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The Chemistry of Acids and Bases

The Chemistry of Acids and Bases

The Chemistry of Acids and Bases. Chemistry I – Chapter 19 Chemistry I HD – Chapter 16 ICP – Chapter 23.

By weston
(116 views)

ACIDS & BASES-

ACIDS & BASES-

ACIDS & BASES-. ACIDS & BASES-. Electrolytes: Liquid that allows electricity to flow. Dissociation: Electrolytes break down into ions that conduct electricity. ACIDS & BASES REVIEW. Acids turn Litmus Red. Acids have a pH below 7. Acids are clear in Phenolphthalein.

By gitano
(307 views)

Chapter 14 Acid/Base Equilibrium

Chapter 14 Acid/Base Equilibrium

AP Chemistry Unit 10. Chapter 14 Acid/Base Equilibrium. 1. Some Definitions. Arrhenius An acid is a substance that, when dissolved in water, increases the concentration of hydrogen ions. A base is a substance that, when dissolved in water, increases the concentration of hydroxide ions.

By nanda
(297 views)

The Chemistry of Acids and Bases

The Chemistry of Acids and Bases

The Chemistry of Acids and Bases. Chemistry I – Chapter 19 Chemistry I HD – Chapter 16 IPC – Chapter 23.

By kenna
(57 views)

Acids and Bases Chapter 19

Acids and Bases Chapter 19

Acids and Bases Chapter 19. Some Properties of Acids. Produce H + (as H 3 O + ) ions in water (the hydronium ion is a hydrogen ion attached to a water molecule-this ion determines pH) Taste sour (like vinegar) Corrode metals Electrolytes React with bases to form a salt and water

By latif
(211 views)

Ionic Equilibria I 離子平衡 : Acids and Bases

Ionic Equilibria I 離子平衡 : Acids and Bases

18. 維他命 C Ascorbic acid. Ionic Equilibria I 離子平衡 : Acids and Bases. 檸檬酸 Citric acid. Chapter Goals. A Review of Strong Electrolytes ( 強電解質 ) The Autoionization of Water ( 水的自身離子化 ) The pH and pOH Scales (pH 值和 pOH 值 )

By artie
(152 views)

Ch. 16: Equilibrium in Acid-Base Systems

Ch. 16: Equilibrium in Acid-Base Systems

Ch. 16: Equilibrium in Acid-Base Systems. 16.3a: Acid-Base strength and equilibrium law. Definitions. Arrhenius A: produce H+ in aqueous solution B: produces OH- in aqueous solution very limited Bronsted-Lowry A: H+ donor B: H+ acceptor more general. Acid ionization constant.

By zada
(255 views)

Ch. 16: Equilibrium in Acid-Base Systems

Ch. 16: Equilibrium in Acid-Base Systems

Ch. 16: Equilibrium in Acid-Base Systems. 16.3a: Acid-Base strength and equilibrium law. Definitions. Arrhenius A: produce H + in aqueous solution B: produces OH - in aqueous solution very limited Bronsted -Lowry A: H + donor B: H + acceptor more general. Acid ionization constant.

By eliot
(259 views)

Unit 6: pH Calculations

Unit 6: pH Calculations

Unit 6: pH Calculations. Homework: Read pages: 353-357 WS: Concentration and pH. pH. What is Log 10 ? Power to which 10 must be raised to equal that number Log 1000 = ? 3 pH = -log[H + ]. pH. power of [H + ] pH = – log [H + ] pH = power to which 10 must be raised to equal the [H + ]

By nakia
(136 views)

Intro to Acids & Bases

Intro to Acids & Bases

Intro to Acids & Bases. Acids Taste sour Reacts with metals Turns litmus red Conducts electricity. Base Taste bitter Slippery Turns litmus blue Conducts electricity. Properties of Acids & Bases. Ions in Solution. Acidic solutions – contain more H + than OH -

By ketan
(60 views)

