A chemist dissolves 172. mg of pure barium hydroxide in enough water to make up 120. mL of solution. Calculate the pH of the solution. (The temperature of the solution is 25 °C.) Be sure your answer has the correct number of significant digits.

A chemist dissolves 172. mg of pure barium hydroxide in enough water to make up 120. mL of solution. Calculate the pH of the solution. (The temperature of the solution is 25 °C.) Be sure your answer has the correct number of significant digits.

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter21: The Chemistry Of The Main Group Elements

Section: Chapter Questions

Problem 78PS

See similar textbooks

Related questions

Q: A certain weak acid found in Ketchup has a K, of 3.56 x 106. Calculate the pH of an aqueous solution…

Q: Calculate the pH of a 0.84 M HONH2 solution. Give your answer to three sig figs. Kb(HONH2) = 1.0 x…

A: Given: The concentration of HONH2 solution = 0.84 M Kb(HONH2) = 1.0 x 10‒5 To Calculate: pH of the…

Q: A chemist dissolves 451. mg of pure sodium hydroxide in enough water to make up 100. ml. of…

Q: Calculate the pH of a 0.01 M solution of hydroxyl amine (K, = 1.1 x 10*).

Q: 1. S)A student prepares a solution of 23.25 g of acetic acid dissolved in enough water to make 2.00…

A: Given, CH3COOH (aq) + H2O (l) ⇌ H3O+ (aq) + CH3COO-(aq) mass of acetic acid = 23.25 g Volume of the…

Q: What is the pH of the following solutions? Identify each as acidic, basic, or neutral. a. 0.010 M…

A: If pH is greater than 7 it is basic. If pH is less than 7 it is acidic

Q: acid base K. K, name formula name formula ethylamine C2H5NH, 6.4× 10 hydrofluoric acid HF 6.8 × 10¬4…

A: Using concept of acid base neutralization to determine the pH of Salt.

Q: Calculate the pH of a solution that has a hydroxide ion concentration, [OH−], of 1.35×10−8 M.

Q: A chemist dissolves 715. mg of pure potassium hydroxide in enough water to make up 80. mL of…

Q: A chemist dissolves 843. mg of pure potassium hydroxide in enough water to make up 80. mL of…

A: Mass of KOH = 843 mg1mg = 10-3 gMass of KOH = m = 0.843 gMolar mass of KOH = 56.1 g/mol = MMoles of…

Q: A chemist dissolves 455. mg of pure barium hydroxide in enough water to make up 90. mL of solution.…

A: pH = 14 - pOH Since the reaction taking place is Ba(OH)2 ----> Ba2+ + 2OH- And since barium…

Q: A chemist dissolves 132. mg of pure hydrochloric acid in enough water to make up 60. mL of solution.…

Q: A chemist dissolves 724.mg of pure potassium hydroxide in enough water to make up 170.mL of…

A: potassium hydroxide will release hydroxide ions in the solution.

Q: The pH of a solution is 2.45. What is the molar concentration of hydronium ions in the solution?…

A: We have given that pH = 2.45 [H3O+] = ?

Q: A chemist dissolves 52. mg of pure barium hydroxide in enough water to make up 110. mL of solution.…

A: Answer:- This question is answered by using the simple concept of calculation of pH using the…

Q: A chemist dissolves 164. mg of pure nitric acid in enough water to make up 120. mL of solution.…

Q: A chemist dissolves 283. mg of pure barium hydroxide in enough water to make up 150. mL of solution.…

A: Given: mass of Ba(OH)2=283 mg=0.283 g volume of solution=150 mL

Q: A newspaper reported that the level of acidity in a sample taken from an extensively studied…

Q: 画 A chemist dissolves 178. mg of pure barium hydroxide in enough water to make up 160. mL of…

Q: A chemist dissolves 622. mg of pure barium hydroxide in enough water to make up 180. mL of solution.…

Q: A chemist dissolves 369. mg of pure barium hydroxide in enough water to make up 60. mL of solution.…

A: Given: mass of Ba(OH)2=369 mg =0.369 gvolume of solution=60 mL To…

Q: A chemist dissolves 705. mg of pure perchloric acid in enough water to make up 160. mL of solution.…

A: Given information, Mass of pure perchloric acid = 705. mg = 0.705 g As ( 1g = 1000 mg ) Volume of…

