We think you have liked this presentation. If you wish to download it, please recommend it to your friends in any social system. Share buttons are a little bit lower. Thank you!
Presentation is loading. Please wait.
Published byJohn Aron Carpenter
Modified over 4 years ago
Properties of Acids ·Sour taste, Change color of dyes, Conduct electricity in solution, React with many metals, React with bases to form salts
Properties of Bases ·Bitter taste, Feel slippery, Change color of dyes, Conduct electricity in solution, React with acids to form salts
Arrhenius ·Acids: release H + or H 3 O + in solution ·Bases: release OH - in solution
Arrhenius ·Acid: HA --> H + + A - ·HCl --> H + + Cl - ·Base: MOH --> M + + OH - ·NaOH -->Na + + OH -
Bronsted-Lowry ·Acid: Proton donor ·Base: Proton Acceptor
Bronsted-Lowry ·HA + H 2 O --> H 3 O + + A - ·HI + H 2 O --> H 3 O + + I - ·Acid Base CA CB ·NH 3 + H 2 O --> NH 4 + + OH - ·Base Acid CA CB
Lewis Acid/Base ·Acid: Electron Acceptor ·Base: Electron Donor
Lewis Acid/Base ·H 3 N: + BF 3 --> H 3 N-BF 3 ·Base Acid Neutral
Common Names ·H + Hydrogen ion ·H 3 O + Hydronium ion ·H - Hydride ion ·OH - Hydroxide ion ·NH 3 Ammonia ·NH 4 + Ammonium ion
Amphoterism ·Can act like an acid or a base ·Can donate or accept protons
Define acids & bases by each of the three methods
Naming Acids ·All acids are H-anion ·If the anion is: ·-ides hydro___ic acids ·-ates ___ic acids ·-ites ___ous acids
Naming Bases ·Almost all bases are metal hydroxides ·Name by normal method ·Ammonia (NH 3 ) as well as many amines are bases
Strong Acids or Bases ·Strong acids or bases ionize 100 % in solution ·Weak acids or bases ionize <100 % in solution
Strong Acids ·HClO 4 Perchloric acid ·H 2 SO 4 Sulfuric acid ·HNO 3 Nitric acid ·HClHydrochloric acid ·HBrHydrobromic acid ·HIHydroiodic acid
Strong Bases ·All column I hydroxides ·Ca(OH) 2 Calcium hydroxide ·Sr(OH) 2 Strontium hydroxide ·Ba(OH) 2 Barium hydroxide
Name & give the formula for at least 4 each of strong acids & strong bases
Binary Acids ·Acids containing only 2 elements ·HClHydrochloric acid ·H 2 SHydrosulfuric acid
Ternary Acids ·Acids containing 3 elements ·H 2 SO 4 Sulfuric acid ·H 2 SO 3 Sulfurous acid ·HNO 3 Nitric acid
Monoprotic Acids ·Acids containing only one ionizable hydrogen ·HBr Hydrobromic acid ·HCNHydrocyanic acid ·HC 2 H 3 O 2 Acetic acid
Diprotic Acids ·Acids containing 2 ionizable hydrogens ·H 2 SO 4 Sulfuric acid ·H 2 SO 3 Sulfurous acid ·H 2 CO 3 Carbonic acid
Triprotic Acids ·Acids containing 3 ionizable hydrogens ·H 3 PO 4 Phosphoric acid ·H 3 PO 3 Phosphorus acid ·H 3 AsO 4 Arsenic acid
Polyprotic Acids ·Acids containing more than one ionizable hydrogens ·H 2 SO 4 Sulfuric acid ·H 4 SiO 4 Silicic acid ·H 2 CO 2 Carbonous acid
Monohydroxic Base ·A base containing only one ionizable hydroxide ·NaOHSodium hydroxide ·KOHPotassium hydro. ·LiOHLithium hydroxide
Neutralization Rxn ·A reaction between an acid & a base making salt & H 2 O ·HA (aq) + MOH (aq) MA (aq) + H 2 O (l)
Neutralization Rxn HCl (aq) + NaOH (aq) NaCl (aq) + H 2 O (l)
Drill: Identify: acid, base, CA, & CB HCO 3 - + H 2 O H 2 CO 3 + OH -
Work problems 1 – 6 on page 395
Titration ·A method of determining the concentration of one solution by reacting it with a standard solution ·M A V A = M B V B for monoprotics
Standard Solution ·A solution with known concentration
Titration ·When titrating acids against bases, the end point of the titration is at the equivalence point
Make Calculations ·Calculate the molarity of 25.0 mL HCl when it’s titrated to its equivalence point with 50.0 mL 0.200 M NaOH
