Cave Chemistry. What cave formation needs: 1. Make a hole in the ground 2. Partially fill it with cool formations.

Slides:

Advertisements

Similar presentations

PreAP Chem Go over Ksp wkst Buffers What to expect on the test Homework.

Advertisements

Using Tables F & G.

Strong Acids/ Bases Strong Acids more readily release H+ into water, they more fully dissociate H2SO4  2 H+ + SO42- Strong Bases more readily release.

Equilibrium and Solubility 1.Solubility rules for common ions 2.Using the solubility product, K sp, to calculate solubility - molar solubility, gram solubility.

Ocean Acidification Scott Doney Woods Hole Oceanographic Institution.

Limiting Reactants & Percent Yield

CHEMICALS IN ACTION Thermal Decomposition Reactions.

Karst Chemistry I. Definitions of concentration units Molality m = moles of solute per kilogram of solvent Molarity [x]= moles of solute per kilogram.

Chemical Equilibrium and the Acidification of the Ocean A Chem 30 Lesson Jordan Sevenhuysen February 9 th, 2012.

Chem 1310: Introduction to physical chemistry Part 5: Buffers and solubility Peter H.M. Budzelaar.

THE RELATIONSHIP BETWEEN H2CO3* AND HCO3-

Lecture 14. Charge balance Sum of positive charges = sum of negative charges In natural waters: [H + ]+2[Ca 2+ ]+2[Mg 2+ ]+[Na + ]+[K + ]=[HCO 3 - ]+2[CO.

CHEMISTRY 2000 Topic #3: Thermochemistry and Electrochemistry – What Makes Reactions Go? Spring 2008 Dr. Susan Lait.

Lecture 51/31/05 Wednesday afternoon lab section Do pre-lab exercise 2 Hand in pre-lab 1 on Wed. Use pre-lab 1 values to do the calculations at the end.

Chem 1310: Introduction to physical chemistry Part 3: Equilibria Miscellaneous.

ALKALINITY Bicarbonate-carbonate 1. Alkalinity is… …the measure of the ability of a water to neutralize an acid. 2.

CHEMICAL INTERACTIONS INVESTIGATION 1: SUBSTANCES.

Chemical Equilibrium Unit 11. My Chemistry Presentation Chemical Reactions We usually think of chemical reactions as having a beginning and an end. reactants.

Acid Deposition. pH Scale 7 is neutral As numbers decrease, acidity increases As numbers increase, alkalinity increases.

Chem. 31 – 3/4 Lecture. Announcements I Exam 1 –Still Grading –Key Posted Next Lab Report Due: Cl lab report –Due next Wednesday –Must turn in in Excel.

H2O + CO2 H2CO3 H2CO3 (HCO3)- + H+ 1. Rainwater acidifies.

General Chemistry II Chemical Equilibrium for Gases and for Sparingly-Soluble Ionic Solids Lecture 2

Chapter 9 Chemical Equilibrium

Chapter 18: Chemical Equilibria Irreversible reactions: The reactants combine to form products and the reaction stops when the limiting reagent has been.

Saturated solution – no more solute will dissolve solubility product constant – equilibrium constant for ionic compounds that are only slightly soluble.

Gallery Walk problems. Consider the following reaction: I 2 (g) + Cl 2 (g)  2 ICl (g) K p = 25°C Calculate  G 25°C under the following.

Karst Chemistry II. Conductivity – Specific Conductance Conductance – the electrical conductivity of aqueous solution, and is directly related to the.

IX.Salts and Hydrolysis  Salts are simply ionic compounds.  Salts can be formed by: 1.A metal reacting with a non-metal. 2 Na (s) + Cl 2(g)  2 NaCl.

Solubility from K s. Calculate the solubility, in g L -1, of CaCO 3, given K s (CaCO 3 ) = 5 × M(CaCO 3 ) = 100 g mol –1. 1 Write the equilibrium.

Solubility Equilibria 16.6 AgCl (s) Ag + (aq) + Cl - (aq) K sp = [Ag + ][Cl - ]K sp is the solubility product constant MgF 2 (s) Mg 2+ (aq) + 2F - (aq)

To calculate the new pH, use the Henderson- Hasselbalch equation: 1141.

Chemistry 1011 Slot 51 Chemistry 1011 TOPIC Thermochemistry TEXT REFERENCE Masterton and Hurley Chapter 8.

EXPERIMENTAL YEILD IN THE REACTION Na 2 CO 3(aq) + CaCl 2(aq)  CaCO 3(aq) + 2 NaCl(s) OBJECTIVE : MASS OF CALCIUM CARBONATE PRODUCED DATA…THAT DAY IN.

Solubility Equilibria Solubility Product Constant, K sp Precipitation Complex Ions.

Common Ion Effect CH 3 COOH H + (aq) + CH 3 COO  (aq) pH of 0.1 M soln = Add 0.1 M CH 3 COONa: CH 3 COONa  Na + + CH 3 COO  (aq) pH = What happened.

Class average for Exam I 70. Fe(OH) 3 Fe 3+ (aq) + 3 OH - (aq) [Fe 3+ ][OH - ] 3 = 1.1 x [y][3y] 3 = 1.1 x If there is another source of.