Hydrogen Ions and Acidity

Hydrogen Ions and Acidity

Hydrogen Ions and Acidity. The Ionization of Water and pH. Hydrogen Ions in Water. We are used to thinking of water as a pure liquid that contains only H 2 O molecules. However, as a pure liquid, water ionizes into hydrogen ions and hydroxide ions: H 2 O( l ) → H + ( aq ) + OH - ( aq )

By altessa
(234 views)

Unit 3

Unit 3

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 indicate concentration in mol/L K w = [H + ] [OH - ] = 1.0x10 -14

By lonna
(111 views)

Hydrogen Ions and Acidity

Hydrogen Ions and Acidity

Hydrogen Ions and Acidity. The Ionization of Water and pH. Hydrogen Ions in Water. We are used to thinking of water as a pure liquid that contains only H 2 O molecules. However, as a pure liquid, water ionizes into hydrogen ions and hydroxide ions: H 2 O( l ) → H + ( aq ) + OH - ( aq )

By oral
(138 views)

Thursday, May 15 th : “A” Day Friday, May 16 th : “B” Day Agenda

Thursday, May 15 th : “A” Day Friday, May 16 th : “B” Day Agenda

Thursday, May 15 th : “A” Day Friday, May 16 th : “B” Day Agenda. Collect Crossword Puzzle Collect Concept Review Ch. 15 Review – pass back/warm-up Ch. 15 Test Looking Ahead Mon/Tues: Finals Review Wed/Thurs: Fun Lab/Sr. Finals (Thurs)

By virote
(98 views)

Chemical Reactions 2: Equilibrium & Oxidation-Reduction

Chemical Reactions 2: Equilibrium & Oxidation-Reduction

Chemical Reactions 2: Equilibrium & Oxidation-Reduction. Acid-Base Equilibrium. Acids Fruit juices, soft drinks, gastric juices Sour taste Red and blue litmus paper turn Red Arrhenius: acids release H + when dissolved in Water (aqueous solution)

By zavad
(138 views)

Calculating pH

Calculating pH

Calculating pH. Strong Acids. The seven strong acids are HCl , HBr , HI, HNO 3 , H 2 SO 4 , HClO 3 , and HClO 4 . These are, by definition, strong electrolytes and exist totally as ions in aqueous solution. H 2 O ( l ) + H 2 O ( l ). H 3 O + ( aq ) + OH − ( aq ).

By albin
(121 views)

Strong Acids

Strong Acids

Strong Acids. Strong acids fully dissociate so: They are fully separated into their ions They are good conductors of electricity Are not in a state of equilibrium A 10x dilution results in pH increase of 1 React quickly as [H 3 O + ] is high Examples include: H 2 SO 4 , HNO 3 , HCl.

By yadid
(93 views)

Lecture 2 Dr. Kumar Aid-base balance-Salivary Buffering

Lecture 2 Dr. Kumar Aid-base balance-Salivary Buffering

Lecture 2 Dr. Kumar Aid-base balance-Salivary Buffering. Buffer solutions. Before you start it would be helpful to … know that weak acids and bases are only partly ionised in solution be able to calculate pH from hydrogen ion concentration

By quito
(125 views)

Chemical calculations II

Chemical calculations II

Chemical calculations II. Vladimíra Kvasnicová. Calculation of pH. pH = - log a(H 3 O + ) a = γ x c a = activity γ = activity coefficient c = concentration (mol /L) in diluted (mM) solutions : γ = 1  a = c pH = - log c( H 3 O + )

By leda
(99 views)

Acid and Base Strength

Acid and Base Strength

Acid and Base Strength. Acids. Have a sour taste. Acids. Turn blue litmus red. Turn methyl orange red. Acids. Will react with: some metals to produce a salt and H 2 . metal oxides to produce a salt and H 2 O. metal carbonates to produce a salt, H 2 O, and CO 2.

By urban
(102 views)

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