Liquid ammonia (anhydrous NH3(0)) is often used as a solvent. Like water, ammonia undergoes autoionization by the transfer of a proton: 2NH3 = NH4+ + NH2" K = 1x10-33 at -50°C Since ammonia is better proton acceptor than water, the ionization of acids is relatively enhanced in liquid ammonia. For example, acetic acid is a strong acid in liquid ammonia. Estimate [NH4+] (mol/L) in pure (i.e. neutral) liquid ammonia at -50°C. mol/L Submit Answer Tries 0/5 Calculate [NH4+] (mol/L) in a 7.07x10-5 M solution of acetic acid in liquid ammonia at -50°C. mol/L Submit Answer Tries 0/5 Estimate [NH2] (mol/L) in a 7.07x10-5 M solution of acetic acid in liquid ammonia at -50°C.

Liquid ammonia (anhydrous NH3(0)) is often used as a solvent. Like water, ammonia undergoes autoionization by the transfer of a proton: 2NH3 = NH4+ + NH2" K = 1x10-33 at -50°C Since ammonia is better proton acceptor than water, the ionization of acids is relatively enhanced in liquid ammonia. For example, acetic acid is a strong acid in liquid ammonia. Estimate [NH4+] (mol/L) in pure (i.e. neutral) liquid ammonia at -50°C. mol/L Submit Answer Tries 0/5 Calculate [NH4+] (mol/L) in a 7.07x10-5 M solution of acetic acid in liquid ammonia at -50°C. mol/L Submit Answer Tries 0/5 Estimate [NH2] (mol/L) in a 7.07x10-5 M solution of acetic acid in liquid ammonia at -50°C.

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

Similar questions

Which of the following equations represents the acid equilibrium associated with Ка, for H, PO,? A) HPO,2 (aq) + H,O (1) = PO, (aq) + H,O* (aq) B) H,PO, (aq) + H,O (1) = H̟PO, (aq) + H,O* (aq) C) H̟PO, (aq) + H,O (1) = H̟PO, (aq) + OH (aq) D) H,PO, (aq) + H,O (1) = HPO,* (aq) + H,O* (aq) 80 DII DD F2 F3 F4 FS F9 F11 @ $ & ( 2 3 4 6 8 9 W E R S D F G K C V B N M I
6. What is the pH of a 0.250M solution of methyl amine (CH3NH2, Kp = 4.4 x 104)?
What is [OH-] in a solution of 1.25 M NH3 and 0.85 M NHANO3? NH3 (aq) + H20 (1) = NH4+ (aq) + OH- (aq) Kp=1.8x10-5 Write your answer with 2 significant digits.
What is the concentration of a formic acid (HCHO,) solution with a pH = 3.15? The K, of formic acid is 1.8 x 104.
Write the expression for the acid-dissociation constant Ka for HC4H7O2. (Concentration equilibrium expressions take the general form: Kc = [C]c / [A]a . [B]b. Subscripts and superscripts that include letters must be enclosed in braces {}.)
The weak acid 0.250 M HNO2 is dissolved in water. HNO2(aq) ⇌H+ (aq) + NO2− (aq) . The resulting concentration of [H+] is 0.00253 M. Calculate the concentrations of [NO2− ] and [HNO2]. What is the freezing point?
HCIO is a weak acid (K, = 4.0 x 10-) and so the salt NaCIO acts as a weak base. What is the pH of a solution that is 0.039 M in NaCIO at 25 °C7 pH =
Complete the balanced molecular reaction for the following weak base with a strong acid: Na CIO2(aq) + H2SO«(aq) – 4- |2+ 3+ 04+ 1 4 6. 7 8 9 Do (s) (1) (g) (aq) Na CI S H H2O OH Reset x H2O Delete 1L LO
Predict acid-base properties of salts. What is the acid-base nature of the following salts? K₂(HCIO) = 3.50×10-8, K₂((C₂H5)2NH) = 6.9x10-4; Ka(HCIO) = 3.5×10-8 (a) barium hypochlorite, Ba(CIO) 2 (b) diethylammonium hypochlorite, [(C₂H5)2NH₂]CIO Check & Submit Answer Show Annroach
8:43 1 5G E Question 13 of 25 Submit Determine concentration of OH in a 0.60 M solution of HNO2 (Ka = 7.1 x 10-4). 1 2 3 Based on the given values, set up ICE table in order to determine the unknown. HNO2(aq)+ H20(1) =H;O*(aq) + NO, (aq) Initial (M) Change (M) Equilibrium (M) 5 RESET 0.60 7.1 × 10-4 1.4 x 10-11 0.30 +x -X +2x -2x 0.60 + x 0.60 - x 0.60 + 2x 0.020 - 2x 1.4 × 10-1" + x 1.4 × 10-11 - x 1.4 x 10-11 + 2х 1.4 x 10-11 - 2x
When carbon dioxide gas dissolves in water, it reacts with the water to form carbonic acid. This is why soft drinks have a low pH, and soda water is often recommended as a mild cleaning agent. It is also why there is concern that rising levels of atmospheric carbon dioxide may cause the Earth's oceans to become more acidic. Here is the reaction between carbon dioxide gas and water: H₂O(1) + CO₂(g) H₂CO3(aq) Suppose an engineer decides to study the rate of this reaction. He prepares four reaction vessels with 152.7 g of water and 34.3 g of carbon dioxide gas each. The volume and temperature of each vessel is shown in the table below. Arrange the reaction vessels in decreasing order of initial rate of reaction. In other words, select a "1" next to the vessel in which the engineer can reasonably expect the initial rate of reaction to be highest, a "2" next to the vessel in which the initial rate of reaction would be next highest, and so on. vessel volume temperature A B C D 8.0 L 1.0 L…
If the pH of a 0.0850 M solution of HBRO2 is 2.29, then what is the value for the acidity constant, Ką, of HBRO2? HBrO2(aq) + H2O(1) H3O*(aq) + BrO2 (aq) K¸ = ? K, for HB1O2: