Answered: What is the pH of a 1.2 M pyridine…

What is the pH of a 1.2 M pyridine solution that has Kp = 1.9 x 10 9? The equation for the dissociation of pyridine is C5H5N(aq) + H2O(1)= C5H5NH*(aq) + OH"(aq). 10.68 9.68 8.72 4.32

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...

See similar textbooks

Related questions

Q: Formic acid, HCOOH, ionizes in water according to the following equation. The equilibrium constant…

Q: -7 The acid dissociation constant K, of alloxanic acid (HC,H,N,O,) is 2.24 x 10'. Calculate the pH…

Q: A solution is prepared at 25 °C that is initially 0.26M in chloroacetic acid (HCH,CICO,), a weak…

Q: The chemical equation for the dissociation of HSO4 in water HSO4 (aq) H(aq) + SO4² (aq) a2 K₁2 = 1.2…

Q: Identify the correct equation for the equilibrium constant K, for the weak acid dissociation of…

A: Equilibrium constant expression is the ratio of the product of concentration of each reactant raised…

Q: A solution is prepared at 25 °C that is initially 0.15M in acetic acid (HCH,CO,), a weak acid with…

Q: Calculate the pH at 25 °C of a 0.60M solution of sodium benzoate (NaCH,CO2). Note that benzoic acid…

A: Given: [C6H5CO2−]=0.60M;pKa(C6H5CO2H)=4.20;pH=???Step 1: Write the dissociation of…

Q: 0.244 L of 0.200 M HCl(aq) is combined with 0.0600 L of 0.400 M CH3NH2(aq). What is the pH of the…

A: Given Volume of .200M HCl= 0.244LVolume of 0.400M CH3NH2 = 0.600LKb = 4.4x10-4

Q: Calculate the hydronium ion concentration in an aqueous solution of 7.52x10-2 M ascorbic acid,…

Q: 13. Consider the following acids and their dissociation constants: HPO,2 (aq) + H2O(1) → H3O* (aq) +…

A: 13 (a)

Q: 1) A mixture of 5.1 x 10-3 moles of HSO4 (hydrogen sulfate) is dissolved in 25 mL of water. At…

A: The question is based on the concept of molarity.molarity is a method of expressing concentration of…

Q: Determine the pH of a 0.74 M aqueous solution of hydrocyanic acid (HCN) and the concentration of all…

A: It refers to the acid dissociation constant having the significance of that fact that how much or…

Q: A solution is prepared at 25 °C that is initially 0.21 M in benzoic acid (HC H₂CO₂), a weak acid…

A: Concentration of benzoic acid = [HC6H5CO2] = 0.21 M Concentration of potassium benzoate = [KC6H5CO2]…

Q: The amino acid glutamine has ionization constants ?a1=6.46×10−3Ka1=6.46×10−3 and…

Q: A solution is prepared at 25 °C that is initially 0.64 M in trimethylamine ((CH3),N).. a weak base…

A: The objective of this question is to calculate the pH of a solution containing a weak base and its…

Q: For the following reaction: NH(aq) + HJSO(aq) =NH (aq) +HSO, (04) Identify the correct description…

A: an acid is a species which donates Proton while a base accepts proton.An acid after donating Protons…

Q: The reaction of the weak acid HCN with the strong base KOH is HCN(aq) + KOH(aq) HOH(1) + KCN(aq) To…

Q: Chlorine gas used for disinfection combines with water to form hypochlorous acid (HOCI). The HOCI…

A: Given, Reversible reaction : HOCl ⇌ H+ + OCl- K=2.7×10-8

Q: A solution is prepared at 25 °C that is initially 0.089 M in propanoic acid (HC₂H-CO₂), a weak acid…

A: Concentration of propanoic acid = [HC2H5CO2] = 0.089 M Concentration of potassium propanoate =…

Q: Write the equilibrium constant expression, K,

A: It is the ratio of product of concentration of products raised to their stoichiometric coefficient…

Q: 1) Calculate the pH of a solution prepared by dissolving 1.45 g of sodium acetate, CH3COONa, in 50.0…

Q: Consider the weak bases below and their Kp values: Ky = 1.8 x 10-5 Kp = 5.6 x 10-4 10-9 NH3 C2H5NH2…

A: Given is , bases and their Kb.