Q: A chemist dissolves 447. mg of pure barium hydroxide in enough water to make up 100. mL of solution.…

A: Since molecular mass of Ba(OH)2 = 171 gm/mol Hence moles of Ba(OH)2 = 0.447 / 171 = 2.614 X 10-3…

Q: A newspaper reported that the level of acidity in a sample taken from an extensively studied…

A: Any solutions's characteristics whether it is alkaline or else acidic is defined by its pH value.…

Q: A chemist dissolves 592. mg of pure barium hydroxide in enough water to make up 160. mL of solution.…

A: At 25 oC, the solubility of barium hydroxide, Ba(OH)2 is approximately 4.70 g / 100 mL water. Since…

Q: Acetic acid (CH3COOH, ?a=1.80×10−5) is a weak acid, so the salt sodium acetate (CH3COONa) acts as a…

Q: A chemist dissolves 325. mg of pure potassium hydroxide in enough water to make up 50. mL of…

Q: A chemist dissolves 515. mg of pure barium hydroxide in enough water to make up 180. mL of solution.…

Q: Tartaric acid is found in many fruits, including grapes, and is partially responsible for the dry…

A: The first dissociation constant gives a major contribution to the calculation of the pH of tartaric…

Q: A chemist dissolves 465. mg of pure potassium hydroxide in enough water to make up 90. mL of…

A: Mass of KOH in g = 465 / 1000 = 0.465 g Volume of solution in L = 90/1000 = 0.090 L Moles of KOH =…

Q: What is the pH of a solution that has an H concentration of 2.6 x 10 M? Enter your answer to the…

A: 4) Given, Concentration of the H+ ion = [H+] = 2.6 × 10-8 M pH of the solution = ? The formula used…

Q: A chemist dissolves 849.mg of pure barium hydroxide in enough water to make up 60.mL of solution.…

A: Given,

Q: A chemist dissolves 601. mg of pure barium hydroxide in enough water to make up 190. mL of solution.…

Q: A chemist dissolves 378. mg of pure barium hydroxide in enough water to make up 170. mL of solution.…

A: The pH is used to determine the acidity or alkalinity of a solution. Molarity is used to define the…

Q: A chemist dissolves 722. mg of pure potassium hydroxide in enough water to make up 140. mL of…

Q: For solutions with the following pH values, determine the concentration of hydrogen ion (or…

Q: A chemist dissolves 646. mg of pure barium hydroxide in enough water to make up 60. mL of solution.…

Q: A chemist dissolves 365. mg of pure perchloric acid in enough water to make up 280. mL of solution.…

A: pH = - log [H+] If the acid is a strong acid, it dissociates completely in solution. In such case,…

Q: A teacher pipettes 5.0

A: M1V1 = M2 V2 Where M1 = initial Molarity= 1.5 M V1 = initial volume = 5 mL M2 = final Molarity…

Q: A chemist dissolves 152. mg of pure potassium hydroxide in enough water to make up 100. mL of…

A: Given : Mass of KOH = 152.mg Volume of solution = 100.mL To calculate : pH of solution at 25°C

Q: A chemist dissolves 649. mg of pure barium hydroxide in enough water to make up 90. mL of solution.…

A: Given, mass of barium hydroxide, Ba(OH)2 = 649. mg = 0.649 g Volume of the solution = 90. mL = 0.09…

Q: A chemist dissolves 715. mg of pure sodium hydroxide in enough water to make up 110. mL of solution.…

A: To calculate the pH of the given sodium hydroxide solution, first of all, we calculate the molar…

Q: A chemist dissolves 190. mg of pure nitric acid in enough water to make up 190. mL of solution.…

A: Given : mass of nitric acid i.e HNO3 = 190 mg = 0.190 g…

Q: A chemist dissolves 635. mg of pure potassium hydroxide in enough water to make up 80. mL of…

Q: The acidic ingredient in vinegar is acetic acid. The pH of vinegar is around 2.4, and the molar…

A: Ionization of acetic acid(CH3COOH): CH3COOH(aq) ⇌…

Q: Calculating the pH of a strong base solution A chemist dissolves 388. mg of pure potassium hydroxide…

A: Given, The mass of potassium hydroxide = 388. mg Volume of solution = 60. mL The pH of the…

Q: A 1.5 x 103 M aqueous sulfuric acid (H2SO4) solution is prepared in the general chemistry lab. What…

