SOLUBILITY PRODUCT (K sp ) Slightly Soluble Salts & ph AND BUFFERS (Part Two)
|
|
- Clement Cannon
- 6 years ago
- Views:
Transcription
1 SOLUBILITY PRODUCT (K sp ) Slightly Soluble Salts & ph AND BUFFERS (Part Two) ADEng. PRGORAMME Chemistry for Engineers Prepared by M. J. McNeil, MPhil. Department of Pure and Applied Sciences Portmore Community College Main Campus
2 LECTURE OBJECTIVES Use the solubility product constant, K sp, concept. Calculate the K sp of compounds. Have an understanding of the common-ion effect. Predict the formation of a precipitate.
3 SOLUBILITY OF IONIC SALTS The solubility of ionic salts varies considerably. Most nitrates are very soluble, while phosphates and may other salts of transition metal ions are often insoluble.
4 SOLUBILITY AND TEMPERATURE The solubility of ionic salts varies considerately with the temperature. Some such as KNO 3 have a wide solubility range. The solubility of NaCl in water varies only slightly. Define saturation, supersaturation and undersaturation.
5 SOLUBILITY Table salt is water soluble, but the addition of more and more salt the dissolution decreases until it ceases. Why? Atomic level - NaCl (ionic bonds) grain will break apart into their ions and ushered away by the water. Result - A net increase in the [Na + (aq)] and [Cl - (aq)] in the solution. With the increase increase increase the amount of ions, eventually no more ions can be added, and it will be pushed back to the solid form of salt. Solution = Solute and Solvent (solid) Breaking apart the solid solute into its ions by dissolving it in solution. Solid form (solute) (on the LHS) Aqueous form in ionic form (on the RHS) An equilibrium is achieved in a solution since the reaction is reversible. The compound thus have its unique equilibrium constant and we call this.
6 THE SOLUBILITY PRODUCT CONSTANT, K sp Many important ionic compounds are only slightly soluble in water and equations are written to represent the equilibrium between the compound and the ions present in a saturated aqueous solution. K sp is way of measuring the solubility of any salt. The solubility product constant, K sp, is the product of the concentrations of the ions involved in a solubility equilibrium, each raised to a power equal to the stoichiometric coefficient of that ion in the chemical equation for the equilibrium. Substances that forms a satuarated solution will have a K sp.
7 SOLUBILITY PRODUCT E.g. Copper(II) sulphate On adding more and more CuSO 4, the crystals - not just sitting there, but The rate of dissolution = rate of crystallization (precipitation) in a solution equilibrium. How do we measure whether the reaction goes to the RHS or LHS = equilibrium constant of the substance being dissolved in water.
8 SOLUBILITY EQUILIBRIUM In saturated solutions dynamic equilibrium exists between undissolved solids and ionic species in solutions. Solids continue to dissolve and ionpairs continue to form solids. The rate of dissolution process is equal to the rate of precipitation. General expression: Always take the solid [LHS] and break it down into its constituent ions [RHS]. M m X n (s) mm n+ (aq) + nx m- (aq) The ions, M n+ (aq) and X m- (aq) will remain constant over time and an equilibrium constant expression can be derived that can describe the solution at a given temperature. Solubility product, K sp = [M n+ ] m [X m- ] n If the molar solubility of the ions, [M n+ (aq)] and [X m- (aq)] are altered, the Ksp value can still be determined just before precipitation. Large Ksp have high solubility (NaCl) Small Ksp have low solubility
9 Example 1 SOLUBILITY EQUILIBRIUM EQUATION AND K sp CaF 2 (s) Ca 2+ (aq) + 2 F - (aq) K sp = [Ca 2+ ][F - ] 2 K sp = 5.3 x 10-9 units Example 2 As 2 S 3 (s) 2 As 3+ (aq) + 3 S 2- (aq) K sp = [As 3+ ] 2 [S 2- ] 3 K sp = 4.4 x units
10 SOLUBILITY PRODUCT CONSTANTS AT 25 o C
11 K sp AND MOLAR SOLUBILITY CALCULATIONS The solubility product constant is related to the solubility of an ionic solute, but K sp and molar solubility - the molarity of a solute in a saturated aqueous solution - are not the same thing. Calculating solubility equilibria fall into two categories: determining a value of K sp from experimental data calculating equilibrium concentrations when K sp is known. SOLUBILITY (SOLID) AND SOLUBILITY PRODUCTS (IONS)
12 CALCULATING K sp FROM MOLAR SOLUBILITY 1. Determine the K sp of copper(ii) bromate. Use the ICE table: Cu(BrO 3 ) 2 Cu 2+ 2BrO 3 - Initial Change - +x +2x Equilibrium - +x +2x Cu 2+ K sp = [Cu 2+ ] [BrO 3- ] K sp = x. 2x K sp = 2x 2 units 12
13 CALCULATING K sp FROM MOLAR SOLUBILITY 2. It is found that 1.2 x 10-3 mol of lead (II) iodide, PbI 2, dissolves in 1.0 dm 3 of aqueous solution at 25 o C. What is the K sp at this temperature? PbI 2 (s) Pb 2+ (aq) + 2 I - (aq) K sp = [Pb 2+ ] [I - ] 2 For every lead iodide that dissolves, there is one lead ion and 2 iodide ions. Therefore, [Pb 2+ ] = 1.2x10-3 units [I - ] = 2.4x10-3 units K sp = (1.2x10-3 ) (2.4x10-3 ) 2 K sp = 6.9 x 10-9 units So we must find the concentrations of each ion and then solve for K sp.
14 CALCULATING MOLAR SOLUBILITY FROM K sp 3. Calculate the concentration of [Ag + ] and [Cl - ] in a saturated solution of silver chloride. The K sp for silver chloride : K sp = 1.8x K sp = [Ag + ] [Cl - ] = 1.8x10-10 Let x = [Ag + ] = [Cl - ] using I.C.E. Substitute into the K sp expression x 2 = 1.8x10-10 x = 1.8x10-10 x = 1.34 x 10-5 units [Ag + ] = [Cl - ] = 1.34 x 10-5 units
15 CALCULATING MOLAR SOLUBILITY FROM K sp 4. Calculate the molar solubility of silver chromate, Ag 2 CrO 4, in water from K sp = 1.1x for Ag 2 CrO 4. Ag 2 CrO 4 (s) 2 Ag + + CrO 2-4 K sp = [Ag + ] 2 [CrO 2-4 ] K sp = 1.1x10-12 Let x = [CrO 2-4 ] 2x = [Ag + ] using I.C.E. Substitute into the K sp expression 4x 3 = 1.1x10-12 x = 3 1.1x10-12 /4 x = [CrO 2-4 ] = 6.5 x10-5 units 2x = [Ag + ] = 1.30 x 10-4 units
16 FACTORS THAT AFFECT SOLUBILITY Temperature Solubility generally increases with temperature; Common ion effect Common ions reduce solubility; Salt effect This slightly increases solubility; ph of solution ph affects the solubility of ionic compounds in which the anions are conjugate bases of weak acids; Formation of complex ion The formation of complex ion increases solubility.
