| ACIDS | BASES | CONJUGATE ACID-BASE PAIRS | WARM-UP | REVIEW |
|---|---|---|---|---|
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Arrhenius: produce H+ ions in water
Bronsted-Lowry: acids donate a proton (H+)
What is the difference between Arrhenius and Bronsted-Lowry acids?
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Arrhenius bases: produce OH- ions in water (ex. NaOH)
Bronsted-Lowry: proton acceptor (ex. Cl-)
What is the difference between Arrhenius and Bronsted-Lowry bases? Give an example of each.
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each pair is related by the loss & gain of H+
How are conjugate acid-base pairs related?
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1.96 g/L
What is the density of carbon dioxide at STP?
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5.0% m/v glucose
What concentration of glucose is isotonic to our body's?
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hydrosulfuric acid
Name: H2S
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13.9
Calculate the pH of a 0.78 M solution of NaOH.
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NH2 (base) + H2O (acid) --> NH4(conjugate acid) + OH- (conjugate base)
Label each of the following products and reactants as either a base, acid, or its conjugate pair
NH3 + H2O --> NH4+ + OH- |
40 L N2 at STP
50g of N2 has a volume of ____ liters at STP
|
water goes out of the cells by osmosis
In a hypertonic solution...
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HCl - hydrochloric acid
H2S04 - sulfuric acid HNO3 - nitric acid
What are the 3 strong acids you need to know?
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1. ionic compounds containing hydroxide ions (OH-) or oxide ion (O2-)
2. molecular compounds that react with water to produce hydroxide ions
Bases fall into what two categories?
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HSO4- (acid) + H2O (base) --> SO42- (conjugate base) + H3O+ (conjugate acid)
Label each of the following products and reactants as either a base, acid, or its conjugate pair
HSO4- + H2O --> SO42- + H3O+ |
Na+ and Cl- ions on the surface of an NaCl crystal are attracted to polar water molecules; ions become hydrated in solution with many H2O molecules surrounding each ion
Explain the dissolution process of NaCl in water. What happens to the particles at the molecular level?
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hypertonic; greater
In osmosis, water always moves toward the ________ solution: that is, toward the solution with the _____________ solute concentration
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number of hydrogen ions that can be released into the solution by an acid is referred to as the
acids proticity an acid which can release one H+ ion into solution is termed monoprotic and has a proticity of one. Examples of monoprotic acids are HCl, HC2H3O2 (acetic acid) and HNO3. an acid which can release two H+ ions into solution is termed diprotic and has a proticity of two. Examples of diprotic acids are H2SO4, H2C2O4 • 2 H2O (oxalic acid) and H2CO3. an acid which can release three H+ ions into solution is termed triprotic and has a proticity of three
Define: proticity
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Water is amphoteric because it can behave both as an acid and base
What molecule is considered amphoteric? What does this mean?
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a. HF
b. HPO4- c. H2S
What is the conjugate acid?
a. F- b. PO4 2- c. HS- |
decreases
With higher temperatures, gas solubility ____________
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a. no net change in volume
b. increase volume of container c. decrease volume of container
What happens to the elastic container when the following conditions are in place (Pint = pressure inside the container; Pext = pressure outside the container)
a. Pint = Pext b. Pint > Pext c. Pint < Pext |
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STRONG: complete ionization (100%), weak conjugate bases, large concentrations of H30+ and anion (A-)
WEAK: few dissociation (usually less than 1%); most remain undissociated, strong conjugate bases, concentrations of H30+ and anion (A-) are small
What is the difference between weak and strong acids?
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12.7
Calculate the pH of a 0.05 M solution of NaOH
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a. Br-
b. NH2- c. CO3 2-
What is the conjugate base?
a. HBr b. NH3 c. HCO3- |
0.373 M
A 10.0 mL sample of an unknown H3PO4 solution requires 112 mL of 0.100 M KOH to complete react with H3PO4 according to the following reaction. Determine the concentration in molarity of the unknown H3PO4 solution.
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during inhalation, lungs expand, the pressure in the lungs decreases, air flows toward the lower pressure in the lungs
during exhalation, lung volume decreases, pressure within the lung increases, air flows from the higher pressure in the lungs to the outside BOYLE'S LAW: pressure & volume
Explain Boyle's law in context of how we breathe.
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