Date: Section: Report Sheet: pH: Measurement and Application. A: Determination of pH Using Acid-Base Indicators: Indicator Color HCI NaH,PO, HC,H,O, ZNSO, Methyl Violet Thymol Blue Methyl Yellow Congo Red Bromocresol Green pH Range

Date: Section: Report Sheet: pH: Measurement and Application. A: Determination of pH Using Acid-Base Indicators: Indicator Color HCI NaH,PO, HC,H,O, ZNSO, Methyl Violet Thymol Blue Methyl Yellow Congo Red Bromocresol Green pH Range

Living by Chemistry

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ISBN:9781464142314

Author:Angelica M. Stacy

Publisher:Angelica M. Stacy

ChapterU6: Showtime: Reversible Reactions And Chemical Equilibrium

Section: Chapter Questions

Problem 19STP

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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

Name:
Date:
Section:
Report Sheet: pH: Measurement and Application.
A: Determination of pH Using Acid-Base Indicators:
Indicator
Color
HCI
NaH,PO,
HC,H,0,
ZnSO,
Methyl Violet
Thymol Blue
Methyl Yellow
Congo Red
Bromocresol
Green
pH Range

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A chemist takes 8.579 mL of liquid acetic acid, CH₃COOH (molar mass: 60.052 g/mol) with 1.05 g/mL density and mix it with 12.305 g of solid sodium acetate, CH₃COONa (molar mass: 82.0343g/mol) and prepare an aqueous solution of 1.0 L by adding required amount of water. (Acidity constant of CH₃COOH is 1.8x10⁻⁵) a) What is the pH of such solution?b) What would the pH of the solution be if 0.020 mol NaOH added?c) What would the pH of the solution be if 0.15 mol NaOH added to the solution in a?d) What would the pH of the solution be if 0.17 mol NaOH added to the solution in a? e) What would the pH of the solution be if 0.020 mol HCl added to the solution in a? f) What would the pH of the solution be if 0.15 mol HCl added to the solution in a?g) What would the pH of the solution be if 0.17 mol HCl added to the solution in a?