17 THE COMMON ION EFFECT IN SOLUBILITY EQUILIBRIA The precipitate of a solute on addition of another solution which has an ion in common with the solute is referred to as the common ion effect. The solubility of a slightly soluble ionic compound is lowered when a second solute that furnishes a common ion is added to the solution. The common ion effect also affects solubility equilibria. Le Châtelier s principle is followed for the shift in concentration of products and reactants upon addition of either more products or more reactants to a solution.
18 THE COMMON ION EFFECT E.g. Consider the following solubility equilibrium: AgCl(s) Ag + (aq) + Cl - (aq); K sp = 1.6 x ; The solubility of AgCl is 1.3 x 10-5 mol/l at 25 o C. If NaCl is added, equilibrium shifts left due to increase in [Cl - ] and some AgCl will precipitate out. AgCl(s) Ag + (aq) + Cl - (aq); NaCl(s) Na + (aq) + Cl - (aq); For example, if [Cl - ] = 1.0 x 10-2 M, Solubility of AgCl = (1.6 x )/(1.0 x 10-2 ) = 1.6 x 10-8 mol/l (Solubility decreases
19 THE COMMON ION EFFECT BaSO 4 (s) Ba 2+ (aq) + SO 42 (aq) Na 2 SO 4 (s) 2Na + (aq) + SO 42 (aq) The presence of the sodium sulphate increases the concentration of SO 4 2- ions in the mixture. An increase in the concentration of [SO 42 ] (common ion) would cause a decrease in the [Ba 2+ ] ions to keep the solubility product at a constant value. The equilibrium will thus shift to counteract the stress imposed and reduce the solubility of BaSO 4. The addition of the sulphate ions results in the precipitation of the solid BaSO 4.
20 THE COMMON ION EFFECT CALCULATIONS 1. What is the solubility of Ag 2 CrO 4 in 0.10 M K 2 CrO 4? K sp = 1.1x10-12 for Ag 2 CrO 4. Let 2x = Ag + and CrO 4 2- = 10-1 (4x 2 )(10-1 ) = 1.1 x x 2 = 1.1 x / x 2 = 1.1 x x = 1.66 x 10-6 [Ag + ] = 2x = 3.32 x 10-6 Comparison of solubility of Ag 2 CrO 4 In pure water: 6.5 x 10-5 M In 0.10 M K 2 CrO 4 : 1.7 x 10-6 M The common ion effect!!
21 DETERMINING WHETHER PRECIPITATION OCCURS Q ip is the ion product reaction quotient and is based on initial conditions of the reaction. Q ip is ion product expressed in the same way as K sp for a particular system. To predict if a precipitation occurs: Q ip can then be compared to K sp!!!!!!!! - Precipitation should occur if Q ip > K sp (precipitate). - Precipitation cannot occur if Q ip < K sp (no precipitate). - A solution is just saturated if Q ip = K sp (unsaturated solution). Q sp and Q ip are termed the ion product expressed in the same way as K sp for a particular system.
22 PREDICTING PRECIPITATION 1. The concentration of calcium ion in blood plasma is M. If the concentration of oxalate ion is 1.0x10-7 M, do you expect calcium oxalate to precipitate? K sp = 2.3x10-9. CaC 2 O 4 Ca 2+ (aq) + C 2 O 4 2- (aq) [Ca 2+ ] [C 2 O 4 2- ] = 2.3x10-9 Three steps: 1. Determine the initial concentrations of ions. (Put both in the K sp formula) 2. Evaluate the reaction quotient Q ip. 3. Compare Q ip with K sp. If Q ip > K sp, then it will precipitate.
23 PREDICTING PRECIPITATION In applying the precipitation criteria, the effect of dilution when solutions are mixed must be considered. E.g ml of M Pb(NO 3 ) 2 is added to 30.0 ml of 0.10 M NaCl. Predict if precipitate of PbCl 2 will form. (Ksp for PbCl 2 = 1.6 x 10-5 ) Calculation: [Pb 2+ ] = (20.0 ml x M)/(50.0 ml) = M [Cl - ] = (30.0 ml x 0.10 M)/(50.0 ml) = M Q sp = [Pb 2+ ][Cl - ] 2 Q sp = (0.010 M)(0.060 M) 2 Q sp = 3.6 x 10-5 Q ip can then be compared to K sp!!!!!!!! To predict if a precipitation occurs: - Precipitation should occur if Q ip > K sp (precipitate). Q sp > K sp precipitate of PbCl 2 will form. - Precipitation cannot occur if Q ip < K sp (no precipitate). - A solution is just saturated if Q ip = K sp (unsaturated solution).
24 PRACTICAL APPLICATIONS OF SOLUBILITY EQUILIBRIA Qualitative Analyses Isolation and identification of cations and/or anions in unknown samples Synthesis of Ionic Solids of commercial interest. Selective Precipitation based on K sp Separation and identification of cations, such as Ag +, Ba 2+, Cr 3+, Fe 3+, Cu 2+, etc. can be carried out based on their different solubility and their ability to form complex ions with specific reagents, such as HCl, H 2 SO 4, NaOH, NH 3, and others. Separation and identification of anions, such as Cl -, Br -, I -, SO 4 2-, CO 3 2-, PO 4 3-, etc., can be accomplished using reagents such as AgNO 3, Ba(NO 3 ) 2 under neutral or acidic conditions.
25
26 SELECTIVE PRECIPITATION (Mixtures of Metal Ions) Use a reagent whose anion forms a precipitate with only one or a few of the metal ions in the mixture. Example: Solution contains Ba 2+ and Ag + ions. (Double displacement reaction) Adding NaCl will form a precipitate with Ag + (AgCl), while still leaving Ba 2+ in solution. Read up on limitations of K sp.