1 Equilbrium Constant and EXTERNAL EFFECTS Formation of stalactites and stalagmites CaCO 3 (s) + H 2 O(liq) + CO 2 (g)  Ca 2+ (aq) + 2 HCO 3 - (aq)

Ely Mine Trip Be here by 8 am! – we should be back by 5pm Sunday at the latest Need: camping gear, warm clothes, clothes that can get messy! Field Notebook.

CHAPTER 17 - SOLUBILITY AND PRECIPITATION. Read intro on page 560 Dissolution CaCl 2(s) ↔ Ca +2 (aq) + 2 Cl - (aq) CaCl 2(s) ↔ Ca +2 (aq) + 2 Cl - (aq)Precipitation.

CH 17: Solubility and Complex-Ion Equilibria Renee Y. Becker CHM 1046 Valencia Community College 1.

Ch (Net Ionic Equations)

Solubility Product (K sp ) Everything dissolves in water to a point.

Heterogeneous Equilibria: A homogenous reaction is one in which all the substances are in the same state. A heterogeneous reaction is one in which all.

Percent Yield. Definitions The theoretical yield is the maximum amount of product that could be made from the reactants. The actual yield is the amount.

Pacific school of Engineering Sub: C.E.T-2 Topic: Chemical reaction Equilibrium Mayani Chintak Sudani Dhrutik Bhikadiya Hardik.

Weathering Process Rocks are classed as “dead”, hard and chemically inactive. Soils are considered to be “alive”, soft, porous and chemically active. They.

Storing carbon dioxide Learning objectives:  Describe the factors determining the relative solubility of a solute in aqueous and non aqueous solvents.

ΜΕΤΑΣΥΛΛΕΚΤΙΚΗ ΦΥΣΙΟΛΟΓΙΑ ΕΡΓΑΣΤΗΡΙΟ 3. Μετασυλλεκτική Εργ3-Λιοσάτου Γ.2 ΒΙΟΛΟΓΙΚΟΙ ΠΑΡΑΓΟΝΤΕΣ ΠΟΥ ΕΠΗΡΕΑΖΟΥΝ ΤΗ ΦΘΟΡΑ ΤΩΝ ΟΠΩΡΟΚΗΠΕΥΤΙΚΩΝ Αναπνοή Η λειτουργία.

Chemical Equilibrium Unit 11. My Chemistry Presentation Chemical Reactions We usually think of chemical reactions as having a beginning and an end. reactants.

pH calculations strong acids complete dissociation HA  H+ + A-

pH calculations strong acids complete dissociation HA  H+ + A-

Chem. 1B – 10/11 Lecture.

Calculating ΔHfθ from combustion data

Applications of Aqueous Equilibria

UNIT III Tutorial 10: Ksp Calculations

: Ka, Kb and the Conjugate Pair

5. [Ca2+] / [Ca]T = So, [Ca2+] = 0.75 x = M

Cave Chemistry.

اثرات گرمايش جهاني تغييرات آب و هوا، تأثيرات عميق و شديدي بر بسياري از عوامل اساسي موثر بر سلامت از جمله : آب، غذا، هوا و محيط زيست دارد كه اين مورد خود.

Ocean Acidification CO2 CO2 CO2 Carbonic Acid

CH 17: Solubility and Complex-Ion Equilibria

Cave Chemistry.

Cave Chemistry.

Cave Chemistry Tronconas.

Percent Yield A batting average is a measure of how often a batter gets a hit as a percentage of how many times he tries. In chemistry, the percent yield.

O2 O2 CH4 H2O CO2 H2O2 CH3OH O2 O2 CH4 H2O CO2 H2O2 CH3OH O2 O2 CH4

pH calculations strong acids complete dissociation HA  H+ + A-

AP chemistry Big idea 1 Titration of Milk.

2.4 Chemical Reactions.

Presentation transcript:

Cave Chemistry

What cave formation needs: 1. Make a hole in the ground 2. Partially fill it with cool formations

Cave Chemistry CaCO 3 (s)  Ca 2+ (aq) + CO 3 2- (aq) K sp (CaCO 3 ) = 4.8 x Calculate solubility in mg/L: Actual solubility: 80 mg/L Why???

Effect of [CO 2 ]. What should happen as [CO 2 ] increases? CaCO 3 (s)  Ca 2+ (aq) + CO 3 2- (aq) CO 2 + H 2 O  H 2 CO 3 H 2 CO 3  HCO H + Ka 1 (H 2 CO 3 ) = 4.2 x HCO 3 -  CO H + Ka 2 (HCO 3 - ) = 4.8 x

CaCO 3 (s)  Ca 2+ (aq) + CO 3 2- (aq) CO 2 + H 2 O  H 2 CO 3 H 2 CO 3  HCO H + Ka 1 (H 2 CO 3 ) = 4.2 x HCO 3 -  CO H + Ka 2 (HCO 3 - ) = 4.8 x The Key Reaction is:

So: 1. Formation of the big hole

So: 2. Making those formations