QUESTION 9Calculate the pH when 1.199 g of HCOONA (FW 68.01 g/mol) is added to 40.4 mL of 0.500 M formic acid, HCOH (FW = 46.03 g/mol). Ignore any changes in volume. The K, value for HCOOH is 1.8 x 10 4.Enter your answer in decimal format with two decimal places (value ± 0.05).

Given : Mass of HCOONa = 1.199 g Concentration of HCOOH = 0.500 M Volume of HCOOH solution = 40.4 =…

Calculate the pH when 1.199 g of HCOONA (FW - 68.01 g/mol) is added to 40.4 ml of 0.500 M formic acid, HCOOH (FW - 46.03 g/mol). Ignore any changes in volume. The Ka value for HCOOH is 1.8 x 10-4. Enter your answer in decimal format with two decimal places (value + 0.05).

Calculate the pH when 1.199 g of HCOONA (FW - 68.01 g/mol) is added to 40.4 ml of 0.500 M formic acid, HCOOH (FW - 46.03 g/mol). Ignore any changes in volume. The Ka value for HCOOH is 1.8 x 10-4. Enter your answer in decimal format with two decimal places (value + 0.05).

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 116QRT

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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.

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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.

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

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