27 ph and BUFFERS 1. What is meant by a buffer solution? 2. Explain how buffer solutions control ph? 3. Calculate the ph of a specific buffer. 4. Discuss the importance of buffers in biological systems and industrial processes.
28 BUFFER SOLUTIONS Buffers are solutions which resists changes in ph when small quantities of acid of alkali are added Acidic Buffer (ph < 7) made from a weak acid + its sodium or potassium salt (conjugate base or a salt of the weak acid) ethanoic acid sodium ethanoate Alkaline Buffer (ph > 7) made from a weak base + its chloride (conjugate acid or a salt of the weak base ammonia ammonium chloride
29 USES OF BUFFER SOLUTIONS In biological systems (saliva, stomach, and blood) it is essential that the ph stays constant in order for any processes to work properly. e.g. If the ph of blood varies by 0.5 it can lead to unconsciousness and coma. ph affects the structure and function of enzymes. Many household and cosmetic products need to control their ph values. Buffer solutions counteract the alkalinity of the soap and prevent irritation. Washing powder and eye drops. Standardising ph meters
30 ACTION OF BUFFER SOLUTION It is essential to have a weak acid for an equilibrium to be present so that ions can be removed and produced. The dissociation is small and there are few ions. CH 3 COOH(aq) CH 3 COO (aq) + H + (aq) relative concs. HIGH LOW LOW NB A strong acid can t be used as it is fully dissociated and cannot remove H + (aq) HCl(aq) > Cl (aq) + H + (aq) Adding acid Any H + is removed by reacting with CH 3 COO ions to form CH 3 COOH via the equilibrium. Unfortunately, the concentration of CH 3 COO is small and only a few H + can be mopped up. A much larger concentration of CH 3 COO is required. To build up the concentration of CH 3 COO ions, sodium ethanoate is added, which dissociates completely. CH 3 COO Na + (aq) > CH 3 COO (aq) + Na + (aq) relative concs. LOW HIGH HIGH
31 ACTION OF BUFFER SOLUTION We have now got an equilibrium mixture which contains a high concentration of both the undissociated weak acid, CH 3 COOH(aq), and its conjugate base, CH 3 COO (aq). CH 3 COOH(aq) CH 3 COO (aq) + H + (aq) relative concs. HIGH LOW LOW CH 3 COO Na + (aq) CH 3 COO (aq) + Na + (aq) relative concs. LOW HIGH HIGH This adds OH ions Adding alkali These react with the small concentration of H + ions: H + (aq) + OH (aq) H 2 O(l) Removal of H + from the weak acid equilibrium means that more CH 3 COOH will dissociate to form ions to replace those being removed. CH 3 COOH(aq) CH 3 COO (aq) + H + (aq) As the added OH ions remove the H + from the weak acid system, the equilibrium moves to the right to produce more H + ions. (There needs to be a large concentration of undissociated acid molecules to be available)
32 BUFFER SOLUTIONS - IDEAL CONC. The concentration of a buffer solution is important If the concentration is too low, there won t be enough CH 3 COOH and CH 3 COO to cope with the ions added. Summary For a buffer solution one needs... large [CH 3 COOH(aq)] - for dissociating into H + (aq) when alkali is added weak acid (equilibrium shifts to the right) large [CH 3 COO (aq)] - for removing H + (aq) as it is added conjugate base (equilibrium shifts to the left) `This situation can t exist if only acid is present; a mixture of the acid and salt is used. The weak acid provides the equilibrium and the large CH 3 COOH(aq) concentration. The sodium salt provides the large CH 3 COO (aq) concentration. One uses a WEAK ACID + its SODIUM OR POTASSIUM SALT
33 ACTION OF ALKALINE BUFFERS Alkaline buffer Very similar but is based on the equilibrium surrounding a weak base; AMMONIA NH 3 (aq) + H 2 O(l) OH (aq) + NH 4+ (aq) relative concs. HIGH LOW LOW but one needs ; a large conc. of OH (aq) to react with any H + (aq) added a large conc of NH 4+ (aq) to react with any OH (aq) added There is enough NH 3 to act as a source of OH but one needs to increase the concentration of ammonium ions by adding an ammonium salt. Use AMMONIA (a weak base) + AMMONIUM CHLORIDE (one of its salts)
34 CALCULATING THE ph OF AN ACIDIC BUFFER SOLLUTION Whenever you are asked to calculate the ph of a buffer solution, ALWAYS USE THE Henderson-Hasselbach equation ph = pk a + log 10 [salt]/[acid] Calculate the ph of a buffer whose [HA] is 0.1 mol dm -3 and [A ] of 0.1 mol dm -3. The K a of the weak acid HA is 2 x 10-4 mol dm -3
35 CALCULATING THE ph OF AN ACIDIC BUFFER SOLLUTION (Alternative calculation to Henderson-Hasselbalch equation use) Question One Calculate the ph of a buffer whose [HA] is 0.1 mol dm -3 and [A ] of 0.1 mol dm -3. The K a of the weak acid HA is 2 x 10-4 mol dm -3 K a = [H + (aq)] [A (aq)] [HA(aq)]
36 CALCULATING THE ph OF AN ACIDIC BUFFER SOLLUTION Calculate the ph of a buffer whose [HA] is 0.1 mol dm -3 and [A ] of 0.1 mol dm -3. K a = [H + (aq)] [A (aq)] [HA(aq)] re-arrange [H + (aq)] = [HA(aq)] x K a [A (aq)]
37 CALCULATING THE ph OF AN ACIDIC BUFFER SOLLUTION Calculate the ph of a buffer whose [HA] is 0.1 mol dm -3 and [A ] of 0.1 mol dm -3. K a = [H + (aq)] [A (aq)] [HA(aq)] re-arrange [H + (aq)] = [HA(aq)] x K a [A (aq)] from information given [A ] = 0.1 mol dm -3 [HA] = 0.1 mol dm -3
38 Calculating the ph of an acidic buffer solution Calculate the ph of a buffer whose [HA] is 0.1 mol dm -3 and [A ] of 0.1 mol dm -3. K a = [H + (aq)] [A (aq)] [HA(aq)] re-arrange [H + (aq)] = [HA(aq)] x K a [A (aq)] from information given [A ] = 0.1 mol dm -3 [HA] = 0.1 mol dm -3 If the K a of the weak acid HA is 2 x 10-4 mol dm -3. [H + (aq)] = 0.1 x 2 x 10-4 = 2 x 10-4 mol dm
39 CALCULATING THE ph OF AN ACIDIC BUFFER SOLLUTION Calculate the ph of a buffer whose [HA] is 0.1 mol dm -3 and [A ] of 0.1 mol dm -3. K a = [H + (aq)] [A (aq)] [HA(aq)] re-arrange [H + (aq)] = [HA(aq)] x K a [A (aq)] from information given [A ] = 0.1 mol dm -3 [HA] = 0.1 mol dm -3 If the K a of the weak acid HA is 2 x 10-4 mol dm -3. [H + (aq)] = 0.1 x 2 x 10-4 = 2 x 10-4 mol dm ph = - log 10 [H + (aq)] = 3.699
40 CALCULATING THE ph OF AN ACIDIC BUFFER SOLLUTION Question Two Calculate the ph of the solution formed when 500cm 3 of 0.1 mol dm -3 of weak acid HX is mixed with 500cm 3 of a 0.2 mol dm -3 solution of its salt NaX. K a = 4 x 10-5 mol dm -3. Henderson-Hasselbach equation ph = pk a + log 10 [salt]/[acid] ph = 4.699
41 ASSIGNMENT Discuss the importance of buffers in biological and industrial processes. Include reference to blood buffer systems such as hydrogencaronale, phosphate and amino acid systems (zwitterions), enzyme catalysed reactions and the food processing industry.