Equivalence Point ·The point where the H + concentration is equal to the OH - concentration
Indicator ·An organic dye that changes color when the pH changes
Make Calculations ·Calculate the mL of 12.5 M HCl required to make 2.5 L of 0.200 M HCl
Molarity ·Moles of solute per liter of solution (M)
Normality ·Number of moles of hydrogen or hydroxide ions per liter of solution (N)
Titration Formula ·N A V A = N B V B ·Elliott’s Rule: ·# H M A V A = # OH M B V B
Make Calculations ·Calculate the molarity of 30.0 mL H 2 CO 3 when it’s titatrated to its equivalence point with 75.0 mL 0.200 M NaOH
Make Calculations ·Calculate the molarity of 40.0 mL H 3 PO 4 when it’s titatrated to its equivalence point with 30.0 mL 0.20 M Ba(OH) 2
Calculate the volume of 0.250 M HCl needed to titrate 50.00 mL 0.200 M NaOH to its equivalence point
Calculate the molarity 25.0 mL H 3 PO 4 that neutralizes 50.00 mL 0.200 M Ca(OH) 2 to its equivalence point
Drill: Calculate the volume of 0.10 M H 3 PO 4 that neutralizes 50.00 mL 0.200 M Ca(OH) 2 to its equivalence point
pH ·The negative log of the hydrogen or hydronium ion concentration ·pH = -log[H + ] ·pOH = -log[OH - ]
Calculate the pH of: 1) [H + ] = 0.040 M 2) [HCl] = 0.0025 M 3) [HBr] = 0.080 M
Calculate the pOH of: 1) [OH - ] = 0.030 M 2) [KOH] = 0.0025 M 3) [NaOH] = 4.0 x 10 -5 M
Titration Curve: Strong acid vs strong base
Titration Curve: Strong acid vs strong base; then weak acid vs strong base
Titration Curve: Strong base vs strong acid; then weak base vs strong acid
Acids and Bases.
Acids & Bases. 1. Properties of Acids and Bases: TasteTouch Reactions with Metals Electrical Conductivity Acidsour looks like water, burns, stings Yes-
ACIDS AND BASES CHAPTER : WHAT ARE ACIDS AND BASES? Objectives: To name acids and bases. To write formulas for acids and bases.
Modern Chemistry Chapter 14
Acids and Bases Chapter 19. Ions in Solution Aqueous solutions contain H + ions and OH - ions If a solution has more H + ions than OH - ions it is.
As temperature increases, the molecules velocity increases, increasing the pressure on the container.
I. Introduction to Acids & Bases Acids & Bases. A. Properties electrolytes turn litmus red sour taste react with metals to form H 2 gas slippery.
Acids, Bases & Salts Pre-AP Chemistry LFHS
ACIDS & BASES EQ: Why are some aqueous solutions acidic, others basic, and some neutral? What makes them that way? GPS: SC7. Students will characterize.
Properties of acids Electrolytes: conduct electricity React to form salts Change the color of an indicator Have a sour taste.
Unit 13 Marker Board Review Acids & Bases You need a marker board, marker, eraser, calculator, & periodic table.
Acids/Bases/Salts Properties. Common Acids Lacticsour milk Aceticvinegar Phosphorictart taste in soda Citriccitrus fruits Malicapples Tartaricgrapes Formicant.
1A + 2B 1C + 1D Calculate the equilibrium concentrations of each species when 150 mL 2.5 M A is mixed with mL 2.5 M B. K c = 2.0 x
I. Introduction to Acids & Bases
Acids, Bases and Salts.
Acids and Bases. Properties of Acids/Bases Acids are substances which… Bases are substances which…
1A + 1B 1C + 1D Calculate the equilibrium concentrations of each species when 150 ml 2.0 M A is mixed with ml 2.0 M B. K c = 0.25.
1 Some Properties of Acids þ Produce H + (as H 3 O + ) ions in water (the hydronium ion is a hydrogen ion attached to a water molecule) þ Taste sour þ.
Acids, Bases, and Salts Chapter Acids – Taste sour – React with metals to form H 2 gas – Will change the color of and acid-base indicator Turns.
© 2019 SlidePlayer.com Inc. All rights reserved.