Q: What is the pH at 25 °C of water saturated with CO2 at a partial pressure of 1.10 atm? The Henry’s…

Q: Calculate the change in pH when 9.00 of 0.100 M HCl * (aq) is added to 100.0 of a buffer solution…

Q: The following reactions 1) CIO (aq) + HF (aq) F (aq) + HCIO (aq) 2) CIO (aq)+ CH5COOH (aq)HCIO (aq)…

Q: The lactate ion, C,H,O7 (aq), reacts with water to form lactic acid and hydroxide ion. C,H;05 (aq) +…

A: Given : [OH-] = 5.2 x 10-6 M So as per ICE table x = 5.2 x 10-6 M

Q: Calculate the pH of 1.0 M hydrazinium chloride, N2H5CI. For hydrazine, N2H4, Kp = 1.3 x 106. pH =…

Q: A weak base has a base hydrolysis constant, Kp, of 5.5 x 10-6. What is the pH of a 0.21 M solution…

A: The question is based on the concept of chemical equilibrium. we have to calculate pH of the given…

Q: Trimethylamine, (CH3)3N, is a gas with a fishy, ammonia-like odor. An aqueous solution that is 0.36…

A: Given, pH = 11.68 We know that, pH + pOH = 14 And, pOH = -log[OH-] Thus, pOH = 14-pH =>…

Q: A solution is prepared at 25 °C that is initially 0.27M in chloroacetic acid (HCH₂CICO₂), a weak…

A: pH of buffer solution is calculated by using Henderson Hesselbalch equation.

Q: In the study of biochemical processes, a common buffering agent is the weak base…

A: The objective of the question is to determine the additional volume of .

Q: Phosphoric acid, H₂PO4 (aq), is a triprotic acid, meaning that one molecule of the acid has three…

A: Given dataDetermine the concentration of all species in a phosphoric acid solution. is a unit of…

Q: 11.An acid-base equilibrium system is created by dissolving 0.20mol CH3COOH in water and diluting…

Q: Calculate the pH at 25 °C of a 0.44 M solution of lidocaine HCI (C14H2]NONH,CI). Note that lidocaine…

A: Solution of iodocain HCl is (C14H21NONH2Cl) = 0.44 M, pKb of weak base iodocaine (C14H21NONH) =7.94…

Q: Find the pH of 0.54 M C5H5N(aq) given that its Kb = 1.7×10-9.

Q: A solution is prepared at 25 °C that is initially 0.22M in diethylamine ((C,H5)¸NH), a weak base…

Q: The acid dissociation constant K, of boric acid (H,BO3) is 5.8 × 10 Calculate the pH of a 2.5M…

A: Give, the dissociation constant (Ka) of boric acid = 5.8×10-10 We have to calculate the pH of a 2.5…

Q: If the pH of a 0.200 M solution of the CICH2O¯ ion is 12.05, then what is the value for the basicity…

A: Given: pH = 12.05 Thus, pOH = 14 - 12.05 = 1.95 As pOH = -log[OH-] Thus, [OH-] = 10-pOH = 10-1.95 =…

Q: Use the modified H-H shown below to calculate the blood plasma pH under the following conditions:…

A: [HCO3-] = 0.022 M = 0.022 mol/L = 22 mmol/L pCO2 = 46 mmHg pH = 6.1 + log[HCO3-]0.03×pCO2 pH = ?…

Question

What is the pH of a 1.2 M pyridine solution that has Kh = 1.9 x 10-9? The equation for the dissociation of pyridine is
C5H5N(aq) + H20() = C5H5NH*(aq) + OH"(aq).
10.68
9.68
8.72
4.32

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Step 5

Step 6

Step 7

Trending now

This is a popular solution!