Chapter 15 Additional Aspects of
Chemistry, The Central Science Chapter 15 Additional Aspects of Buffers: Solution that resists change in ph when a small amount of acid or base is added or when the solution is diluted. A buffer solution
More informationChap 17 Additional Aspects of Aqueous Equilibria. Hsu Fu Yin
Chap 17 Additional Aspects of Aqueous Equilibria Hsu Fu Yin 1 17.1 The Common-Ion Effect Acetic acid is a weak acid: CH 3 COOH(aq) H + (aq) + CH 3 COO (aq) Sodium acetate is a strong electrolyte: NaCH
More informationUnit 3: Solubility Equilibrium
Unit 3: Chem 11 Review Preparation for Chem 11 Review Preparation for It is expected that the student understands the concept of: 1. Strong electrolytes, 2. Weak electrolytes and 3. Nonelectrolytes. CHEM
More informationUnit 3: Solubility Equilibrium
Unit 3: Chem 11 Review Preparation for Chem 11 Review Preparation for It is expected that the student understands the concept of: 1. Strong electrolytes, 2. Weak electrolytes and 3. Nonelectrolytes. CHEM
More informationChapter 18. Solubility and Complex- Ionic Equilibria
Chapter 18 Solubility and Complex- Ionic Equilibria 1 The common ion effect Le Chatelier Why is AgCl less soluble in sea water than in fresh water? AgCl(s) Ag + + Cl Seawater contains NaCl 2 Problem: The
More informationChapter 17 Additional Aspects of
Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 17 Additional Aspects of John D. Bookstaver St. Charles Community College Cottleville,
More informationCh. 14/15: Acid-Base Equilibria Sections 14.6, 14.7, 15.1, 15.2
Ch. 14/15: Acid-Base Equilibria Sections 14.6, 14.7, 15.1, 15.2 Creative Commons License Images and tables in this file have been used from the following sources: OpenStax: Creative Commons Attribution
More informationChapter 17. Additional Aspects of Equilibrium
Chapter 17. Additional Aspects of Equilibrium Sample Exercise 17.1 (p. 726) What is the ph of a 0.30 M solution of acetic acid? Be sure to use a RICE table, even though you may not need it. (2.63) What
More informationOperational Skills. Operational Skills. The Common Ion Effect. A Problem To Consider. A Problem To Consider APPLICATIONS OF AQUEOUS EQUILIBRIA
APPLICATIONS OF AQUEOUS EQUILIBRIA Operational Skills Calculating the common-ion effect on acid ionization Calculating the ph of a buffer from given volumes of solution Calculating the ph of a solution
More informationSolubility Equilibria. Dissolving a salt... Chem 30S Review Solubility Rules. Solubility Equilibrium: Dissociation = Crystalization
Chem 30S Review Solubility Rules Solubility Equilibria Salts are generally more soluble in HOT water(gases are more soluble in COLD water) Alkali Metal salts are very soluble in water. NaCl, KOH, Li 3
More informationSolubility Equilibrium. Solutions. Dissociation Equations. April/May Chemistry 30
Solubility Equilibrium Chemistry 30 Solutions Mixture containing two or more components, but looks like one homogeneous substance Solute: dissolved substance Solvent: dissolving substance In this course:
More informationChapter 17: Additional Aspects of Aqueous equilibria. Common-ion effect
Chapter 17: Additional Aspects of Aqueous equilibria Learning goals and key skills: Describe the common ion effect. Explain how a buffer functions. Calculate the ph of a buffer solution. Calculate the
More informationChapter 17. Additional Aspects of Aqueous Equilibria 蘇正寬 Pearson Education, Inc.
Chapter 17 Additional Aspects of Aqueous Equilibria 蘇正寬 chengkuan@mail.ntou.edu.tw Additional Aspects of Aqueous Equilibria 17.1 The Common-Ion Effect 17.2 Buffers 17.3 Acid Base Titrations 17.4 Solubility
More informationMore About Chemical Equilibria
1 More About Chemical Equilibria Acid-Base & Precipitation Reactions Chapter 15 & 16 1 Objectives Chapter 15 Define the Common Ion Effect (15.1) Define buffer and show how a buffer controls ph of a solution
More informationChapter 17. Additional Aspects of Aqueous Equilibria. Lecture Presentation. James F. Kirby Quinnipiac University Hamden, CT
Lecture Presentation Chapter 17 Additional Aspects of James F. Kirby Quinnipiac University Hamden, CT Effect of Acetate on the Acetic Acid Equilibrium Acetic acid is a weak acid: CH 3 COOH(aq) H + (aq)
More informationChapter 17. Additional Aspects of Equilibrium
Chapter 17. Additional Aspects of Equilibrium 17.1 The Common Ion Effect The dissociation of a weak electrolyte is decreased by the addition of a strong electrolyte that has an ion in common with the weak
More informationAP Chemistry Table of Contents: Ksp & Solubility Products Click on the topic to go to that section
Slide 1 / 91 Slide 2 / 91 AP Chemistry Aqueous Equilibria II: Ksp & Solubility Products Table of Contents: K sp & Solubility Products Slide 3 / 91 Click on the topic to go to that section Introduction
More informationSolubility and Complex-ion Equilibria
Solubility and Complex-ion Equilibria Contents and Concepts Solubility Equilibria 1. The Solubility Product Constant 2. Solubility and the Common-Ion Effect 3. Precipitation Calculations 4. Effect of ph
More informationSOLUBILITY REVIEW QUESTIONS
Solubility Problem Set 1 SOLUBILITY REVIEW QUESTIONS 1. What is the solubility of calcium sulphate in M, g/l, and g/100 ml? 2. What is the solubility of silver chromate? In a saturated solution of silver
More informationEquilibri acido-base ed equilibri di solubilità. Capitolo 16
Equilibri acido-base ed equilibri di solubilità Capitolo 16 The common ion effect is the shift in equilibrium caused by the addition of a compound having an ion in common with the dissolved substance.
