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.

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

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.

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.

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

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

1. Compare your pKa, Ka and molar mass from your experiment to the expected values for KHP. How well do they compare? What might account for the differences? 2. Based on your results in Part 1, is the method used reliable in determining pKa, Ka and molar mass of a weak acid? Explain. 3. Discuss your thinking on how you determined the identity of your unknown. Were there two (or more) acids that were difficult for you to distinguish between? If so, how did you makeyour final decision?

1. Compare your pKa, Ka and molar mass from your experiment to the expected values for KHP. How well do they compare? What might account for the differences? 2. Based on your results in Part 1, is the method used reliable in determining pKa, Ka and molar mass of a weak acid? Explain. 3. Discuss your thinking on how you determined the identity of your unknown. Were there two (or more) acids that were difficult for you to distinguish between? If so, how did you makeyour final decision?

1. Compare your pKa, Ka and molar mass from your experiment to the expected values for KHP. How well do they compare? What might account for the differences? 2. Based on your results in Part 1, is the method used reliable in determining pKa, Ka and molar mass of a weak acid? Explain. 3. Discuss your thinking on how you determined the identity of your unknown. Were there two (or more) acids that were difficult for you to distinguish between? If so, how did you makeyour final decision?

Determine the pH (to two decimal places) of the following solution. A table of pKa values can be found here. If the 5% approximation is valid, use the assumption to compute pH. 3.15×10-3 M triethylamine

What is the acid dissociation constant Ka for its conjugate acid? If the base dissociation constant Kb for hypochlorite ion is 3.3x10-7

A Dashboard 101 Chem101 + а ap.101edu.co Question 10 of 16 Submit Complete the balanced chemical reaction for the following weak base with a strong acid. In this case, write the resulting acid and base as its own species in the reaction. NH:(aq) + HCI(aq) - 14- O3- |2+ 3+ 14+ 1 2 3 4 7 9. 1 I5 16 (s) (g) (aq) H3O+ H2O OH- CI Reset • x H2O Delete + 10:24 PM P Type here to search 65°F Mostly sunny 10/31/2021 1L

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

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 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 ||

Reacting GeO2 with H2O forms the tetraprotic (four H+ ions) acid, H4GeO4.  On a piece of paper, write down the chemical equations for the four acid dissociation equilibria.  Match each chemical species below with its correct (hypothetical) pKa value. Group of answer choices H4GeO4              [ Choose ]             12.70             10.24             6.91             4.56            H3GeO4 -              [ Choose ]             12.70             10.24             6.91             4.56            H2GeO4 2-              [ Choose ]             12.70             10.24             6.91             4.56            HGeO4 3-              [ Choose ]             12.70             10.24             6.91             4.56

In Experiment 4, we used titration to determine the total acid content of samples, which we reported in terms of molarity. Reporting acidity through pH measurements is quite different, in that we can only measure the amount of the acid in its ionized form. You were tasked to investigate a clear aqueous solution of an unknown monoprotic acid. You decided to use two Chem 16.1 methods to gather data.Method 1 – TITRATION: A 10. mL aliquot of the sample was diluted with 25 mL distilled water. Two drops of phenolphthalein were added and then it was titrated 3.54 mL of 0.048 M standardized NaOH to the endpoint.Method 2 – pH STRIP: You took 1 mL of the sample and used a pH strip to estimate the pH, which turned out to be around 3.3. Another 1 mL of the sample was diluted with 9 mL of water. The pH was taken again and is now around 3.8 d) Based on your answer in a) and c), do you think the unknown is really a strong acid or is it a weak acid instead? Defend your answer in one sentence.e)…