A: Given information: Concentration of sulfuric acid = 1.5×10-3 M

Q: A chemist dissolves 552. mg of pure barium hydroxide in enough water to make up 190. mL of solution.…

A: We have given that A chemist dissolve 552mg of pure barium hydroxide in enough water to make 190mL…

Q: The pH of an aqueous solution of pyridine (C5H5N) is 10.0 at room temperature. What is the initial…

A: Weak acid or base are those substance which does not dissociate 100%. The value of degree of…

Q: Explain how a set of weak bases, all with approximately the same 0.1 molarity, can have different pH…

A: Answer

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

A chemist dissolves 172. mg of pure barium hydroxide in enough water to make up 120. mL of solution. Calculate the pH of the solution. (The temperature of
the solution is 25 °C.)
Be sure your answer has the correct number of significant digits.
x10
?

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

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

A solution of sodium cyanide, NaCN, has a pH of 12.10. How many grams of NaCN are in 425 mL of a solution with the same pH?
One half liter (500. mL) of 2.50 M HCl is mixed with 250. mL of 3.75 M HCl. Assuming the total solution volume after mixing is 750. mL, what is the concentration of hydrochloric acid in the resulting solution? What is its pH?
The pH scale was designed to make it convenient to express hydrogen ion concentrations that are small in aqueous solutions. The definiton of pH is in terms of base 10 logarithms. pH = - log[H*] where [H*] is the hydrogen ion concentration. a. If the hydrogen ion concentration in a solution is 7.26 x 10 mol L, the pH is b. If the pH of a solution is 3.607, the hydrogen ion concentration is mol L.
In chemistry, the pH of a solution is a measure of the acidity or alkalinity of a solution. Water has a pH of 7 and, in general, acids have a pH less than 7 and alkaline solutions have a pH greater than 7. Find the pHpH of a solution with a hydronium ion concentration of 7.7 x 10-5 moles/liter. Round your answer to two decimal places, if necessary.
In chemistry, the pH of a solution is a measure of the acidity or alkalinity of a solution. Water has a pH of 7 and, in general, acids have a pH less than 7 and alkaline solutions have a pH greater than 7. Find the pH of a solution with a hydronium ion concentration of 7.4 x 10-³ moles/liter. Round your answer to two decimal places, if necessary.
The concentration of hydronium ion in a sample of a solution is 4.5 x 10-3 mol/L. What is the pH of this solution? The answer should be to the proper number of significant digits
The pH scale was designed to make it convenient to express hydrogen ion concentrations that are small in aqueous solutions. The definiton of pH is in terms of base 10 logarithms. pH = -log[H¹] where [H] is the hydrogen ion concentration. a. If the hydrogen ion concentration in a solution is 5.98 x 10-3 mol/L, the pH is b. If the pH of a solution is 3.171, the hydrogen ion concentration is mol/L.
pH = −log[H+] where [H+] is the hydrogen ion concentration, measured in moles per liter. Solutions with a pH-value of less than 7 are acidic; solutions with a pH-value of greater than 7 are basic; solutions with a pH-value of 7 (such as pure water) are neutral. Black coffee has a pH of 5 and pure water has a pH of 7. Compare the pH of each and determine how much more acidic black coffee is than pure water.
The concentration of hydronium ion in a sample is 3.5 x 10-7 mol/L. What is the pH of the above solution? The question should be answered to the proper number of significant digits.
The pH scale was designed to make it convenient to express hydrogen ion concentrations that are small in aqueous solutions. The definiton of pH is in terms of base 10 logarithms. pH = − log [H+] where [+] is the hydrogen ion concentration. a. If the hydrogen ion concentration in a solution is 4.92 × 10-³ mol/L, the pH is b. If the pH of a solution is 3.078, the hydrogen ion concentration is mol/L.
The pH scale was designed to make it convenient to express hydrogen ion concentrations that are small in aqueous solutions. The definiton of pH is in terms of base 10 logarithms. pH = -log[H+] where [H] is the hydrogen ion concentration. a. If the hydrogen ion concentration in a solution is 5.98 x 10-3 mol/L, the pH is b. If the pH of a solution is 3.735, the hydrogen ion concentration is mol/L.
The concentration of hydroxylamine in a solution is 0.71 M. What is the pH of the solution? The Kb of hydroxylamine (HONH2) is 1.1 x 10−8. Express your answer using at least three significant figures. Do not use scientific notation.