More informationReview 7: Solubility Equilibria
Review 7: Solubility Equilibria Objectives: 1. Be able to write dissociation equations for ionic compounds dissolving in water. 2. Given Ksp, be able to determine the solubility of a substance in both
More informationWe CAN have molecular solutions (ex. sugar in water) but we will be only working with ionic solutions for this unit.
Solubility Equilibrium The Basics (should be mostly review) Solubility is defined as the maximum amount of a substance which can be dissolved in a given solute at a given temperature. The solubility of
More informationAcid-Base Equilibria and Solubility Equilibria Chapter 17
PowerPoint Lecture Presentation by J. David Robertson University of Missouri Acid-Base Equilibria and Solubility Equilibria Chapter 17 The common ion effect is the shift in equilibrium caused by the addition
More informationChapter 19. Solubility and Simultaneous Equilibria p
Chapter 19 Solubility and Simultaneous Equilibria p. 832 857 Solubility Product ) The product of molar concentrations of the constituent ions, each raised ot the power of its stoichiometric coefficients
More informationChemistry 102 Chapter 17 COMMON ION EFFECT
COMMON ION EFFECT Common ion effect is the shift in equilibrium caused by the addition of an ion that takes part in the equilibrium. For example, consider the effect of adding HCl to a solution of acetic
More informationChapter 17. Additional Aspects of Equilibrium
Chapter 17. Additional Aspects of Equilibrium 17.1 The Common Ion Effect The dissociation of a weak electrolyte is decreased by the addition of a strong electrolyte that has an ion in common with the weak
More informationUNIT III: SOLUBILITY EQUILIBRIUM YEAR END REVIEW (Chemistry 12)
I. Multiple Choice UNIT III: SOLUBILITY EQUILIBRIUM YEAR END REVIEW (Chemistry 12) 1) Which one of the following would form an ionic solution when dissolved in water? A. I 2 C. Ca(NO 3 ) 2 B. CH 3 OH D.
More informationChapter 15 - Applications of Aqueous Equilibria
Neutralization: Strong Acid-Strong Base Chapter 15 - Applications of Aqueous Equilibria Molecular: HCl(aq) + NaOH(aq) NaCl(aq) + H 2 O(l) SA-SB rxn goes to completion (one-way ) Write ionic and net ionic
More informationChapter 4. Reactions in Aqueous Solution. Lecture Presentation. John D. Bookstaver St. Charles Community College Cottleville, MO
Lecture Presentation Chapter 4 in Solution 2012 Pearson Education, Inc. John D. Bookstaver St. Charles Community College Cottleville, MO Properties of Solutions Solute: substance in lesser quantity in
More informationSchool of Chemistry, Howard College Campus University of KwaZulu-Natal CHEMICAL ENGINEERING CHEMISTRY 2 (CHEM171)
School of Chemistry, Howard College Campus University of KwaZulu-Natal CHEMICAL ENGINEERING CHEMISTRY 2 (CHEM171) Lecture Notes 1 st Series: Solution Chemistry of Salts SALTS Preparation Note, an acid
More informationSolubility Equilibrium
2016 Ksp note.notebook Solubility Equilibrium Learning Goals: to understand what happens when a compound dissolves in water to calculate the extent of dissolution...the molar solubility to calculate the
More informationChemical Equilibrium
Chemical Equilibrium Many reactions are reversible, i.e. they can occur in either direction. A + B AB or AB A + B The point reached in a reversible reaction where the rate of the forward reaction (product
More informationLECTURE #25 Wed. April 9, 2008
CHEM 206 section 01 LECTURE #25 Wed. April 9, 2008 LECTURE TOPICS: TODAY S CLASS: 18.1-18.2 NEXT CLASS: finish Ch.18 (up to 18.5) (1) 18.1 The Common Ion Effect basis of all Ch.18 = shift in eqm position
More informationSolubility and Complex-ion Equilibria
Solubility and Complex-ion Equilibria Solubility Equilibria Many natural processes depend on the precipitation or dissolving of a slightly soluble salt. In the next section, we look at the equilibria of
More informationLecture Presentation. Chapter 16. Aqueous Ionic Equilibrium. Sherril Soman Grand Valley State University Pearson Education, Inc.
Lecture Presentation Chapter 16 Aqueous Ionic Equilibrium Sherril Soman Grand Valley State University The Danger of Antifreeze Each year, thousands of pets and wildlife species die from consuming antifreeze.
More informationAqueous Equilibria, Part 2 AP Chemistry Lecture Outline
Aqueous Equilibria, Part 2 AP Chemistry Lecture Outline Name: The Common-Ion Effect Suppose we have a weak acid and a soluble salt of that acid. CH 3 COOH NaCH 3 COO CH 3 COOH CH 3 COO + H + Since NaCH
More informationModified Dr. Cheng-Yu Lai
Ch16 Aqueous Ionic Equilibrium Solubility and Complex Ion Equilibria Lead (II) iodide precipitates when potassium iodide is mixed with lead (II) nitrate Modified Dr. Cheng-Yu Lai Solubility-product constant
More informationHomework: 14, 16, 21, 23, 27, 29, 39, 43, 48, 49, 51, 53, 55, 57, 59, 67, 69, 71, 77, 81, 85, 91, 93, 97, 99, 104b, 105, 107
Homework: 14, 16, 21, 23, 27, 29, 39, 43, 48, 49, 51, 53, 55, 57, 59, 67, 69, 71, 77, 81, 85, 91, 93, 97, 99, 104b, 105, 107 Chapter 15 Applications of Aqueous Equilibria (mainly acid/base & solubility)
More informationAnalytical Chemistry Lecture III by/ Dr. Ekhlas Q. J. BUFFER SOLUTIONS
Analytical Chemistry Lecture III by/ Dr. Ekhlas Q. J. BUFFER SOLUTIONS Buffer solutions Definition Solutions which resist changes in ph when small quantities of acid or alkali are added. a solution that
More informationAP Chemistry. CHAPTER 17- Buffers and Ksp 17.1 The Common Ion Effect Buffered Solutions. Composition and Action of Buffered Solutions
AP Chemistry CHAPTER 17- Buffers and Ksp 17.1 The Common Ion Effect The dissociation of a weak electrolyte is decreased by the addition of a strong electrolyte that has an ion in common with the weak electrolyte.
