C. Johannesson III. Titration (p. 493 - 503) Ch. 15 & 16 - Acids & Bases.

Slides:

Advertisements

Similar presentations

Neutralization Reactions

Advertisements

III. Titration (p. 493 – 503) Ch. 15 & 16 – Acids & Bases.

III. Titration (p ) Ch. 15 & 16 - Acids & Bases.

Acid-Base Reactions. Review Acids are proton (H +1 ion) donors. ◦ H 2 SO 4 (aq) + H 2 O(l)  HSO 4 -1 (aq) + H 3 O +1 (aq)  In this reaction, H 2 SO.

Neutralization Reactions Reaction that occurs between an acid and a base. Example: HCl + NaOH  NaCl + H 2 O & Water Products always include: A “Salt”

Warm up What is the molarity of a 500mL solution that contains 2.9 grams of hydrochloric acid, HCl? 2. What is the pH and pOH of that solution?

Titration.  Titration Analytical method in which a standard solution is used to determine the concentration of an unknown solution. standard solution.

Titration.  Titration Analytical method in which a standard solution is used to determine the concentration of an unknown solution. standard solution.

Topic: Titration Do Now:.

Neutralization Chapter 21.

Acid-Base Titrations.

Le Châtelier’s principle. The significance of Kc values If Kc is small (0.001 or lower), [products] must be small, thus forward reaction is weak If Kc.

Molarity by Dilution Diluting Acids How to Calculate Acids in concentrated form are diluted to the desired concentration using water. Moles of acid before.

Neutralization Reactions

(equimolar amounts of acid and base have reacted)

Reactions of Acids & Bases Reactions of Acids & Bases.

Section 16.3 Titrations and Buffers 1.To know how to neutralize acids and bases (titration) Learning Goal.

Acids and Bases

What type of reaction? HCl + NaOH  H2O + NaCl

Topic: Titration Do Now:. Acid-Base Titration A procedure used in order to determine the molarity of an acid or baseA procedure used in order to determine.

Catalyst 1. What is the difference between a strong base and a weak base? 2. What does it mean for something to dissociate? 3. What are the units of Molarity?

Chapter 15 &. Properties of acids n Taste Sour (kids, don’t try this at home). n Conduct electricity. n Some are strong, some are weak electrolytes. n.

Concentrations: amount of solute present in a given mass or volume of solution. % by Mass – % solute = mass of solute/mass of solution x 100% A 10%

DAILY QUESTION November 25, A neutralization reaction occurs between an ______ and a _______.

I. Introduction to Acids & Bases Acids & Bases. A. Properties  electrolytes  turn litmus red  sour taste  react with metals to form H 2 gas  slippery.

Lab 20- Acids & Bases Titration.

Unit 13 Acids and Bases. D. Finding the pH of Solutions Self- ionization of water – the simple dissociation of water H 2 O H + + OH - Concentration of.

TITRATION Titration of a strong acid with a strong base ENDPOINT = POINT OF NEUTRALIZATION = EQUIVALENCE POINT At the end point for the titration of a.

C. Johannesson III. Titration/Neutralization 18.4 Ch. 18- Acids & Bases.

Ch Acids & Bases III. Neutralization (p )  Neutralization Reaction  Titration.

III. Titration (p ) Ch. 16 – Determining pH and Titrations.

Unit 3 Acids and Bases. Hydrogen ions and pH Ion product constant of water (K w ) H 2 O  H + + OH - In pure water : [H + ] = [OH - ] * [ ] are used to.

Loose Ends from Bell Work An acidic solution makes the color of pH paper turn ___________________, while a basic solution makes the color of pH paper turn.

C. Johannesson III. Titration Ch. 14 & 15 - Acids & Bases.

Titrations. Standard Solution Sample Solution Burette A titration is a volumetric analysis technique used to find the [unknown] of a sample solution by.

Titrations Chapter 13.

Titration  Lab technique commonly utilized to determine an UNKNOWN concentration of a chemical compound with a KNOWN concentration of another chemical.

Titration. Definition Process used to determine the strength of an unknown acid or base Can determine the unknown acid by adding to it a base of known.

Acid-Base Reactions and Titrations Chemistry. Examples of Acid-Base Rxns HNO 3 + KOH  H 2 O + KNO 3 H 2 SO NH 4 OH  (NH 4 ) 2 SO H 2 O LiOH.

Acids and Bases Notes Part 2 Acid Rain Many industrial processes produce gases such as NO, NO 2, CO 2, SO 2, and SO 3. These compounds can dissolve in.

Objectives Describe how an acid-base indicator functions. Explain how to carry out an acid-base titration. Calculate the molarity of a solution from titration.

Warm Up What is the molarity of a 500mL solution that contains moles of HCl? 2. What is the pH and pOH of that solution? 3. What is a.

