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Metal halides

Double Replacement Products - Notes

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Chemistry
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Solutions
Chemical properties
Chemical equation
equations
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Spectator ion
Metal halides
Precipitation
Lead(II) chloride
Salt metathesis reaction
Sodium sulfate
solubility

Notes - Double Replacement Products TERMS Soluble - substances that can be dissolved in water. Insoluble - substances that cannot be dissolved in water. Precipitate - a substance that falls out of solution when it is one of the products of a reaction. Precipitates are insoluble in water. The symbol for a precipitate is ? and would be a solid (s) for the state of matter RULES In a double replacement reaction the metal parts of each reactant switch places. Write down the new products. Look up the new products in a table of solubilities. If a product is listed as being insoluble, this product is a precipitate. Write the symbol for a precipitate, ? , after any product that is listed in the table of solubilities as being insoluble.

lab10

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Chemistry
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Chemistry
Iodides
Metal halides
Oxidizing agents
Silver compounds
Lead compounds
Potassium iodide
Lead(II) iodide
Silver nitrate
Precipitation
Silver iodide
Purified water

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Chapter 5b

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Chemistry
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Chlorides
Metal halides
Titration
Silver chloride
Stoichiometry
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Potassium hydroxide
health
behavior
Human development
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Love
Psychoanalysis
Human behavior
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Chemistry 1210: Introduction to General Chemistry Dr. Gina M. Florio 27 Sept. 2012 Jespersen, Brady, Hyslop Chapter 5B Molecular View of Reactions in Aqueous Solution Properties of Solutions: Quantitative Composition The molar concentration or molarity (M) is defined as: units of M = mol/L (mol L-1) Example: How many grams of AgNO3 are needed to prepare 250 mL of a 0.0125 M AgNO3 solution? NOTE: You can also solve this for concentration OR liters of solution CH. 5 Properties of Solutions: Quantitative Composition Solutions of high concentration can be diluted to make solutions of lower concentration. Dilution: CH. 5 Example: How much 1.0 M CuSO4 (aq) solution is required to prepare 250 mL of a 0.10 M CuSO4 (aq) solution? How much water is required? Solution Stoichiometry CH. 5

ch. 4

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Physics
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Chemistry
Chlorides
Metal halides
Bases
Equilibrium chemistry
Oxidizing agents
redox
Chemical equation
Lead(II) chloride
Iron(III) chloride
Precipitation
Hydrogen chloride

Chapter 4 Practice Test 1. A 20.0-g sample of HF is dissolved in water to give 2.0 ? 102 mL of solution. The concentration of the solution is: a) 1.0 M b) 3.0 M c) 0.10 M d) 5.0 M e) 10.0 M Ans: d) 5.0 M Page: 4.3 2. Which of the following aqueous solutions contains the greatest number of ions? a) 400.0 mL of 0.10 M NaCl b) 300.0 mL of 0.10 M CaCl2 c) 200.0 mL of 0.10 M FeCl3 d) 200.0 mL of 0.10 M KBr e) 800.0 mL of 0.10 M sucrose ANS: b) 300.0 mL of 0.10 M CaCl2 PAGE: 4.3 3. What mass of calcium chloride, CaCl2, is needed to prepare 2.850 L of a 1.56 M solution? a) 25.9 g b) 60.8 g c) 111 g d) 203 g e) 493 g ANS: e) 493 g PAGE: 4.3 4. What volume of 18.0 M sulfuric acid must be used to prepare 15.5 L of 0.195 M H2SO4? a) 168 mL

Nomenclature

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Chemistry
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Chemistry
Inorganic chemistry
ion
Physical chemistry
Chemical nomenclature
Coordination complex
Nitride
Iodide
IUPAC nomenclature of inorganic chemistry
Metal halides

9/13/12 12:51 PM Nomenclature of binary inorganic compounds (naming) Binary: Cation (+) Anion (-) NaCl Na+ & Cl- MgF2 Mg2+ 2F- Acetic acid HC2H3O2 Iron (III) Chloride FeCl3 Type 1: made up of cations that form only one type of charge NaNa+ AlAl3+ Type 2: the cations form more than one type of charge FeFe2+ or Fe3+ CuCu1+ or Cu2+ Type 3: hydrates: CuSO4 x 6H2 O Type 4: non-metal + non-metal Binary compounds Type 5: Acids *First column of periodic table alkali metals (1+ charge) *2nd column of p.t. alkaline earth metals (2+ charge) *Ag 1+ -- Zn 2+ -- Al 3+ (diagonal line) 1-2-3 Noble gases Stair case on p.t. right of staircase are noble gases/non-metals Chem 109 Nomenclature 9/13/12 12:51 PM Fl, Cl, Br row form 1- 2+Ca|Br21- Oxidation state & Charge
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