More informationI. Multiple Choice Questions (Type-I) is K p
Unit 7 EQUILIBRIUM I. Multiple Choice Questions (Type-I) 1. We know that the relationship between K c and K p is K p K c (RT) n What would be the value of n for the reaction NH 4 Cl (s) NH 3 (g) + HCl
More information( 1 ) Concept of acid / base
Section 6.2 Ionic Equilibrium Unit 628 ( 1 ) Concept of acid / base The best definition of acids and bases is that proposed by T.M. Lowry and also, independently by J.N. Bronsted in 1923. BronstedLowry
More informationIII.1 SOLUBILITY CONCEPT REVIEW
III.1 SOLUBILITY CONCEPT REVIEW Read Hebden p. 73 76 and review basic solubility definitions. Soluble means Insoluble means The Dissolving Process IONIC Solutions MOLECULAR Solutions (Covalent compounds)
More informationAqueous Equilibria Pearson Education, Inc. Mr. Matthew Totaro Legacy High School AP Chemistry
2012 Pearson Education, Inc. Mr. Matthew Totaro Legacy High School AP Chemistry The Common-Ion Effect Consider a solution of acetic acid: HC 2 H 3 O 2 (aq) + H 2 O(l) H 3 O + (aq) + C 2 H 3 O 2 (aq) If
More informationSolubility Equilibria
Chapter 17 SOLUBILITY EQUILIBRIA (Part II) Dr. Al Saadi 1 Solubility Equilibria The concept of chemical equilibrium helps to predict how much of a specific ionic compound (salt) will dissolve in water.
More informationChapter 17. Additional Aspects of Aqueous Equilibria. Lecture Presentation. John D. Bookstaver St. Charles Community College Cottleville, MO
Lecture Presentation Chapter 17 Additional Aspects of John D. Bookstaver St. Charles Community College Cottleville, MO The Common-Ion Effect Consider a solution of acetic acid: CH 3 COOH(aq) + H 2 O(l)
More informationThe solvent is the dissolving agent -- i.e., the most abundant component of the solution
SOLUTIONS Definitions A solution is a system in which one or more substances are homogeneously mixed or dissolved in another substance homogeneous mixture -- uniform appearance -- similar properties throughout
More informationTry this one Calculate the ph of a solution containing M nitrous acid (Ka = 4.5 E -4) and 0.10 M potassium nitrite.
Chapter 17 Applying equilibrium 17.1 The Common Ion Effect When the salt with the anion of a is added to that acid, it reverses the dissociation of the acid. Lowers the of the acid. The same principle
More informationQuick Review. - Chemical equations - Types of chemical reactions - Balancing chemical equations - Stoichiometry - Limiting reactant/reagent
Quick Review - Chemical equations - Types of chemical reactions - Balancing chemical equations - Stoichiometry - Limiting reactant/reagent Water H 2 O Is water an ionic or a covalent compound? Covalent,
More informationLearning Objectives. Solubility and Complex-ion Equilibria. Contents and Concepts. 3. Precipitation Calculations. 4. Effect of ph on Solubility
Solubility and Comple-ion Equilibria. Solubility and the Common-Ion Effect a. Eplain how the solubility of a salt is affected by another salt that has the same cation or anion. (common ion) b. Calculate
More informationChemical Equilibrium. Many reactions are, i.e. they can occur in either direction. A + B AB or AB A + B
Chemical Equilibrium Many reactions are, i.e. they can occur in either direction. A + B AB or AB A + B The point reached in a reversible reaction where the rate of the forward reaction (product formation,
More informationSolubility Equilibrium When a substance dissolves an equilibrium results between the precipitate and the dissolved ions. The solution becomes
Solubility Equilibrium When a substance dissolves an equilibrium results between the precipitate and the dissolved ions. The solution becomes saturated. The particles dissolving equals the particles precipitating.
More information173 Buffer calculation: Tris buffer - Tris(hydroxymethyl)-aminomethane. tris base
173 Buffer calculation: Tris buffer - Tris(hydroxymethyl)-aminomethane tris base tris-hcl (conjugate acid of tris base) Calculate the ph of a buffer made from 50 ml of 0.10M tris and 50 ml of 0.15M tris-hcl.
