EXERCISE 2: Calculate the pH of a 0.50 M NH3 at 25°C.At 25°C, the base dissociation constant (Kb) of ammonia (NH3 ) is 1.8 × 10-5.Complete the ICE Table below:+NH4+ (aq)OH-(aq)Hydrolysis EquationNH3(aq) + H₂O(l)INITIAL0.500(Analytical molarity)CHANGE-X+XEQUILIBRIUM(6 pts)[NH3][NH4*]=[OH-] =Write the equilibrium expression for the base dissociation constant, K, and substitute themathematical equation containing the variable x into the equilibrium expression.Then calculate the value of [OH-] and pH of the solution. Show your complete solution.0+X

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EXERCISE 2: Calculate the pH of a 0.50 M NH3 at 25°C. At 25°C, the base dissociation constant (Kb) of ammonia (NH3 ) is 1.8 × 10-5. Complete the ICE Table below: + Hydrolysis Equation NH4+ (aq) OH (aq) NH3(aq) + H₂O(l) INITIAL 0.50 0 (Analytical molarity) CHANGE -X +X EQUILIBRIUM (6 pts) [NH3] = [NHA] = [OH-] = Write the equilibrium expression for the base dissociation constant, K, and substitute the mathematical equation containing the variable x into the equilibrium expression. Then calculate the value of [OH-] and pH of the solution. Show your complete solution. 0 +X

EXERCISE 2: Calculate the pH of a 0.50 M NH3 at 25°C. At 25°C, the base dissociation constant (Kb) of ammonia (NH3 ) is 1.8 × 10-5. Complete the ICE Table below: + Hydrolysis Equation NH4+ (aq) OH (aq) NH3(aq) + H₂O(l) INITIAL 0.50 0 (Analytical molarity) CHANGE -X +X EQUILIBRIUM (6 pts) [NH3] = [NHA] = [OH-] = Write the equilibrium expression for the base dissociation constant, K, and substitute the mathematical equation containing the variable x into the equilibrium expression. Then calculate the value of [OH-] and pH of the solution. Show your complete solution. 0 +X

General Chemistry - Standalone book (MindTap Course List)

11th Edition

ISBN:9781305580343

Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Chapter15: Acids And Bases

Section15.8: The Ph Of A Solution

Problem 15.10E: A 0.010 M solution of ammonia, NH3, has a pH of 10.6 at 25C. What is the concentration of hydroxide...

