A chemist dissolves 625. mg of pure barium hydroxide in enough water to make up 160. mL of solution. Calculate the pH of the solution. (The temperature of the solution is 25 °C.) Round your answer to 3 significant decimal places. 0 X 5

A chemist dissolves 625. mg of pure barium hydroxide in enough water to make up 160. mL of solution. Calculate the pH of the solution. (The temperature of the solution is 25 °C.) Round your answer to 3 significant decimal places. 0 X 5

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 1ALQ: Consider two beakers of pure water at different temperatures. How do their pH values compare? Which...

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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

Please explain this question, because the answer I got was wrong.

A chemist dissolves 625. mg of pure barium hydroxide in enough water to make up 160. mL of solution. Calculate the pH of the solution. (The temperature of
the solution is 25 °C.)
Round your answer to 3 significant decimal places.
X
Ś

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Step 2: Calculate the Concentration of Barium Hydroxide

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Step 3: Find the pOH Value

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Step 4: Find the pH Value

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