Indicators And Titration. Indicators Usually organic acid or base whose color is sensitive to pH Indicator is weak acid or base In basic solution, indicator.

I. Introduction to Acids & Bases Acids & Bases. A. Properties  electrolytes  turn blue litmus red  sour taste  react with metals to form H 2 gas 

DO NOW!!! What is the molarity of a 500mL solution that contains 0.29 moles of hydrochloric acid, HCl? 2. What is the pH and pOH of that solution?

WARM UP 1. Write the equation for the neutralization reaction between sulfuric acid (H 2 SO 4 ) and ammonium hydroxide (NH 4 OH).

Fun fun. Acid-Base Reactions. Acid-Base Neutralization  Acids and bases will react with each other to form water and a salt.  Water has a pH of 7—it.

Aim: How can we use titration to find the strength of a solution? Do Now: 1.Take out a calculator and reference tables. 2.Write a neutralization reaction.

Titration A standard solution is used to determine the concentration of another solution.

Acids & Bases Titration.

v. Neutralization reactions

Acids & Bases III. Titration.

Ch Acids & Bases III. Neutralization (p )

Ch. 15 & 16 - Acids & Bases III. Titration (p )

Acids & Bases III. Titration.

Acids & Bases Titration.

Unit 13 – Acid, Bases, & Salts

Titration standard solution unknown solution Titration Analytical method in which a standard solution is used to determine the concentration of an unknown.

Titration Acids & Bases.

Unit 13 – Acid, Bases, & Salts

Acid-Base Reactions are Neutralization Reactions

Unit 13 – Acid, Bases, & Salts

Ch. 15 & 16 - Acids & Bases III. Titration (p )

Acids & Bases III. Titration.

Ch Acids & Bases.

Unit 14 – Acid, Bases, & Salts

Ch. 15 & 16 - Acids & Bases III. Titration (p )

Unit 13 – Acid, Bases, & Salts

Ch. 15 & 16 - Acids & Bases III. Titration (p )

Presentation transcript:

C. Johannesson III. Titration (p ) Ch. 15 & 16 - Acids & Bases

LPChem:Wz A. Neutralization  Chemical reaction between an acid and a base.

LPChem:Wz A. Neutralization  Chemical reaction between an acid and a base.  Products are a salt (ionic compound) and water.

C. Johannesson A. Neutralization ACID + BASE  SALT + WATER HCl + NaOH  NaCl + H 2 O Salts can be neutral, acidic, or basic! Neutralization does not always mean pH = 7. strong acid strong base neutral salt

C. Johannesson A. Neutralization ACID + BASE  SALT + WATER HCl + CuOH  CuCl + H 2 O HC 2 H 3 O 2 + NaOH  NaC 2 H 3 O 2 + H 2 O weak acid strong acid weak base strong base acidic salt basic salt

LPChem:Wz A. Neutralization ACID + BASE  SALT + WATER Strong + Strong  Neutral + water Acid Base Salt. Strong + Weak  Acidic + water Acid Base Salt. Weak + Strong  Basic + water Acid Base Salt.

C. Johannesson B. Titration  Titration Analytical method in which a standard solution is used to determine the concentration of an unknown solution. standard solution unknown solution

LPChem:Wz  Equivalence point  Point at which equal amounts of H 3 O + and OH - have been added.  (moles H 3 O + = moles OH - ) Mathematically determined by… Rapid pH change B. Titration

C. Johannesson  End Point  Visual end of titration indicator color change Should be very similar to equivalence point. B. Titration

 Strong Acid & Strong Base =  Titration equivalence is at pH = 7 LPChem:Wz Neutral Salt

B. Titration  Strong Acid & Weak Base =  Titration equivalence at pH < 7 LPChem:Wz Acidic Salt On your homework today, do #3 like this.

B. Titration  Weak Acid & Strong Base =  Titration equivalence at pH > 7 LPChem:Wz Basic Salt

C. Johannesson B. Titration moles H 3 O + = moles OH - M  V  n = M  V  n M:Molarity V:volume n:# of H + ions in the acid or OH - ions in the base

LPChem:Wz B. Titration  10.0 mL of 2.3M LiOH are required to neutralize 20.0 mL of HNO 2. Find the molarity of HNO 2. H3O+H3O+ M = ? V = 20.0 mL n = 1 OH - M = 2.3M V = 10.0 mL n = 1 MV# = MV# (2.3M)(10.0mL)(1) = M(20.0mL)(1) M = 1.15M HNO 2

C. Johannesson B. Titration  42.5 mL of 1.3M KOH are required to neutralize 50.0 mL of H 2 SO 4. Find the molarity of H 2 SO 4. H3O+H3O+ M = ? V = 50.0 mL n = 2 OH - M = 1.3M V = 42.5 mL n = 1 MV# = MV# (1.3M)(42.5mL)(1) =M(50.0mL)(2) M = 0.55M H 2 SO 4