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pH and Indicators Chemistry Mrs. Coyle
Basic 14>ph>7 Neutral ph=7 Acidic 1
Self Ionization of H 2 O H 2 O H + (aq) + OH - (aq) Ion Product Constant K w for Water: K w = [H + ] x [OH - ] =1.0 x
For pure H 2 O [H + ] = [OH - ] = 1.0 x M
pH 1909 Soren Sorensen (Danish) pH=-log[H + ] What is the pH of pure water?
Ex 1: Find the pH for [H + ]=10 -3 M Answer: pH=3
Ex 2: Find the pH for [H + ]=5x10 -3 M Answer: pH=2.3
Finding [H + ] from pH [H + ]= 10 -pH
Ex 3: Find the [H + ] for pH=5 Answer: [H + ] = M
Ex 4: Find the [H + ] for pH=5.8 [H + ]= 10 -pH Answer: [H + ] = 1.6x10 -6 M
pOH pH=-log[H + ] pH + pOH=14
Basic(Alkaline) Solutions Acidic Solutions Neutral Solutions
Acids Change phenolphthalein to colorless.
Acids Turn litmus paper from blue to red.
Bases Change phenolphthalein to pink.
Aqueous solutions & concepts of pH Chapter I. Ion Product constant - water A. Acids→ hydronium ions (H 3 O+) Bases → hydroxide ions (OH-) B.Self.
Acids and Bases. Ionization of Water H 2 O + H 2 O H 3 O + + OH - K w = [H 3 O + ][OH - ] = 1.0
PH of Weak Acids AP Chemistry Unit 9 Chapter 14. Strengths of Acids and Bases “Strength” refers to how much an acid or base ionizes in a solution. STRONGWEAK.
PH. pH—Scale to measure how acidic or basic a solution is 0-14 Pure water is 7 and neutral (not an acid or base) Acids—less than 7(lower number more acidic)
PH is the measurement of the concentration of H+ ions in a solution. (Or how acidic or basic a solution is.) 1. The pH scale has a range from 1 to 14.
PH and concentration. HIGHER GRADE CHEMISTRY CALCULATIONS pH and Concentration pH is related to the concentration of hydrogen ions. e.g [H + (aq)] = 1.
PH and pOH By: Sam F., Sam D., Rochani, Evan, Will, Sherry, Mariana.
pH Water Water is in equilibrium with its ions H 2 O(l) H + (aq) + OH - (aq) K w = [H + ][OH - ] K w = 1.0 x at 25°C In neutral solutions [H.
INDICATORS & pH: Part 2 What is the difference between an acid and a base? Acid: H 3 O + (hydronium) ion Base: OH - (hydroxyl) ion Acids: react with metals.
pH: a measure of the acidity or basicity of an aqueous solution The measure of hydrogen ions (these are positively charged)
Ch. 8. pH Scale Used to measure how acidic or basic a substance is Ranges from 0-14.
PH Scale. Ion product constant for water K w H 2 O H + + OH - K w = [H + ] [OH - ] = 1.0 X mol/L Since [H + ] = [OH - ] for water Then each equals.
Ch.15: Acid-Base and pH Part 1. Self-Ionization of Water Pure water is a VERY weak electrolyte It undergoes self-ionization H 2 O (l) + H 2 O (l) H 3.
Hydrogen Ions and Acidity Chapter What is K w ? K w is the equilibrium constant for the self-ionization of water Water molecules are in constant.
PH AND POH By: Ben, Josh, Priya, Margarita, Monica, Tharun, Kyra, Cameron.
PH. What is pH? pH is a measure of how acidic or basic a solution is pH of a solution is compared to the pH scale.
The pH scale. pH scale This scale is used to determine the concentrat’n of H + ions versus OH - ions Things that are neutral are pH 7, acids are below.
Acids, Bases, and Solutions A hydrogen ion (H + ) is an atom of hydrogen that has lost its electron. An acid is any substance that produces hydrogen ions.
© Boardworks Ltd 2003 Indicators: the pH scale This attaches a number called the pH value to each universal indicator colour. This means we can quickly.
12. Mixtures Of Strong Acids and Bases (Hebden p. 141 – 143)
Chapter 19 Self-Ionization of Water and pH. Strong vs. Weak Strong: 100% dissociation of H + or OH – – Strong electrolytes (conduct electricity very well)
Mariam Al Thani 7A. The pH scale measures if something is an acid or a base on a scale of 1 to 14. The pH scale measures if something is an acid or a.
Acids and Bases pH Calculations pH scale. pH Scale Created to express acidity as a more simple number than molarity. pH stands for “power” of the hydrogen.
pHpH pH scale- measure of H + ions (acidity); “power of hydrogen” H + = hydronium ion OH- = hydroxide ion #10.
PH of the Lower Cape Fear Estuary Nate Cline CHM 576 November 30, 2009.
KS 3 laboratory Indicators De Lisle Catholic Science College Science department.
Mixtures & Solutions Biology. Mixtures Combination of substances where components retain their own properties Do not combine chemically Are the following.
Acid Base Balance U Normal Values pH – pCO2 – 4.5 – 6 pO2 – 10.6 – 14 HCO3 – BE Lact <2.
ASİT. BAZ [H + ].[OH - ]=1x pH=-log[H + ] pOH=-log[OH - ] pH + pOH=14.
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