acids and bases arrhenius acid – any ha, h2a, h3a, or r-cooh compound where a - is any anion...
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Acids and Bases
Arrhenius acid – any HA, H2A, H3A, or R-COOH compound
where A- is any anionExamples: HCl, H2CO3, H3PO3, CH3COOH
Arrhenius base – any MOH, M(OH)2, or M(OH)3 compound where M+ is either a
metallic cation or the ammonium ionExamples: KOH, Mg(OH)2, Al(OH)3
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Bronsted-Lowry acid – a proton donor Bronsted-Lowry base – a proton acceptor
In acids and bases, to what proton are they referring? Right, the H+ ion is the proton.
Substances that can behave as either an acid or a base are amphoteric or amphiprotic.
Bronsted-Lowry definition
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Acid and Base Characteristics
Acids Have pH < 7 Cause blue litmus
paper to turn red Taste sour React with metals to
produce H2 gas
Bases Have pH > 7 Cause red litmus
paper to turn blue Taste bitter Feel slippery
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Acids and bases react together to form water and a salt. A salt is a chemical compound created from the combination of an acid and a base.
HA + MOH HOH + MA acid base water salt
Neutralization Reactions
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Titration is a lab procedure used to determine the concentration of an unknown solution. Titration problems look no different from the solution stoichiometry problems with which you are already familiar. The only difference is the use of the word titrate. Read “titrate” as “reacts with.”
Titration Problems
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What mass of phosphoric acid is needed to titrate 150 ml of 0.4 M solution of potassium hydroxide?
First, since there are two chemicals reacting, a balanced equation is in order
H3PO4 + 3KOH K3PO4 + 3 H2O
Solving a Titration Problem
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Next, you have the volume and the molarity of the KOH solution. You are looking for the mass of the phosphoric acid.
0.150 L KOH ( 0.4 mol KOH) (1 mol H3PO4)(98 g H3PO4) 1 L KOH 3 mol KOH 1 mol H3PO4
= 1.96 g of H3PO4 needed for reaction
Continuation of Titration Problem
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pH is a measure of the acidity or basicity of a solution. Mathematically, it is expressed as
pH = - log [H+] where the brackets mean molarity
You may see H3O+ referred to as you are reading. H3O+ is the hydronium ion and simply means a hydrogen ion has attached to the water molecule.
For all intents and purposes, H3O+= H+ .
pH, pOH, [H+ ], [OH-]
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You don’t have to understand logarithms to find pH.
It’s as easy as pushing a button on your calculator!
Ex: Find the pH of a solution with an [ H+ ] = 4.2 x 10-5 M.In your calculator: (-) log 4.2 x 10-5 and enter/ =. The pH = 4.38. Note that pH and pOH values do not have units on them. H+ and OH- have units of molarity as they are concentrations.
pH, pOH, [H+ ], [OH-]
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A p function always means to take the negative logarithm of the term.
pH = - log [H+] pOH = - log [OH-]
pH and pOH are relatedpH + pOH = 14
If you know one value, you can find the other by subtracting from 14.
pH, pOH, [H+ ], [OH-]
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Water exists in equilibrium with its ions. H2O (l) H+ (aq) + OH- (aq)
We can write a relationship of the two ions called Kw.
Kw = 1 x 10-14 = [ H+ ] [ OH- ]
This means that if you know one ion concentration, the other can easily be found by substitution into the equality to solve.
pH, pOH, [H+ ], [OH-]
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If you are given pH, you can work backwards to find the hydrogen ion concentration.
Ex: The pH of a solution is 10.8. What is the [ H+ ] pH = - log [H+] 10.8 = - log [H+] divide through by -1 -10.8 = log [H+] On your calculator, push 2nd/shift log (-) 10.8. You
are raising 10 to the power of -10.8. You find the [ H+ ] = 1.58 x 10-11 M.
Finding [ H+ ] given pH