More informationCHAPTER 7.0: IONIC EQUILIBRIA
Acids and Bases 1 CHAPTER 7.0: IONIC EQUILIBRIA 7.1: Acids and bases Learning outcomes: At the end of this lesson, students should be able to: Define acid and base according to Arrhenius, Bronsted- Lowry
More informationCH 4 AP. Reactions in Aqueous Solutions
CH 4 AP Reactions in Aqueous Solutions Water Aqueous means dissolved in H 2 O Moderates the Earth s temperature because of high specific heat H-bonds cause strong cohesive and adhesive properties Polar,
More information2/4/2016. Chapter 15. Chemistry: Atoms First Julia Burdge & Jason Overby. Acid-Base Equilibria and Solubility Equilibria The Common Ion Effect
Chemistry: Atoms First Julia Burdge & Jason Overby 17 Acid-Base Equilibria and Solubility Equilibria Chapter 15 Acid-Base Equilibria and Solubility Equilibria Kent L. McCorkle Cosumnes River College Sacramento,
More informationSaturated vs. Unsaturated
Solubility Equilibria in Aqueous Systems K sp (Equilibria of Slightly Soluble Salts, Ionic Compounds) Factors that Affect Solubility (Common Ion Effect, AcidBase Chemistry) Applications of Ionic Equilibria
More informationAdditional Aspects of Aqueous Equilibria David A. Katz Department of Chemistry Pima Community College
Additional Aspects of Aqueous Equilibria David A. Katz Department of Chemistry Pima Community College The Common Ion Effect Consider a solution of acetic acid: HC 2 H 3 O 2(aq) + H 2 O (l) H 3 O + (aq)
More informationChapter 19 Solubility and Complex Ion Equilibria
Chapter 19 Solubility and Complex Ion Equilibria "if you are not part of the solution, then you are part of the precipitate" - all solutions of salts exist as a balance between the dissolved cations and
More informationChapter 16. Solubility Equilibria 10/14/2010. Solubility Equilibria. Solubility Product (Constant), K sp. Solubility and the Solubility Product
Solubility Equilibria These are associated with ionic solids dissolving in water to form aqueous solutions Chapter 16 Solubility Equilibria It is assumed that when an ionic compound dissolves in water,
More informationTYPES OF CHEMICAL REACTIONS
TYPES OF CHEMICAL REACTIONS Precipitation Reactions Compounds Soluble Ionic Compounds 1. Group 1A cations and NH 4 + 2. Nitrates (NO 3 ) Acetates (CH 3 COO ) Chlorates (ClO 3 ) Perchlorates (ClO 4 ) Solubility
More informationCHEM 12 Unit 3 Review package (solubility)
CHEM 12 Unit 3 Review package (solubility) 1. Which of the following combinations would form an ionic solid? A. Metalloid - metal B. Metal non-metal C. Metalloid metalloid D. Non-metal non-metal 2. Which
More informationChapter 6. Types of Chemical Reactions and Solution Stoichiometry
Chapter 6 Types of Chemical Reactions and Solution Stoichiometry Chapter 6 Table of Contents (6.1) (6.2) (6.3) (6.4) (6.5) (6.6) (6.7) (6.8) Water, the common solvent The nature of aqueous solutions: Strong
More informationChemistry 12 Review Sheet on Unit 3 Solubility of Ionic Substances
Chemistry 12 Review Sheet on Unit 3 Solubility of Ionic Substances 1. Identify each of the following as ionic or molecular substances: a) NaCl (aq)... b) CH 3 COOH (aq)... c) CCl 4(l)... d) HNO 3(aq)...
More informationSolution Stoichiometry
Chapter 8 Solution Stoichiometry Note to teacher: You will notice that there are two different formats for the Sample Problems in the student textbook. Where appropriate, the Sample Problem contains the
More information... so we need to find out the NEW concentrations of each species in the system.
171 Take 100. ml of the previous buffer (0.050 M tris / 0.075 M tris-hcl), and add 5.0 ml of 0.10 M HCl. What is the ph of the mixture? The HCl should react with basic component of the buffer (tris), and
More informationIons in Solution. Solvent and Solute
Adapted from Peer-led Team Learning Begin at the beginning and go on till you come to the end: then stop." Early ideas of atoms and compounds, developed primarily through the reactions of solids and gases,
More informationSolubility and Complex Ion. Equilibria
Solubility and Complex Ion a mineral formed by marine organisms through biological precipitation CALCITE Equilibria CaCO 3(s) Ca 2+ (aq) + CO 3 2- (aq) K = K sp = [Ca 2+ ][CO 3 2- ] = 2.8 x 10-9 K sp =
More informationChapter 4. The Major Classes of Chemical Reactions 4-1
Chapter 4 The Major Classes of Chemical Reactions 4-1 The Major Classes of Chemical Reactions 4.1 The Role of Water as a Solvent 4.2 Writing Equations for Aqueous Ionic Reactions 4.3 Precipitation Reactions
More informationCHAPTER 16 ACID-BASE EQUILIBRIA AND SOLUBILITY EQUILIBRIA
CHAPTER 16 ACID-BASE EQUILIBRIA AND SOLUBILITY EQUILIBRIA 16.5 (a) This is a weak acid problem. Setting up the standard equilibrium table: CH 3 COOH(aq) H (aq) CH 3 COO (aq) Initial (): 0.40 0.00 0.00
More informationIntroducing Driving Force #3 - Formation of a Solid
Introducing Driving Force #3 - Formation of a Solid A solid that forms in an aqueous reaction is called a precipitate Precipitation reactions are also known as double replacement reactions Cations trade
More informationWhat is the ph of a 0.25 M solution of acetic acid (K a = 1.8 x 10-5 )?
1 of 17 After completing this chapter, you should, at a minimum, be able to do the following. This information can be found in my lecture notes for this and other chapters and also in your text. Correctly
More information1. Forming a Precipitate 2. Solubility Product Constant (One Source of Ions)
Chemistry 12 Solubility Equilibrium II Name: Date: Block: 1. Forming a Precipitate 2. Solubility Product Constant (One Source of Ions) Forming a Precipitate Example: A solution may contain the ions Ca
More informationEquilibrium principles in aqueous systems are limited to qualitative descriptions and/or calculations involving:
NCEA Chemistry 3.6 Aqueous Systems AS 91392 Demonstrate understanding of equilibrium principles in aqueous systems Aqueous systems are limited to those involving sparingly soluble ionic solids Equilibrium
More informationAdvanced Chemistry Practice Problems
Aqueous Equilibria: olar Solubility and the Common Ion Effect 1. Question: Which of the following compounds will decrease the solubility of lead(ii) bromide in water? a. Lead(II) nitrate b. Sodium chloride
More informationChem 12 Practice Solubility Test
Chem 12 Practice Solubility Test 1. Which combination of factors will affect the rate of the following reaction? Zn (s) + 2HCl ZnCl 2 + H 2(g) A. Temperature and surface area only B. Temperature and concentration
More informationSolutions & Solubility: Net Ionic Equations (9.1 in MHR Chemistry 11)
Solutions & Solubility: Net Ionic Equations (9.1 in MHR Chemistry 11) 1 Solubility vs. Temperature 2 Solubility Table Anions SOLUBILITY Table 8.3 page 363 in MHR Cl Br I S OH SO CO 3 PO 3 SO 3 C 2 H 3
More informationChapter 8: Applications of Aqueous Equilibria
Chapter 8: Applications of Aqueous Equilibria 8.1 Solutions of Acids or Bases Containing a Common Ion 8.2 Buffered Solutions 8.3 Exact Treatment of Buffered Solutions 8.4 Buffer Capacity 8.5 Titrations
More informationAcid-Base Equilibria and Solubility Equilibria
Acid-Base Equilibria and Solubility Equilibria Acid-Base Equilibria and Solubility Equilibria Homogeneous versus Heterogeneous Solution Equilibria (17.1) Buffer Solutions (17.2) A Closer Look at Acid-Base
More informationNet Ionic Reactions. The reaction between strong acids and strong bases is one example:
Net Ionic Reactions Model 1 Net Ionic Reactions. Net ionic reactions are frequently used when strong electrolytes react in solution to form nonelectrolytes or weak electrolytes. These equations let you
More informationChemistry 12 Unit III Solubility Notes
Chemistry 12 Unit III Solubility Notes III.1 A Review Of Solubility There are only three classes of compounds that form ionic solutions: ACIDS, BASES and SALTS. This unit will deal only with SALTS. Acids
More informationSession 8: LECTURE OUTLINE (SECTIONS I1 I4 pp F61 F67)
Session 8: LECTURE OUTLINE (SECTIONS I1 I4 pp F61 F67) I. Elecrolytes a. Soluble substances b. Insoluble substances c. Electrolytes d. Non-Electrolytes e. Ions and electrical conductivity f. Strong and
More informationUnit 10 Solution Chemistry 1. Solutions & Molarity 2. Dissolving 3. Dilution 4. Calculation Ion Concentrations in Solution 5. Precipitation 6.
