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What is a solution?What are the differences between unsaturated,
saturated, and supersaturated solutions?What are some of the general properties of an
acid?What are some of the general properties of a
base?What is a neutralization reaction? What is the pH scale?How is pH used to describe the concentration of
acids and bases?
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PSc.2.2.6 ◦ Recognize common inorganic acids including hydrochloric (muriatic)
acid, sulfuric acid, acetic acid, nitric acid and citric acid. ◦ Recognize common bases including sodium bicarbonate, and
hydroxides of sodium, potassium, calcium, magnesium, barium and ◦ ammonium. ◦ Define acids and bases according to the Arrhenius theory. ◦ Develop an understanding of the pH scale and the classification of
substances therein. ◦ Generalize common characteristics of acids and bases– pH range,
reactivity with metals and carbonates (acids) or fats/oils (bases), ◦ conductivity. ◦ Relate general household uses of acids and bases with their
characteristic properties. ◦ Explain what happens in a neutralization reaction, identifying each
component substance.
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Solution: A type of homogeneous mixture formed when one substance dissolves in another.
There are two parts to a solution1.Solute – the substance that is dissolved.2.Solvent – the substance that causes the other to
dissolve. (Water is usually the solvent.)Example: Lemonade
What part of the lemonade is the solute?lemon juice and sugar
What part of the lemonade is the solvent?water
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Solubility: The maximum amount of a solute that can be dissolved in a given amount of solvent at a given temperature.
Soluble – anything that dissolves in another substance.◦ Ex: Salt is soluble in water.
Insoluble – anything that does not dissolve in another substance.◦ Ex: Oil is insoluble in water.
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If you continue adding sugar to lemonade, eventually the point is reached when no more sugar dissolves and the excess granules sink to the bottom of the glass.
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Unsaturated – more solute can be dissolved in the solvent
Saturated – no more solute can be dissolved in the solventat the current temperature.
Generally, as the temperature of a liquid solvent increases, the amount of solid solute that can dissolve in it also increases.
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Supersaturated –contains more solute than a saturated solution at the same temperature. ◦Ex: Rock Candy is made in this way.
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Solubility Curve Each line on the graph
is called a solubility curve for a particular substance.
You can use a solubility curve to figure out how much solute will dissolve at any temperature given on the graph.
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1. A(n) __________ solution is any solution that can dissolve more solute at a given temperature.
A. electrolyteB. saturatedC. supersaturatedD. unsaturated
The answer is D. A saturated solution contains all the solute it can hold at that temperature, but an unsaturated solution can hold additional solute.
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2. What is a solubility curve used for?
Answer: You can use a solubility curve to figure out how much solute will dissolve at any temperature given on the graph.
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3. The substance being dissolved in a solution is the __________.
A. aqueous phaseB. mediaC. soluteD. solvent
Answer is C. The solute dissolves into the solvent
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An acid is defined by Arrhenius as a substance that dissociates to produce hydrogen ions (H+)
in a water solution.
HCl → H++ Cl-
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Contains hydrogen
Taste sour
Reacts with metals to form hydrogen gas
Reacts with carbonates to form carbon dioxide, water and a salt
Corrode metals
Electrolytes
pH is less than 7
Turns blue litmus paper to red
Mg + 2HCl MgCl2 + H2
Na2CO3 + 2HCl CO2 + H2O + 2NaCl
Conducts Electricity
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HCl (hydrochloric acid) - gastric juiceH2SO4 (sulfuric acid) - fertilizer, car batteriesHC2H3O2 (acetic acid) - vinegarHNO3 (nitric acid) - fertilizersH3C6H5O7 (citric acid) – fruitsOther common uses: dyes, paints, food
preservation & preparation
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A base is defined by Arrhenius as a substance that produces hydroxide ions OH- in a water solution.
NaOH → Na+ + OH-
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Contains OH-
Taste bitter
Electrolytes
Feel soapy, slippery
pH greater than 7
Turns red litmus paper to blue
Reacts with fats/oils to produce soaps
Conducts Electricity
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NaOH - lye, drain and oven cleaner
Mg(OH)2 - laxative, antacid, milk of magnesia
NaHCO3 – cooking, antacid
KOH – batteries, biodiesel, soaps
Ca(OH)2 – cement
Ba(OH)2 – waste water treatment
NH4OH – food processing
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1. The pH of an acidic solution is a. Less than 0. c. Less than 7.b. Greater than 14. d. Greater than 7.
2. A solution whose pH is 7a. Is acidic. c. Is neutral.b. Is basic. d. Is none of the others.
3. Solubility is the _____ amount of a _____ that can be dissolved in a given amount of ______ at a given temperature.a. Least, solute, solventb. Max, solute, solventc. Least, solvent, soluted. Max, solvent, solute
Warm-Up - Warm-Up - Write the Write the questionsquestions
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pH◦The pH scale is used to determine how acidic or basic
a solution is.◦measured with a pH meter or an indicator with a
wide color range. (Litmus Paper)◦Ranges from 0 to 14◦7 is neutral
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Reaction of acid and a base forms a salt and water – ALWAYS
Note: A salt is an ionic compound
1. NaOH + HCl NaCl + H2O
Acid?
Base?
Salt?
HCl
NaOH
NaCl
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2. 2HNO3+ Ba(OH)2 H2O + Ba(NO3)
Acid?
Base?
Salt?
H3PO4
NaOH
Na3PO4
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3. 2LiOH + H2SO4 2H2O + Li2SO4
4. 2HClO4 + Ca(OH)2 Ca(ClO4)2 + 2 H2O
5. KOH + HNO3 H2O + KNO3
6. H3PO4 + NaOH H2O + Na3PO4
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Review
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1. The substance being dissolved is called _________.
2. The substance doing the dissolving is called __________.
3. A solution is a ______________ mixture.4. A solution that can dissolve more. _________5. A solution that can dissolved no more.
___________6. A solution that has dissolved more than
normal. ________________
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7. Substances that in solutions have H+ (hydrogen) ions are…
8. Acids produce what in water solution? 9. The acid in oranges. 10.The acids in fertilizers.11.The acid in your stomach.13.Solutions that have OH- ions are 14.Bases produce what in solution? (name)
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14.Base that is in batteries15.Base in milk of magnesia16.Bases have a ______feel and ________ taste.17.Acids have a _______ taste.18.Acids and bases are both corrosive and react
with indicators to produce a _______ change.19.Both produce ions in water and are therefore
_____________.