pH

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter21: Chemistry Of The Nonmetals

Section: Chapter Questions

Problem 43QAP

See similar textbooks

Related questions

Q: 3. A 0.0560 g quantity of acetic acid is dissolved in enough water to make 50.0 mL of solution.…

A: (a) Initial Concentration of CH3COOH Given mass of acetic acid = 0.056 gms, Volume of…

Q: The CO2 we breathe reacts with water in our blood to form the weak acid H2CO3. What mole ratio of…

A: Given:Ka of H2CO3 is 4.4 ✕ 10−8

Q: (a) Give the conjugate base of the following Brønsted–Lowry acids: (i) HIO3, (ii) NH4+. (b) Give the…

A: Conjugate base : the conjugate base is able to gain a proton in a chemical reactio Conjugate…

Q: If the Kb for hydrazine, N2H4(aq), is 1.7 x 10-6 , calculate the pH of a 1.8 mol/L solution of…

A: To calculate the pH of a 1.8 mol/L solution of hydrazine. Given: Kb for hydrazine, N2H4(aq) = 1.7 x…

Q: CoHsOH(ag) + H2O0 → CaHsO(aq) + H3O*@g K= 1.12 x 1010 (a) Phenol is a weak acid that partially…

A: Since you have asked a question with multiple parts, we are solving first three parts for you. For…

Q: The pH of an aqueous solution of 0.291 M ammonium perchlorate, NH4ClO4 (aq), is This solution is -5…

A: Concentration of NH4ClO4 = 0.291 MKb of NH3 = 1.80×10-5

Q: Propionic acid, HC3H5O2, has Ka= 1.34 x 10–5. (a) What is the molar concentration of H3O+ in 0.15 M…

A: HC3H5O2 is a weak acid and dissociates in aqueous solution as: HC3H5O2+H2O↔C3H5O2-+H3O+

Q: The pH of an aqueous solution of 0.532 M hydrofluoric acid, ( K₂ (HF) = 7.20 × 10¯4) is

A: Concentration of HF solution (C) = 0.532 MKa for HF = 7.20 × 10-4 pH of the solution = ?

Q: The compound methylamine is a weak base like ammonia. A solution contains 0.199 M CH3NH3* and 0.117…

A: TThe base is the substance that gives OH- or accepts H+ ions in solution. The Henderson Hasselbalch…

Q: 8. (a) HA(aq) is a weak acid with a dissociation constant, Ka, of 8.8 x 10−12. What is the pH of a…

Q: Determine the pH of each of the following solutions. (a) 0.684 M hypochlorous acid (weak acid…

Q: Ammonia, NH3, is amphoteric. (a) Give the formula for the conjugate acid of NH3. (b) Give the…

A: Write conjugate acid and conjugate base of NH3 ---

Q: The molarity of an aqueous solution of NaOH is 0.0022 M. (a) What is the concentration of H3O+ in…

Q: 6. Acids and bases are defined by their donation or acceptance of a proton according to the (a)…

A: The correct answer is explained below

Q: The base protonation constant K, of allantoin (C,H,N,O,NH,) is 9.12 x 10 °. Calculate the pH of a…

A: Given Initial Concentration = 0.47 M Kb = 9.12 × 10-6

Q: Determine the pH of 0.082 M ammonia, NH3 (aq) and percent ionization of base.

A: The pH of the solution is calculated to be approximately pH=11.08.The percent ionization is…

Q: Hypochlorous acid, HOCl, is a weak acid having a pKa = 7.46. (a) Show the balanced chemical equation…

A: Given that : For HOCl, pKa = 7.46 We need to find pKb and pH of solution when [OCl-] = 0.050 M

Q: What is the conjugate base of boric acid, B(OH)3? (A) OH– (B) B(OH)4–…

A: According to Bronsted concept , acid is a substance which donates proton and base is the substance…

Q: Determine the pH of each of the following solutions (Ka and Kb values can be found in the appendices…

A: (a) 0.045M hypochlorous acid pKa value = 7.53 Now, pH = (1/2)(pKa - log[HOCl] =…

Q: The value of K₂ for nitrous acid is 4.50×10-4. What is the value of Ko, for its conjugate base, NO₂?…

A: Since you posted multiple type question, then according to the guideline, post first solution for…

Q: Which of the following species can be Brønsted–Lowry bases: (a) Al(OH) 3; (b) Br −; (c) NH 4+; (d)…

A: According to Brønsted–Lowry theory, a chemical species is Brønsted–Lowry base if it accepts a proton…

Q: Predict whether aqueous solutions of the following substances are acidic, basic, or neutral and…

Q: Which one of the following pairs of acids and conjugate bases is incorrectly labeled or incorrectly…

