A weak base has Kb=3.2×10−6. The compound has a solubility of 1.667gL, and the molar mass is 303.36gmol. What is the pH of a saturated solution of this compound? Use pKw=14.00 for the ion-product of water. Round your answer to two decimal places.

A weak base has Kb=3.2×10−6. The compound has a solubility of 1.667gL, and the molar mass is 303.36gmol. What is the pH of a saturated solution of this compound? Use pKw=14.00 for the ion-product of water. Round your answer to two decimal places.

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.25QE

See similar textbooks

Related questions

Q: weak monoprotic acid (HA) has an acid ionization constant Ka = 1.8x10° at 298 K. If 100 mL of a 0.10…

A: First write equilibrium equation for reaction of weak acid and strong base and fine limiting…

Q: What is the pH of a solution prepared by dissolving 1.00 g of the weak acid HA (molar mass = 138.95…

A: pH of solution can be found using the henderson-hesselbech equation.

Q: In the laboratory, a general chemistry student measured the pH of a 0.548 M aqueous solution of…

Q: A solution is prepared at 25 °C that is initially 0.35M in chloroacetic acid (HCH, CICO,), a weak…

Q: What is the pH of a 1.00x 10 molar solution of LICI? Report your answer with 2 places past the…

A: The acid-base nature of the salt solution depends on the nature of the acid and base from which the…

Q: Would you expect a solution of ammonium chloride (NH4Cl) to be acidic or basic when added to water?…

A: Introduction- For the salts of strong acids and strong bases, the pH of salt will be neutral that is…

Q: Solutions of NaClO2, KCH3COO, and Ca(NO2)2 all have pH that is greater than 7 at 25 oC. Using these…

A: The reaction between an acid molecule and a base molecule to form an ionic compound termed as salt…

Q: an aqueous solution containing 3 grams of CH3COOH in 500 ml of it and having a pH = 3 solution of…

A: Given that, pH of 500 mL solution containing 3 g CH3COOH = 3 Molarity of CH3COOH solution = (3…

Q: A 1.00 L solution contains benzoic acid (C7 H5 O₂ H) with a concentration of 0.250 mol/L,and sodium…

Q: What is the pH of a 0.350 M triethylamine, (C2H5)3N, solution? Kb for triethylamine is…

A: Given, 0.350 M triethylamine Kb for triethylamine is 5.3 *10-4

Q: What mass (in g) of potassium fluoride should be added to 0.50 Lof 0.255-M HF(aq) at 25 °C to give a…

Q: In the laboratory, a general chemistry student measured the pH of a 0.578 M aqueous solution of…

A: For a weak acid, we have pH = 1/2(pKa - logA) where A is the concentration of the acid. Given,…

Q: the laboratory, a general chemistry student measured the pH of a 0.428 M aqueous solution of…

A: PH is defined as the power of Hydrogen.it measure acidity, basicity or neutrality of aqueous…

Q: Write the Henderson-Hasselbalch equation for a propanoic acid solution (CH;CH,CO,H, pKa=4.874) using…

A: In general equation, pH=pKa+log10([A-])/[HA] The equation for propanoic acid…

Q: What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M methylamine. CH3NH2. with 25.00…

A: Given : Concentration of methamine i.e CH3NH2 = 0.10 M Volume of CH3NH2 solution = 25.00 mL = 0.025…

Q: A solution is prepared at 25°C that is initially 0.48M in dimethylamine CH32NH, a weak base with…

A: An acidic substance is the substance that can give H+ ions. They are corrosive and sour in nature.…

Q: What is the pH of a 0.25 M solution of sodium propionate, NaC3H5O2, at 25°C? (For propionic acid,…

Q: Calculate the pH of a 0.594 M aqueous solution of pyridinium chloride, C5H5NHCl. The Kb of pyridine…

Q: A student mixes 300 mL of 0.100 M NaOH with 100 mL of 0.300 M H,SO4. The resulting solution has a pH…

A: Given: The Volume of NaOH, (V1) = 300 mL The Volume of H2SO4, (V2) = 1 00 mL. The molarity of NaOH,…

Q: In the laboratory, a general chemistry student measured the pH of a 0.354 M aqueous solution of…

A: Given that: pH = 0.354 [C8H10N4O2] = 12.063 To find: Kb

Q: Calculate the pH of a 0.100 M KCN solution.