Step by step

Solved in 7 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Formic acid, HCOOH, is the simplest of the carboxylic acids and occurs naturally, most notably in some ants. If the formate (HCOO–) concentration is 0.100 M, determine the formic acid (HCOOH) concentration required to buffer a solution at pH = 3.35 HCOOH(aq) ↔ HCOO–(aq) + H+(aq) Ka = 1.80 × 10-4 i) Calculate the pKa of the acid and provide your final answer with 3 decimal places ii) Write the main equation that you will use to help you calculate the formic acid concentration iii) Calculate the formic acid concentration required to buffer the solution at pH = 3.35 and provide your final answer with 3 decimal places
Calculate the equilibrium constant for the following reaction: CH3COOH(aq) + F¯ (aq)=CH₂COO (aq) + HF (aq) Be sure your answer has the correct number of significant digits. Note: Reference the K of acids at 25 °C table for additional information. a x10 x S
a A solution is prepared at 25 °C that is initially 0.55M in benzoic acid (HCH CO₂), a weak acid with K = 6.3 × 105, and 1.3M in potassium benzoate (KC,H,CO₂). Calculate the pH of the solution. Round your answer to 2 decimal places. pH = ☐ X
25. (a) What is a Brønsted-Lowry acid? (b) What is a Brønsted-Lowry base? (c) Use the following chemical equation to explain these concepts and (d) to identify the conjugate acid-base pairs. Point form is both accepted and expected for this question. ( + CO3 (aq) (aq) 2- HCO3 (ag) + S² = HS, (aq)
1. the temperature for each solution is carried out at approximately 297 K where Kw = 1.00 x 10 ^-14 (a) 0.20 g of hydrogen chloride (HCl) is dissolved in water to make 4.5 L of solution. What is the pH of the resulting hydrochloric acid solution? (b) 0.70 g of sodium hydroxide (NaOH) pellets are dissolved in water to make 3.0 L of solution. What is the pH of this solution ?
A solution is prepared at 25 °C that is initially 0.46 M in acetic acid (HCH₂CO₂), a weak acid with K=1.8 × 10¯, and 0.022 Min sodium acetate (NaCH3CO₂). Calculate the pH of the solution. Round your answer to 2 decimal places. pH = 0 X 5
What’s the PH of this question
A diprotic acid, H, A, has acid dissociation constants of K,j = 1.45 x 10-4 and K2 = 5.12 x 10-". Calculate the pH and molar concentrations of H,A, HA, and A²- at equilibrium for each of the solutions. A 0.184 M solution of H,A. pH = 2.2865 [H,A] = 0.1788 [HA"] = 5.17 xI10-3 [A?-] = M 5.12 x10-11 M A 0.184 M solution of NaHA. pH= [H,A] = M. [HA-] = [A2-] = M M
In the following acid-base equilibria of weak acids in water, label the acid (A), the base (B), the conjugate acid (CA), and the conjugate base (CB). HCIO,(aq) + H,O(1) = H,O*(aq) + C1O, (aq) H₂CO3(aq) + H₂O(1) H₂O+ (aq) + HCO3(aq) H,O(1) +CH,NH (aq) = CH,NH,(aq) + H,O*(aq) O CH₂COOH(aq) + H₂O(1) ⇒ CH₂COO¯(aq) + H₂O+ (aq) O B Answer Bank CA A CB
What is the pH of 0.52M (CH3)3N(aq)? Kb = 6.5 x 10-5 Answer to 2 decimal places.
Calculate the molar concentrations of H2S, HS-, S2-, H3O+, and OH- in 0.065 M H2S(aq). Use the values for the successive acidity constants for H2S in the given table.
You are on one of Saturn's many moons and discover a substance, Y2O that undergoes autoionization just like water on Earth. Y2O + Y2O ⇌ Y3O+ + OY– Through a series of experiments, you determine the equilibrium constant (Keq) for this autoionization reaction at various temperatures. The value of Keq at 28.7ºC is 7.6 x 10-14. What is the pY of the pure substance at this temperature? Report your answer to the hundreths place