Answered: Calculate the pH for a 10.0 M solution…

Science

Chemistry

Calculate the pH for a 10.0 M solution of NH3 (kp= 1.8x105) NH3 - NH4 + OH a 13.987 O b .013 O c 1.87 O d 12.13

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.71PAE: Acrylic acid is used in the polymer industry in the production of acrylates. Its K, is 5.6 X 10“’....

See similar textbooks

Related questions

Q: (g) What is the pH of a 0.023 M solution of HCN (K- = 4.9 x 10-10)? 1.64 10.95 • 3.05 • 5.47 4.97

Q: 1. Give the equation for the dissociation of dimethylamine, (CH3)2NH, in water. b. Write the Kb…

Q: What is the pH of a 0.0380 M solution of HONH CI (Kb of HONH₂ is 1.1 x 10°)?

A: The pH of any acidic mixture is always low.

Q: To answer this question, you may need access to the periodic table of elements, a calculator, and…

A: Here we have to calculate pOH of a 0.000259 M HClO4 solution at 25° C.

Q: What is the pH of a 0.030 M solution of KF? Ka of HF is 7.2 x 10-4 6.19 3.16 7.81 7.60 4.67

A: The given salt is KF that is composed of KOH (strong base) and HF (weak acid). It is a basic salt.…

Q: What is the % ionization of a solution of 0.20 M benzoic acid, C,H,COOH (K¸ = 6.6 x 10 ')? Would a…

Q: What is the pH of a 0.430 M solution of CH NHBr (Kb of CHN is 1.7 × 10º)?

A: Given information:Calculate pH. .pH is the measurement of acidity or alkalinity of solution. A…

Q: Determine the pH of a 0.188M NH3 solution. The Kp of NH3 is 1.76 x 105 12.656 8.520 2.740 11.260…

A: Given: Kb = 1.76 X 10-5 [NH3] = 0.188M

Q: The pH of 0.075 M NH3 solution (Kb for NH3 = 1.75 x 10-5) %3D O 4.94 O 2.09 11.05 O 12.03 8.02

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

Q: 8. Calculate the equilibrium concentration of each aqueous species (H2A, HA– A2–, H3O+, and OH–) in…

Q: 6. What are the equilibrium concentrations of a 0.80 M HCN solution for each species (in M to two…

A: we have to calculate the equilibrium concentration of all species for the HCN solution

Q: CH3NH, is a weak base with K, = 4.0 x 104. What is the pH of a 1.0 M solution of CH3NH;CI? O 5.3 O…

A: Here salt is a combination of weak base and strong acid so we can determine pH by applying…

Q: A solution of CgH5N (pyridine, Kp = 1.7 x 10) has a pH of 9.40. What is the [C;H5N]? O 0.37 9.3 x 10…

Q: The pH of an aqueous solution of weak monoprotic acid is 3.15. What is the initial concentration of…

A: Given: The pH of weak mono-protic acid=3.15 pKa of the acid=5.74

Q: Saccharin, a sugar substitute, is a weak acid with the formula, HC7H4NSO3. The pKa of saccharin is…

Q: The ionization constant for NH4+ is K = 5.8 x 10-10 at 25°C. It is in a reversible equilibrium with…

A: K=5.8×10-10 T= 25°C k1=4.000×1010 M-1s-1 NH4Cl = 0.1 M

Q: 2. What is the pH of a 0.01 M HNO3 solution? What is the ratio of acid to conjugate base for this…

A: (1) The dissociation of the given acid can be given as: The concentration of the acid is 0.01 M.…

Q: 4. The equilibrium constant values for a number of reactions are listed below. Indicate whether the…

Q: If the K of a weak base is 8.0 × 10-6, what is the pH of a 0.48 M solution of this base? pH

A: Weak base dissociated less in aqueous solutions

Q: A 0.00653 M solution of an unknown weak acid has a pH of 3.510 at 25 °C, what is the K acid at 25…

Q: Calculate the pH of a 0.20 M solution of NH4NO3. (Kb(NH3) = 1.8 x 10)

A: Salt of Weak base and Strong acid pH = 7 - 1/2 ( pKb - logC )

Q: What is the pH of a 0.652 M solution of hydroxylammonium, a weak acid with a K, of 1.1 x 10-6? Oa.…

A: Given, Concentration of hydroxylammonium [NH3OH]+, (c) = 0.652M acid dissociation constant of a weak…

Q: In the laboratory a student measures the percent ionization of a 0.532 M solution of acetylsalicylic…

A: Ionisation of acetyl salicylic acid in water is as shown below: The expression for acid…

Q: NH3 is a weak base (K, = 1.8 × 10-') and so the salt NH4CI acts as a weak acid. What is the pH of a…

A: Given, Concentration of NH4Cl solution = 0.075 M Kb for NH3 = 1.8 × 10-5 pH of the solution = ?…

Q: Which direction does the equilibrium below favor and what is the deciding factor? H+ cat. H20 ОН HO

Q: What is [OH-] in a solution of 1.25 M NH3 and 0.85 M NHANO3? NH3 (aq) + H20 (1) = NH4+ (aq) + OH-…

A: Henderson equation is used to calculate the pH (and pOH) of the buffer. pH = pKa + log[base]/[acid]…

Q: A 0.0320 M solution of a weak base has a pH of 9.45. Determine the Kp of this weak base.