Q: How many milliliters of 0.800 M KOH should be added to 3.38 g of oxalic acid (C2O4H2) to give a pH…

A: Reaction: H2Ox + OH- —->HOx- + H2OHOx- + OH- ——->Ox- + H2O Equilibrium: H2Ox ——>HOx- + H…

Q: The acid dissociation constant K, of boric acid (H,BO,) is 5.8 x 10. Calculate the pH of a 3.2M…

A: PH of weak acid can be calculated by using the relation. PH = 1/2 [ PKa - logC].

Q: 1. Write a chemical equation for the dissociation of the hypochlorite ion, ClO-1, in water to make a…

A: Hello. Since the question contains multiple parts, the first part is solved. In case the solution…

Q: NH3 is a weak base (Kb=1.8×10−5Kb=1.8×10−5) and so the salt NH4Cl acts as a weak acid. What is the…

Q: In the laboratory, a general chemistry student measured the pH of a 0.400 M aqueous solution of…

A: To find Kb for base, first write reaction of base with water and according to that, find [OH-] or…

Q: In the laboratory, a general chemistry student measured the pH of a 0.552 M aqueous solution of…

Q: Which of the following 1.25M aqueous solution will have the lowest pH? (Qualitative analysis only,…

A: Concentration = 1.25 M ->Base has pH greater than 7. ->Acids has pH less than 7. ->Neutral…

Q: What is the pH of the solution that is prepared by dissolving 0.8 g of lactic acid (90.08 g/mol, Ka…

A: We have given that What is the pH of the solution that is prepared by dissolving 0.8 g of lactic…

Q: What is the pH of a solution prepared by adding 60.4 g ethylammonium chloride (C2H5NH3CI, 81.55…

A: As C2H5NH3Cl is salt of weak base and strong acid while C2H5NH2 is weak base so the resultant…

Q: Calculate the pH of a 2.0 x 10–3 M solution of pyridine (C5H5N). Kb = 1.7 x 10–9

A: The Bronsted-Lowry acid-base theory was purposed by Bronsted and Lowery is called Bronsted-Lowry…

Q: The substance benzoic acid (C6H5COOH) is a weak acid (Ka = 6.3×10-5).What is the pH of a 0.258 M…

A: 1) Given: Concentration of C6H5COOK = 0.258 M The hydrolysis reaction of C6H5COO- coming from…

Q: The acid dissociation constant K, of carbonic acid (H,CO,) is 4.5 x 10. Calculate the pH of a 4.0M…

Q: LA solution is prepared at 25 °C that is initially 0.083 M in chloroacetic acid (HCH,CICO,), a weak…

Q: Methyl Amine (CH3NH2) is a weak base with a Kb of 4.38 x 10-4. What would be the pH of a solution of…

A: The above salt is a mixture of weak base and strong acid. When it dissolves in water it forms an…

Q: Calculate the pH for a 0.1 M solution of C6H5COOH (K, = 6.46 x 105) and the pH for a 0.2 M %3D…

Q: In the laboratory, a general chemistry student measured the pH of a 0.441 M aqueous solution of…

Q: NH3 is a weak base (?b=1.8×10−5Kb=1.8×10−5) and so the salt NH4Cl acts as a weak acid. What is the…

Q: A solution is prepared at 25 °C that is initially 0.37M in chloroacetic acid (HCH, CICO,), a weak…

A: In the above-given problem, a mixture of a weak base and its salt is taken. Now, the salt of the…

Q: In the laboratory, a general chemistry student measured the pH of a 0.423 M aqueous solution of…

A: The value of Kb for the given weak base is = 7.3x10-6 The concentration of the base solution is =…

Q: The acid dissociation constant K, of hypobromous acid (HB1O) is 2.3 x 10. Calculate the pH of a 1.8…

Q: Sodium ascorbate is the sodium salt of ascorbic acid (i.e. Vitamin C) and is used as an antioxidant…

A: We have to predict the pH of 0.15 M solution for ascorbate ion.

