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SOLUTIONS, ACID AND BASES

SOLUTIONS, ACID AND BASES. Solution mixture that has the same composition color , density and taste throughout. Solute substance being dissolved. Solvent substance doing dissolving * Solutions can also be gaseous, like the air you breath, or even solid, like brass and sterling silver.

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SOLUTIONS, ACID AND BASES

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  1. SOLUTIONS, ACID AND BASES

  2. Solution • mixture that has the same composition color, density and taste throughout • Solute • substance being dissolved • Solvent • substance doing dissolving • * Solutions can also be gaseous, like the air you breath, or even solid, like brass and sterling silver.

  3. When forming a solution, there are three ways to speed up the rate of the dissolving process: Stirring • brings more solvent in contract w/ solute Increase Surface area • by breaking up a solid, for instance, by crushing it into a powder, allows more solvent to come in contract w/ solute Increase temperature • increasing temperature speeds up particles causing them to bump each other, breaking apart and coming in contract w/ solvent

  4. Solubility • maximum amount of a solute that can be dissolved in a given amount of solvent at a temperature Concentration • percent by volume of solute in solvent • concentrated– large amount of solute in solvent • dilute– small amount of solute in solvent

  5. Solutions, Solubility & Concentration

  6. Types Of Solution

  7. Acids, Bases and Salts

  8. Four properties of acids: • acids taste sour • acids are electrolytes (can conduct electricity in a solution) • acids are corrosive • acids react with indicators to produce a predictable color change Acid • substance that produces hydrogen ions (H+) in solution

  9. Five properties of bases: • in undissolved state, many bases are crystalline solid • in solution, bases feel slippery • bases have a bitter taste • strong bases are corrosive • bases react with indicators Base substance that produces hydroxide ions (OH-) in solution; also accepts H+ from acids

  10. Indicator • organic compound that changes color in the presence of acid or base Ex. litmus paper • Neutralization • chemical reaction between an acid and a base in a water solution which results in formation of salt and water • Salt • compound formed when negative ions of an acid combine with positive ions from a base

  11. Strength of Acids and Bases

  12. The strength of an acid or base depends on how many acid or base particles dissociate into ions in water. Strong acid • ionizes almost completely in water Weak acid • only partly ionizes in solution Strong base • dissociates completely in solution Weak base • does not completely dissociate

  13. * it is possible to have dilute solutions of strong acids and bases, as well as concentrated solutions of weak acids and bases.

  14. 0 1 2 3 4 5 6 7 8 9 10 11 12 13 14 pH • measure of concentration of H+ ions in a solution or how acidic or basic it is pH scale typically ranges from 0 – 14 ACIDIC BASIC NEUTRAL WEAK WEAK STRONG STRONG

  15. Chemical Bonds And Equation

  16. Types Of Chemical Bonds

  17. Compound • substance made of the combined atoms of two or more elements. Chemical formula • tells what elements a compound contains and the exact number of the atoms of those elements

  18. Superscript • represents oxidation # or how many electrons has gained or lost 2H2O SO42- Coefficient • represents the # of units of each substance Subscripts • represents # of atoms in a molecule of a particular element Atoms form compounds to become chemically stable. An atom is chemically stable when the outer energy level is complete, or full.

  19. https://www.youtube.com/watch?v=QXT4OVM4vXI&t=5s Chemical bond • force that holds together the atoms in a substance ION • positive or negatively charged atom

  20. Writing Formulas and Naming Compounds

  21. Binary compound • compound composed of two elements Oxidation number • positive or negative number (on PTable) which indicates how many electrons an element has gained, lost or shared when bonding with another atom. * When writing a formulas for binary ionic compounds, it is important to remember that compounds formed have a net charge of zero.

  22. Polyatomic Ions a positively or group of atoms negatively charged covalently bonded • The prefix poly means “many”, so the term polyatomic means “having many atoms”

  23. Hydrate • a compound that has water chemically attached to its ions and written into chemical formula. Covalent compounds • can form more than one compound with each other. Scientist use Greek prefixes to indicate # of atoms of each element in binary compound.

  24. Chemical Reactions

  25. Chemical reaction - a reaction in which one or more are changed to new substances Reactants - substances that are about to react Produced ReactantsProducts Products - new substances produced Law of Conversation of Mass • total starting mass of all reactants equals the total final mass all products.

  26. Chemical equation - uses chemical formulas and symbols to describe a chemical reaction and the product it produces (see below)

  27. Coefficients • #’s which represents the number of units of each substance in a rxn 4Al (s) + 3O2 (g)2Al2O3 Subscripts • #’s which represent the number of atoms in a molecule of a particular element

  28. BALANCING CHEMICAL EQUATIONS

  29. Balanced chemical equations • have the same number of atoms of each element on both sides of equation * When balancing chemical equation NEVER change the subscripts, instead change the coefficient in front of the compounds needing balanced.

  30. Steps to Balancing a Chemical Equation Step 1: Write a chemical equation for the reaction using formulas and symbols ­­– make sure reactants are on left side and products on right. Step 2: Count the atoms in reactants and products. Step 3: Choose coefficients that balanced the equation. HINT: Generally, if there is an even # of an element on one side and an odd on the other side, place a 2 in front of compound containing odd number of atoms.

  31. Step 4: Recheck the numbers of each atom on both sides of and adjust coefficients if necessary – remember NEVER change subscripts. Ex. 2NaBr + Cl2 2NaCl + Br2

  32. CHEMICAL RXNS – TYPES, RATES AND ENERGY

  33. Synthesis reaction - reaction where two or more substances combine to form another substance Decomposition reaction - reaction where one substance breaks down, or decomposes, into two or more simpler substances A+B AB AB A+B

  34. Double – displacement reaction - reaction that results in a precipitate, water or gas when a positive ion of one compound swaps with another positive ion of another compound. AB + CD AC + BD Single – displacement reaction - reaction in which one element replaces another in a compound A + B AC + B or A + BC AB + C

  35. Chemical reactions involve energy exchange Exothermic reactions Endothermic Reactions reaction in which energy reaction in which heat is released in front of heat energy is absorbed Ex. burning wood, fireworks Ex. Chemical Ice packs explode photosynthesis

  36. Catalyst • speeds up a chemical reaction without itself being permanently changed Inhibitor • prevents or slows a chemical reaction or interferes with the catalyst

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