Q: 4. Lactic acid C3H603 is found in sour milk where it is produced by the action of lactobacilli in…

A: In this case, we need to write the overall reaction: HC₃H₅O₃ + H₂O <-------> C₃H₅O₃⁻ + H₃O⁺…

Q: 9. A base is added to water and a new equilibrium is established. The new equilibriu described by A.…

A: In the pure water pH and POH both are same

Q: A 0.121 M solution of acetic acid has a pOH of 11.20. What is the K3 of acetic acid? Oa. 2.5 x 106…

A: Given: The concentration of acetic acid is 0.121 M The value of pOH is 11.20

Q: The pH of a solution containing a hydrogen ion concentration of 1 x 10-5 is: A. 3 and its pOH is 6…

Q: Heroin, a derivative of morphine, is a powerful analgesic and a powerful narcotic agent. Calculate K…

Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

Calculate the pH for a 10.0 M solution of NH3 (kp= 1.8x105)
NH3 - NH4 + OH
a
13.987
O b
.013
O c
1.87
O d
12.13

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

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 2 images

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

What are the equilibrium concentrations of acetic acid, the acetate ion, and H3O+ for a 0.10 M solution of acetic acid (K2 = 1.8 105)? What is the pH of the solution?
Consider a 0.60-M solution of HC3H5O3, lactic acid (Ka = 1.4 104). a. Which of the following are major species in the solution? i. HC3H5O3 ii. C3H5O3 iii. H+ iv. H2O v. OH b. Complete the following ICE table in terms of x, the amount (mol/L) of lactic acid that dissociates to reach equilibrium. c. What is the equilibrium concentration for C3H3O3? d. Calculate the pH of the solution.
Most naturally occurring acids are weak acids. Lactic acid is one example. CH3CH(OH)CO2H(s)+H2O(l)H3O+(aq)+CH3CH(OH)CO2(aq) If you place some lactic acid in water, it will ionize to a small extent, and an equilibrium will be established. Suggest some experiments to prow that this is a weak acid and that the establishment of equilibrium is a reversible process.
Ka for acetic acid at 25.0C is 1754 105. At 55.0C, Ka is 1.625 105. What are H and S for the ionization of acetic acid?
The hydrogen phthalate ion, C8HsO4, is a weak acid with Ka = 3.91 106. C8H5O4(aq)+H2O(l)C8H4O42(aq)+H3O+(aq) What is the pH of a 0.050 M solution of potassium hydrogen phthalate. KC8H5O4? Note: To find the pH for a solution of the anion, we must take into account that the ion is amphiprotic. It can be shown that, for most cases of amphiprotic ions, the H3O+ concentration is [H3O+]=Ka1Ka2 For phthalic acid, C8H6O4 is Ka1 is 1.12 103, and Ka2 is 3.91 106.
Hydrazine, N2H4, can interact with water in two steps. N2H4(aq) + H2O() N2H5+(aq) + OH(aq) Kb1 = 8.5 107 N2H5+(aq) + H2O() N2H62+(aq) + OH(aq) Kb2 = 8.9 1016 (a) What is the concentration of OH, N2H5+ and N2H62+ in a 0.010M aqueous solution of hydrazine? (b) What is the pH of the 0.010M solution hydrazine?
Calculate the CO2+ equilibrium concentration when 0.100 mole of [CO(NH3)6](NO3)2 is added to a solution with 0.025 M NH3. Assume the volume is 1.00 L.
Consider the following statements. Write out an example reaction and K expression that is associated with each statement. a. The autoionization of water. b. An acid reacts with water to produce the conjugate base of the acid and the hydronium ion. c. A base reacts with water to produce the conjugate acid of the base and the hydroxide ion.
The dissociation of acetic acid, CH3COOH, has an equilibrium constant at 25 degrees celsius of 1.8 x 10-5. CH3COOH(aq) ⇋ CH3COO-(aq) + H+(aq) If the equilibrium concentration of CH3COOH is 0.46 moles in 0.500 L of water and that of CH3COO is 8.1 x 10-3 moles in the same 0.500 L, calculate the concentration of H + for the reaction.
What is the equilibrium concentration of chloroacetic acid, HC₂H₂O₂Cl, in a solution prepared by dissolving 0.0271 mol of HC₂H₂O₂Cl in 1.50 L of water? For chloroacetic a Ka=1.4 x 10³. O 9.03 x 103 M O 1.37 x 10-2 M O 4.38 x 103 M 5.03 x 10-³ M O 1.81 x 10-2 M
A student determine the k a of an acid to be 5.8722 x 10 -4. What is the pK a? 4.0532 1.0014 3.2312 4.9060 4.4782
Heroin, a derivative of morphine, is a powerful analgesic and a powerful narcotic agent. Calculate K for heroin if the pH of a 1.7 x 10 M solution was found to be 9.60. O 2.3 x 102 O9.5 x 10-7 O 3.7 x 10-7 1.5 x 10-7 9.3 x 10-7