Unit 10 Solution Chemistry 1. Solutions & Molarity 2. Dissolving 3. Dilution 4. Calculation Ion Concentrations in Solution 5. Precipitation 6. Formula, Complete, Net Ionic Equations 7. Qualitative Analysis
More information7. A solution has the following concentrations: [Cl - ] = 1.5 x 10-1 M [Br - ] = 5.0 x 10-4 M
Solubility, Ksp Worksheet 1 1. How many milliliters of 0.20 M AlCl 3 solution would be necessary to precipitate all of the Ag + from 45ml of a 0.20 M AgNO 3 solution? AlCl 3(aq) + 3AgNO 3(aq) Al(NO 3)
More informationAcid-Base Equilibria and Solubility Equilibria
ACIDS-BASES COMMON ION EFFECT SOLUBILITY OF SALTS Acid-Base Equilibria and Solubility Equilibria Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 2 The common
More informationChapter 4. Types of Chemical Reactions and Solution Stoichiometry
Chapter 4 Types of Chemical Reactions and Solution Stoichiometry Chapter 4 Table of Contents 4.1 Water, the Common Solvent 4.2 The Nature of Aqueous Solutions: Strong and Weak Electrolytes 4.3 The Composition
More informationAlief ISD Chemistry STAAR Review. Reporting Category 5: Solutions The Importance of Water
Alief ISD Chemistry STAAR Review C. 10.A Describe the unique role of water in chemical and biological systems. Reporting Category 5: Solutions The Importance of Water Factors that contribute to water s
More informationChapter 17 Additional Aspects of
Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 17 Additional Aspects of John D. Bookstaver St. Charles Community College Cottleville,
More informationed. Brad Collins Aqueous Chemistry Chapter 5 Some images copyright The McGraw-Hill Companies, Inc. Sunday, August 18, 13
ed. Brad Collins Aqueous Chemistry Chapter 5 Some images copyright The McGraw-Hill Companies, Inc. A solution is a homogenous mixture of 2 or more substances at the molecular level The solute(s) is(are)
More informationFunsheet 9.1 [VSEPR] Gu 2015
Funsheet 9.1 [VSEPR] Gu 2015 Molecule Lewis Structure # Atoms Bonded to Central Atom # Lone Pairs on Central Atom Name of Shape 3D Lewis Structure NI 3 CF 4 OCl 2 C 2 F 2 HOF Funsheet 9.1 [VSEPR] Gu 2015
More informationPart One: Solubility Equilibria. Insoluble and slightly soluble compounds are important in nature and commercially.
CHAPTER 17: SOLUBILITY AND COMPLEX ION EQUILIBRIA Part One: Solubility Equilibria A. Ksp, the Solubility Product Constant. (Section 17.1) 1. Review the solubility rules. (Table 4.1) 2. Insoluble and slightly
More informationLast Lecture. K 2 SO 4 (aq) + Ba(NO 3 ) 2 (aq) AgNO 3 (aq) + KCl(aq) NaNO 3 (aq) + KCl(aq) What will happen when these are mixed together?
Announcements Precipitation lab write-up due tomorrow at the start of discussion Text HW due tomorrow in discussion Lon-capa HW #4 Type 1 due Monday, Oct 15 th at 7:00pm Lon-capa HW #4 Type 2 due Wednesday,
More information5. Pb(IO 3) BaCO 3 8. (NH 4) 2SO 3
Chemistry 11 Solution Chemistry II Name: Date: Block: 1. Ions in Solutions 2. Solubility Table 3. Separating Ions Ions in Solutions Ionization Equation - Represents the salt breaking apart into ions. Practice:
More informationReactions in Aqueous Solutions
Copyright 2004 by houghton Mifflin Company. Reactions in Aqueous Solutions Chapter 7 All rights reserved. 1 7.1 Predicting if a Rxn Will Occur When chemicals are mixed and one of these driving forces can
More informationChemical Equilibrium
Chemical Equilibrium THE NATURE OF CHEMICAL EQUILIBRIUM Reversible Reactions In theory, every reaction can continue in two directions, forward and reverse Reversible reaction! chemical reaction in which
More informationFlashback - Aqueous Salts! PRECIPITATION REACTIONS Chapter 15. Analysis of Silver Group. Solubility of a Salt. Analysis of Silver Group
Page III-15-1 / Chapter Fifteen Lecture Notes Flashback - Aqueous Salts! If one ion from the Soluble Compd. list is present in a compound, the compound is water soluble. PRECIPITATION REACTIONS Chapter
More information****************************************************************************
**************************************************************************** To quickly summarize: 1. The solubility of a compound is decreased when an ion which is the same as one of the ions in the compound
More informationChapter 4 Types of Chemical Reaction and Solution Stoichiometry
Chapter 4 Types of Chemical Reaction and Solution Stoichiometry Water, the Common Solvent One of the most important substances on Earth. Can dissolve many different substances. A polar molecule because
More informationChapter Test A. Chapter: Chemical Equilibrium
Assessment Chapter Test A Chapter: Chemical Equilibrium In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question. 1. A 15.0 ml volume
More informationSolutions CHAPTER OUTLINE
Chapter 8A Solutions 1 CHAPTER OUTLINE Type of Solutions Electrolytes & Nonelectrolytes Equivalents of Electrolytes Solubility & Saturation Soluble & Insoluble Salts Formation of a Solid Precipitation
More information