CHEM 1A Chapter Notes - Chapter 8: Titration Curve, Sodium Hydroxide, Buffer Solution

67 views7 pages

browncod58

24 Nov 2016

School

UCSB

Department

Chemistry and Biochemistry

Course

CHEM 1A

Professor

Joseph

For unlimited access to Textbook Notes, a Class+ subscription is required.

psychnerd and 37674 others unlocked

CHEM 1A Full Course Notes

Verified Note

94 documents

Document Summary

8. 1 solutions of acids or bases containing a common ion. When a salt dissolves in water, it breaks up completely into its ions--it is a strong electrolyte: Naf (s) na+ (aq) + f- (aq) The common ion in this solution is f-, since it is produced by both hydrofluoric acid and sodium fluoride. The dissociation equilibrium for hf in the second solution will be driven to the left by the presence of the f- ions from the naf. The shift in equilibrium position that occurs because of the addition of an ion already involved in the equilibrium reaction is called the common ion effect. Also important in solutions of polyprotic acids. The production of protons by the first dissociation step greatly inhibits the. The most important application of acid-base solutions containing a common ion is buffering. A buffered solution is one that resists a change in ph when either hydroxide ions or protons are added.

Related Questions

Need help with red starred sections. Please explain how you got your answer!

Part A A fuel cell differs from a battery because the current is being generated from a reduction-oxidation (redox) reaction in which the reactant is consumed. A classic example of a fuel cell is the phosphoric acid fuel cell (PAFC), which have been used in stationary power generators, buses, and even submarines. Fuel cells require an electrolyte (similar to batteries) to carry electrically charged species between the electrodes, and a PAFC utilizes phosphoric acid (H3PO4) as its electrolyte. Phosphoric acid has three acidic protons that can dissociate in water, as highlighted in red here: H3PO4. However, it is considered a weak acid because some of the acid will remain in molecular form when dissolved in water. Write the complete ionic equation that depicts the dissociation of the first proton for the weak acid phosphoric acid (H3PO4). Make certain you include all charges for any ions produced. Express you answer as a chemical equation including phases. Titrations as analytical neutralization reactions Neutralization reactions can occur between any combination of weak/strong acids and bases. When we want to determine the concentration of a base in solution, we can apply the concept of neutralization by reacting the base with a known amount of an acid in the presence of an indicator (a compound that changes color depending on the pH). This method of determining the concentration of a base is called acid-base titration, and it can also be used to determine the concentration of an acid by titrating it with a known amount of base. A common acid to use for titrations is potassium hydrogen phthalate (written as KHP or KHPh; do not confuse the P for phosphorus). The reason KHP is common is because it is solid at room temperature, and we can accurately mass the amount that is added to solution. As a soluble salt, KHP completely dissociates to form a potassium ion (K+) and an acidic hydrogen phthalate ion (HPâ), which is a weak acid that has only one acidic hydrogen. This ionization is depicted below. KHP(s) â K+(aq)+HPâ(aq) Although ionization (the formation of ions) occurs as a result of acid dissociation for most weak acids, KHP ionizes before acid dissociation occurs. In other words, HPâ is a weak acid ion. Part C If you wanted to determine how much KOH (potassium hydroxide; a strong base) was dissolved in water, you could titrate it with a known amount of KHP (potassium hydrogen phthalate; a weak acid) until a color change indicates that the base is completely neutralized. The molecular equation below depicts this neutralization reaction. KHP(aq)+KOH(aq)âK2P(aq)+H2O(l) Write the net ionic equation that depicts the neutralization of the base by potassium hydrogen phthalate. Instead of using the entire chemical formula of phthalate, use HPâ to represent the acidic hydrogen phthalate ion and P2â to represent the phthalate ion. Express your answer as a net ionic equation including phases.

Exp 25. pH Measurements- Buffers and Their Properties

I need help with finding kPa in the calculations part C for 1,2, and 3 Thanks!