Presentation is loading. Please wait.

Presentation is loading. Please wait.

Salts and Buffers Ch17 4.17.2.

Published byHamdani Sukarno Budiaman Modified over 5 years ago

Similar presentations

Presentation on theme: "Salts and Buffers Ch17 4.17.2."— Presentation transcript:

1 Salts and Buffers Ch17 4.17.2

2 Acid – Base Properties of Salt
Salt is another name for ionic compound When a salt dissolves in water, it breaks into its ions Under certain situations, these ions can behave like acids and bases, affecting the pH of solutions!

3 3 ways a salt can affect pH
A salt can dissociate to form: A neutral soln (pH = 7) An acidic soln (pH < 7) A basic soln. (pH > 7) How do we predict how a salt will behave? We look at the cation and anion of the dissociated salt.

4 Salts that Produce Neutral Solutions
Contain conjugate bases of strong acids Contain cations from strong bases Strong acids Conjugate Base Example of salt HCl Cl- NaCl HBr Br- NaBr HI I- KI HClO3 ClO3- KClO3 Strong Base Cation Example of salt NaOH Na+ NaCl CsOH Cs+ CsI Ca(OH)2 Ca+ Ca(ClO3)2 Sr(OH)2 Sr2+ SrSO4

5 Salts that produce neutral solutions
NaOH Na OH- HCl H Cl- Neutralization reaction

6 Neutral Solutions- WHY?
So why does a salt containing the conjugate base of a strong acid and the conjugate acid of a strong base produce a neutral solution? HCl NaOH Strong acid = Strong base = b/c so weak neither will be gaining H+ or give up H+ so don’t affect pH as pH depends on [H+]

7 Salts that produce basic solutions
Salts derived from a strong base and a weak acid NaC2H3O2 Na+ (aq) + C2H3O2-(aq) C2H3O2-(aq) + H2O HC2H3O2 + OH- Why? b/c conjugate base of the weak acid is a strong base It deprotonates water thus increasing [OH-], increasing basicity H2O

8 So, the weak salt’s ANION must be the conjugate base of a weak acid
The salts CATION must be the cation of strong base salt Cation and Strong base Anion and weak acid Sr(CN)2 Sr Sr(OH)2 CN HCN KF K KOH F HF NaNO2 Na NaOH NO HNO2

9 Why is this useful Why would we need to know the type of solution that a salt produces/ Well, we are interested in pH for all kinds of important reactions, like controlling the pH of our blood and water sources. These things contain salts, which affect this pH. So how do we do pH calculations for solutions containing a salt??

10 Calculate the pH of a 0.30M NaF solution. The Ka for HF =7.2x10-4
NaF Na F- (from SB) (from WA) step 1: identify major species Step 2: write dominate reaction

11 Calculate the pH of a 0.30M NaF solution. The Ka for HF =7.2x10-4
Step 3: calculate Kb, using Ka and Kw Ka x Kb = Kw Acid Conj base Kb=Kw/Ka (for HF) Kb =

12 Calculate the pH of a 0.30M NaF solution. The Ka for HF =7.2x10-4
Step 4 make icebox F H2O (l) HF OH-

Download ppt "Salts and Buffers Ch17 4.17.2."

Similar presentations

Acid-Base Equilibria: Acids and Bases

Acid-Base Equilibria: Acids and Bases
Salts and pH. Soluble salts dissociate in water to produce ions. Salts are basically ionic compounds that can be formed from the reaction from an acid.

Salts and pH. Soluble salts dissociate in water to produce ions. Salts are basically ionic compounds that can be formed from the reaction from an acid.
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.

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.
Acid Strength and Structure Acid-Base Properties of Salts AP Chemistry.

Acid Strength and Structure Acid-Base Properties of Salts AP Chemistry.
Chapter 16: Aqueous Ionic Equilibria Common Ion Effect Buffer Solutions Titrations Solubility Precipitation Complex Ion Equilibria.

Chapter 16: Aqueous Ionic Equilibria Common Ion Effect Buffer Solutions Titrations Solubility Precipitation Complex Ion Equilibria.
Updates Assignment 04 is is due today (in class) Midterms marked (in the box); solutions are posted Assignment 03 is in the box.

Updates Assignment 04 is is due today (in class) Midterms marked (in the box); solutions are posted Assignment 03 is in the box.
Chapter 19 More about ACID-BASES. Self-Ionization of Water Two water molecules produce a hydronium ion & a hydroxide ion by the transfer of a proton.

