium constant, K, for a neutralization reaction can be symbolized as Kn- Determine K, at 25 °C for the reaction NH, (aq) + HB1O(aq) = NH†(aq) + BrO¯(aq) using Kw, and the K, and K, values from the ionization constant tables. Kn ||

6. Which of the following bases are strong enough to remove a proton from the acid below? Justify your answer with approximate pKa values. i NH3 acid NH OH

Write the acid dissociation constant expression (K,) for the dissociation of HCN.

H3PO4 is a polyprotic acid with three acidic protons. Be sure to include the proper phases for all species within the reaction. Identify the products of the third acid dissociation of H3PO4 in water. Be sure to include the proper phases for all species within the reaction. HPO4²- (aq) + H₂O(1)