A: A conjugate base is simply the substance that contains one less H atom and one more negative charge…

Q: The pH of an aqueous solution of 0.400 M hydrocyanic acid, (K₁ (HCN) = 4.00 x 10-¹0) is

A: Given,Molarity of HCN = 0.400 MKa ( HCN ) = 4.00 x 10-10

Q: f) Calculate the pH of the following solutions: (i) A 0.045 M solution of sulphuric acid. (ii) A…

Q: Write the formula for the conjugate base of each of the following acids: (a) CH,CICOOH, (b) HIO4,…

Q: The ionization constant, Ka, for dichloroacetic acid, HC2HO2Cl2 , is 5.0 × 10‑2. What is the pH of…

A: The ionisation reaction for the dichloroacetic acid will be HC2HO2Cl2 ------> H+ + C2HO2Cl2-…

Q: Lactic acid, HC3H5O3, is a weak acid; write an equation for its ionization in aqueous solution. If…

A: given Lactic acid, using PH calculate the value of H+ , apply the H+=Cα using the alpha value…

Q: Determine the pH of a 0.15 M solution of Ca(BrO2)2 at 25 °C. At the same temperature, Ka for HBRO, =…

Q: The active ingredient of bleach such as Clorox is sodium hypochlorite (NaClO). Its conjugate acid,…

A: Given:The word pH stands for the potency of hydrogen and it is used to measure the concentration of…

Q: In the following reactions, identify the Lewis acid and the Lewis base. (a) AlCl3 + Cl¯ → AICI, (b)…

A: A Lewis acid is a chemical species that contains an empty orbital which is capable of accepting an…

Q: (b) Hydrazine, N2H4, is a Brønsted-Lowry base used as a rocket fuel. Write the formula for the…

A: According to the Bronsted Lowry concept, acids are those Substances which can produce Hydrogen ions…

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

4.)Calculate the pH of a 0.300 M solution of ammonium sulfate, (NH₄)₂SO₄. You may assume that the sulfate ion, SO₄^-2, is negligibly basic.

Expert Solution

This question has been solved!

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

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

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

The active ingredient of bleach such as Clorox is sodium hypochlorite (NaClO). Its conjugate acid, hypochlorous acid (HClO), has a Ka of 3.0 × 10–8. (a)The undiluted bleach contains roughly 1 M NaClO. Calculate the pH of 1 M NaClO solution. (b)Some applications require extremely diluted bleach solution, such as swimming pools. Suppose the solution in (a) is diluted by 10,000 -fold. Calculate the pH of the diluted solution, and demonstrate that you can still neglect the autoionization of water in your calculation. (c)Suppose the solution in (a) is diluted by 1million-fold, briefly explain how your approach will be different. Write the equation with [H3O+] as the unknown, but you do not need to solve it.
Ammonia, NH3, is amphoteric. (a) Give the formula for the conjugate acid of NH3. (b) Give the formula for the conjugate base of NH3.
Why is (CH3)3Cl considered to be a Lewis Acid?
If the Kb for hydrazine, N2H4(aq), is 1.7 x 10-6 , calculate the pH of a 1.8 mol/L solution of hydrazine.
The value of K₂ for nitrous acid is 4.50×10-4. What is the value of K₁, for its conjugate base, NO₂? ||
The CO2 we breathe reacts with water in our blood to form the weak acid H2CO3. What mole ratio of H2CO3/HCO3− is required to obtain a pH of 7.40, the pH of blood? (Assume that the Ka of H2CO3 is 4.4 ✕ 10−8.)
Calculate the pH of a 0.597 M solution of chloroacetic acid (CICH;CO,H, K, = 1.36 x 10³).
(f) Calculate the pH of the following solutions: (i) A 0.045 M solution of sulphuric acid. (ii) A solution containing 0.4 g sodium hydroxide in 100 cm³ water. (iii) Given the Ka value for CH3COOH is 1.8 x 10-5, calculate the pH of the acid. The initial concentration of the acid is 0.2 M
Determine the pH of each of the following solutions (Ka and Kb values can be found in the appendices of your textbook or online): (a) 0.045 M hypochlorous acid; (b) 0.0068 M phenol; (c) 0.080 M hydroxylamine.
6. Acids and bases are defined by their donation or acceptance of a proton according to the (a) Arrhenius model. (b) Bronsted-Lowry model. (c) Lewis model.
5. The molarity of an aqueous solution of NaOH is 0.0022 M.(a) What is the concentration of H3O+ in this solution?(b) What is the pH of the solution?(c) What is the OH- concentration in the solution?
The acid ionization constant for Pb(H2O)62+(aq) is 6.3×107. Calculate the pH of a 0.0651 M solution of Pb(NO3)2. pH =