Chapter 19 More about ACID-BASES. Self-Ionization of Water Two water molecules produce a hydronium ion & a hydroxide ion by the transfer of a proton.
14.1 Intro to Acids and Bases 14.2 Acid Strength 14.3 pH Scale

14.1 Intro to Acids and Bases 14.2 Acid Strength 14.3 pH Scale
Part II. Polyprotic acid H 2 CO 3 H + + HCO 3 - Ka 1 = 4.3 x 10 -7 H 2 CO 3 H + + HCO 3 - Ka 1 = 4.3 x 10 -7 HCO 3 - H + + CO 3 -2 Ka 2 = 4.3 x 10 -10.

Part II. Polyprotic acid H 2 CO 3 H + + HCO 3 - Ka 1 = 4.3 x H 2 CO 3 H + + HCO 3 - Ka 1 = 4.3 x HCO 3 - H + + CO 3 -2 Ka 2 = 4.3 x
Chapter 14 Acids and Bases AP*. Section 14.8 Acid-Base Properties of Salts Salts  Ionic compounds.  When dissolved in water, break up into its ions.

Chapter 14 Acids and Bases AP*. Section 14.8 Acid-Base Properties of Salts Salts  Ionic compounds.  When dissolved in water, break up into its ions.
Salts as Acids and Bases Cations Sloshing Anions Sloshing Salt Ionic Compound Dissolves Ions Slosh Ions as Acids Ions as Bases Assuming that only one ion.

Salts as Acids and Bases Cations Sloshing Anions Sloshing Salt Ionic Compound Dissolves Ions Slosh Ions as Acids Ions as Bases Assuming that only one ion.
The Equilibrium of Weak Acids and Bases Weak Acids Molecules HF (aq) + H 2 O (l) ↔ H 3 O + (aq) + F - (aq) Cations NH 4 + (aq) + H 2 O (l) ↔ H 3 O +

The Equilibrium of Weak Acids and Bases Weak Acids Molecules HF (aq) + H 2 O (l) ↔ H 3 O + (aq) + F - (aq) Cations NH 4 + (aq) + H 2 O (l) ↔ H 3 O +
1 The Chemistry of Acids and Bases Chapter 16. 2 Some Properties of Acids þ Produce H + ions in water þ Taste sour þ Corrode metals þ Electrolytes þ React.

1 The Chemistry of Acids and Bases Chapter Some Properties of Acids þ Produce H + ions in water þ Taste sour þ Corrode metals þ Electrolytes þ React.
CHAPTER 14 AP CHEMISTRY. NATURE OF ACIDS AND BASES Acids - sour Acids - sour Bases (alkali) - bitter and slippery Bases (alkali) - bitter and slippery.

CHAPTER 14 AP CHEMISTRY. NATURE OF ACIDS AND BASES Acids - sour Acids - sour Bases (alkali) - bitter and slippery Bases (alkali) - bitter and slippery.
Hydrolysis and Neutralization

Hydrolysis and Neutralization
ICS Madrid Acids, Bases and Salts Left click your mouse to continue.

ICS Madrid Acids, Bases and Salts Left click your mouse to continue.
Acids, Bases, and SALTS According to Arrhenius theory, Acid + base  salt + water Examples: HCl + NaOH  NaCl + H 2 O H 2 SO 4 + Sr(OH) 2  SrSO 4 + 2H.

Acids, Bases, and SALTS According to Arrhenius theory, Acid + base  salt + water Examples: HCl + NaOH  NaCl + H 2 O H 2 SO 4 + Sr(OH) 2  SrSO 4 + 2H.
Salts product of neutralization reaction 1.00 M NaOH mol OH - L 0.075 mol1.00 mol L x L x = 0.075L H+H+ + Cl - + Na + + OH -  H2OH2O+ Na + + Cl - NaCl.

Salts product of neutralization reaction 1.00 M NaOH mol OH - L mol1.00 mol L x L x = 0.075L H+H+ + Cl - + Na + + OH -  H2OH2O+ Na + + Cl - NaCl.
Hydrolysis and Neutralization

Hydrolysis and Neutralization
According to the Arrhenius concept, a base is a substance that produce OH - ions in aqueous solution. According to the Brønsted-Lowry model, a base is.

According to the Arrhenius concept, a base is a substance that produce OH - ions in aqueous solution. According to the Brønsted-Lowry model, a base is.

Similar presentations

Ads by Google