Q: find the pH of a 0.30M solution of sodium benzoate ,NaC7H5O2.Kb for the benzoate ion C7H5O2 is 1.55…

A: The expression for the pH of a salt solution of weak base and strong acid is given as:

Q: In the laboratory, a general chemistry student measured the pH of a 0.377 M aqueous solution of…

Q: Calculate the pH of an aqueous KOH solution that is made by dissolving 654 mg of solid KOH in enough…

Q: A solution is prepared at 25°C that is initially 0.41M in benzoic acid HC6H5CO2, a weak acid with…

A: The solution is as follows :

Q: A solution is prepared at 25 °C that is initially 0.30 M in benzoic acid (HC,H,Co,), a weak acid…

A: Step 1: The given solution is a buffer of weak acid and its conjugate base. So, the Handerson…

Q: Calculating the pH of a dilute acid solution The acid dissociation K, of benzoic acid (C,H,CO,H) is…

A: pH = -log(H+)

Q: What is the pH of a solution prepared by mixing 30.00 mL of 0.10 M CH3CO2H with. 30.00 mL of 0.030M…

Q: Calculate the pH of a 0.400 M CH3NH3Cl solution. Kb for methylamine, CH3NH2, is 4.4 × 10-4.

Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

A weak base has Kb=3.2×10−6. The compound has a solubility of 1.667gL, and the molar mass is 303.36gmol. What is the pH of a saturated solution of this compound?

Use pKw=14.00 for the ion-product of water.
Round your answer to two decimal places.

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

Trending now

This is a popular solution!

Step by step

Solved in 4 steps with 4 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

find the pH of a 0.30M solution of sodium benzoate ,NaC7H5O2.Kb for the benzoate ion C7H5O2 is 1.55 x 10^-10
What is the pH of a solution prepared by combining 0.696 mol of a weak acid (Ka = 5.5 x 10-5) with 0.516 mol of the salt containing its conjugate base in 3.4 L of water? Report your answer to the hundredths place and do not include units.
What is the pH of a solution prepared by combining 0.258 mol of a newly discovered weak acid (Ka = 1.3 x 10-4) with 0.156 mol of the salt containing its conjugate base in 1.4 L of water?
Please don't provide handwritten solution... In the laboratory, a general chemistry student measured the pH of a 0.513 M aqueous solution of triethanolamine, C6H15O3N to be 10.721. Use the information she obtained to determine the Kb for this base.
The Ka of formic acid (HCO2H) is 1.8x10-4. What would the pH of a solution containing equal concentrations of formic acid and sodium formate be? Use the H-H equation for buffers to solve this. This is true in general for solutions where the acid and conjugate base are present in equal concentrations.
What is the pH of a solution prepared by mixing 30.00 mL of 0.10 M CH3CO2H with. 30.00 mL of 0.030M CH3CO2K? Assume that the volume of the solutions are additive and that Ka= 1.8x10^-5 for CH3CO2H
A solution is prepared at 25°C that is initially 0.41M in chloroacetic acid (HCH2ClCO2) , a weak acid with Ka= 1.3 x 10^−3, and 0.081M in potassium chloroacetate (KCH2ClCO2). Calculate the pH of the solution. Round your answer to 2 decimal places.
NH3 is a weak base (Kb=1.8×10−5Kb=1.8×10−5) and so the salt NH4Cl acts as a weak acid. What is the pH of a solution that is 0.0870.087 M in NH4Cl at 25 °C? pH=
Bacteria in the human mouth release enzymes to break up sucrose, and thenpolymerize glucose to form a bacterial plaque. When this glucose is digested, it formslactic acid, which causes tooth decay. Tooth enamel is made of calcium phosphate.Lactic acid has a Ka 1.38x10 -4 and ionizes into lactate and H3O+ ions. Assuming aninitial lactic acid concentration of 0.10 mol/L on your tooth, determine the pH(assume a 1:1:1 mole ratio) and the percent ionization. Should people be concernedwith plaque buildup? Justify your answer.
Calculate the pH of the following solutions: a) 2.0M morphine hydrochloride, C17H19NO3*HCl (pKb = 6.13) b) 0.50M AlCl3 (Ka of [Al(H2O)6] is 1.4 x 10^-5
Calculate the pH of the mixture of 94 mL butanoic acid (CH3CH2CH2COOH) 0.189 mol/L with 109 mL sodium butanoate (CH3CH2CH2COONa) 0.207 mol/L.Give an answer with at least 3 decimal places.
Using chemical equations, show how the triprotic acid H3PO4 ionizes in water. Phases are optional. Kal: ???? Ka2: ???? Ka3: ????