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EXERCISE 2: Calculate the pH of a 0.50 M NH3 at 25°C. At 25°C, the base dissociation constant (Kb) of ammonia (NH3) is 1.8 x 10-5. Step 1. Complete the ICE Table below: Hydrolysis Equation NH3(aq) + H₂O(l) NH, (aq) INITIAL 0.50 0 (Analytical molarity) CHANGE -X +X EQUILIBRIUM [NH₂] = [NH₂¹] = [OH] = Step 2. Write the equilibrium expression for the base dissociation constant, Kt Kb = Step 3. Substitute the mathematical equation containing the variable x into the equilibrium expression. Answer: Step 4 Calculate the value of [OH]. Show the complete solution. SOLUTION Step 5. Calculate pH of the solution. Show the complete solution. ( Answer: + OH (aq) 0 +X
EXERCISE 2: Calculate the pH of a 0.50 M NH3 at 25°C. At 25°C, the base dissociation constant (Kb) of ammonia (NH3 ) is 1.8 × 10-5. Step 1. Complete the ICE Table below: NH4+ (aq) Hydrolysis Equation NH3(aq) + H₂O(1) INITIAL 0.50 0 (Analytical molarity) CHANGE -X +X EQUILIBRIUM [NH3] [NHA] = [OH-] = Step 2. Write the equilibrium expression for the base dissociation constant, K Kb = Step 3. Substitute the mathematical equation containing the variable x into the equilibrium expression. Answer: Step 4 Calculate the value of [OH-]. Show the complete solution. SOLUTION Step 5. Calculate pH of the solution. Show the complete solution. Answer: X + OH (aq) 0 +X
EXERCISE 1: Calculate the pH of a 0.50 M HA at 25°C. At 25°C, the acid dissociation constant (K₂) of the monoprotic weak acid, HA, is 7.2 x 10-6. Step 1. Complete the ICE Table below: Dissociation Equation H+ (aq) A-(aq) INITIAL 0 Concentration CHANGE +X EQUILIBRIUM Concentration [HA] = [H+] = [A-] = Step 2. Write the equilibrium expression for the acid dissociation constant, Ka. Ka = Step 3. Substitute the mathematical equation containing the variable x into the equilibrium expression. Answer: Step 4 Calculate the [H+]. Show the complete solution. Answer: Step 5. Calculate pH of the solution. Show the complete solution. Answer: HA(aq) 0.500 -X 0 +X
EXERCISE 1: Calculate the pH of a 0.50 M HA at 25°C. At 25°C, the acid dissociation constant (Ka) of the monoprotic weak acid, HA, is 7.2 x 10-6. Complete the ICE Table below: Dissociation Equation + HA(aq) H+ (aq) A (aq) INITIAL 0.500 0 Concentration CHANGE -X +X EQUILIBRIUM Concentration (6 pts) [HA] [H+] = [A-] = Write the equilibrium expression for the acid dissociation constant, K₂, and substitute the mathematical equation containing the variable x into the equilibrium expression. Then calculate the [H+] and pH of the solution. Show your complete solution. 0 +X
O ACIDS AND BASES Deriving Kp from K, Complete the table below. Round each of your entries to 2 significant digits. You may assume the temperature is 25 °C. conjugate acid conjugate base K. formula formula CH,NH, 4 4.4 x 10 NH, 5 1.8 x 10 HCN -10 4.9 x 10 Explanation Check 7077 McGraw Hill LIC AlL Rights Reserved. Terms of L
pH practice a.) determine the pH of a nitric acid solution (HNO3) that has been prepared by mixing 2.0 mL of 1.0 M HNO3 with 98.0 mL of water b.) determine the pH of a 25 mL carbonic acid solution (H2CO3) with a concentration of 5.7 x 10-5 M. assume all the protons will dissociate from the acid and react with water to form hydronium ions. c.) determine the pH and pOH of a NaOH solution that has been prepared by diluting 20.0 mL of 6.0 M NaOH with 80.0 mL of water. d.) determine the pH and pOH of a Ca(OH)2 solution that has been prepared by mixing 0.26 g of Ca(OH)2 pellets in 750 mL of water.
Exercise 6b. Arrange the solutions in order of increasing acidity: NaCl, NH4CI, KCN, NaOH, NaCH3COO, NaC3H5O3, Nicotine, C2H5NH3Cl HA and HB are both weak acids in water, and HA is a stronger acid than HB. Which of the following statements is correct? A) A is a stronger base than B, which is a stronger base than H₂O, which is a stronger base than Cl-. B) B is a stronger base than A, which is a stronger base than H₂O, which is a stronger base than Cl-. C) B is a stronger base than A, which is a stronger base than Cl, which is a stronger base than H₂O. D) CI is a stronger base than A, which is a stronger base than B, which is a stronger base than H₂O. E) None of these (A-D) is correct.
The beaker on the left below represents a buffer solution of a weak acid HA and its conjugate base, A. (Water molecules and spectator ions have been omitted for clarity.) a Which beaker on the right, X or Y, depicts the solution after the addition of two formula units of NaOH? b How many HCl molecules can be added to the original buffer solution before the buffer capacity is exceeded? c Draw a picture of the solution where the buffer capacity has been exceeded by the addition of HCl.
Exercise 2: A diprotic acid (H₂A) is titrated with NaOH to determine its molar mass according to the following equation: H₂A (aq) + 2 NaOH(aq) 2H₂O(1) + Na₂A (aq) Several experiments are performed by weighing a sample of H₂A, dissolve in water, with addition of few drops of phenolphthalein (ph.ph) indicator. The following data are obtained. Mass of H₂A Volume (mL) of 0.1M NaOH Molar mass of H₂A Average molar mass 46.5 55.5 0.22 0.28 0.30 0.32 0.25 0.28 Hint: mole H₂A=- Ul
Consider the following beakers. Each contains a solution of the hypothetical atom X. a Arrange the beakers in order of increasing concentration of X. b Without adding or removing X, what specific things could you do to make the concentrations of X equal in each beaker? (Hint: Think about dilutions.)
Exercise 1 Calculate the pH of each of the following solutions: (a) 0.63 M NaCH3CO2(aq), K, = 5.62 × 10-10, %3D (b) 0.19 M NH4CI(aq), K, = 5.6 × 10-10; %3D (c) 0.65 M KCN(aq), K½ = 2 × 10-5.
A 0.010 M solution of ammonia, NH3, has a pH of 10.6 at 25C. What is the concentration of hydroxide ion? (One way to solve this problem is to find the pOH first and then calculate the hydroxide-ion concentration.)

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General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning