Unit 6: Solutions, Acids & Bases

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1 Unit 6: Solutions, Acids & Bases Section 1: Intro to Solutions & Molarity Section 2: Solution Stoichiometry Section 3: Acids & Bases Section 4: ph Calculations & titration

2 Unit Synapsis In this unit will explore what happens at the molecular level when things dissolve in water to form solutions. Because reactants in chemical equations are very often in the form of solutions, we will revisit stoichiometry one more time and look at mole conversions when a substance is in Liters of solution. From there we will move on to acids and bases. Acids and Bases are more or less solutions. Finally we will wrap things up by looking at the way to express the concentration of two important ions in solutions; H + ions and OH - ions.

3 Section 1: Intro to Solutions & Molarity This part of the Unit is covered on pages X-Y in your textbook

4 Section 1: Intro to Solutions & Molarity / Objectives After this lesson I can define solutions and give the three properties of solutions mentioned in lecture that separate them from other types mixtures. Distinguish the terms solute & solvent. Distinguish the terms soluble, insoluble, slightly soluble, miscible, & saturation point. interpret a solubility curve. explain the concept of super-saturated solution & precipitation Describe the dissolving process in terms of random molecular motion. Write chemical equations for ionic compounds dissolving in water. solve problems involving molarity.

5 Solutions A Solution is a homogenous mixture and is formed when one substance dissolves in another. homogenous means it is uniform throughout. Colloids like milk appear to be homogenous but really are heterogeneous and you can see this when you put them under a microscope. Suspensions like smoke and gravel are heterogeneous. Three major properties of solutions that can help you distinguish them from other types of mixtures: A solution is stable; it won t settle out of separate. Even over an extended period of time like Milk & Mayo do. The solute cannot be separated from the solvent by filtration (or mechanically). It s impossible to see the parts of a solution with the naked eye. There are two parts of a solution: The solute gets dissolved (could be solid, liquid, or gas) The solvent does the dissolving Solvent s can also be solids, liquids, or gases. Water is by far the most common and most important solvent. It has been called the universal solvent, and the solvent of life. We are going strictly focus on solutions where water is the solvent in Chemistry B. Solutions where water is the solvent are called aqueous solutions.

6 Solubility If a substance will dissolve in a given solvent it s said to be soluble. Examples: Sugar, Salt, Alcohol and Carbon Dioxide are soluble in water If a substance will not dissolve in a given solvent it s said to be insoluble. Examples: Oil & Sand are insoluble in water If a substance is soluble, it could be miscible or it could have a saturation point. Miscible means there is no limit to how much of the solute can dissolve in the solvent. Saturation Point means there is a limit. Examples: Salt & Sugar have a saturation point in water. There is only so much you can dissolve in a given amount. Alcohol, however, is miscible in water. There is no limit to how much alcohol can be dissolved in a given amount water. A solution that has the maximum amount of solute dissolved in a given amount of solvent is said to be a saturated solution.

7 Saturation Point & Saturated Solutions A couple things you should know about saturation point & Saturated Solutions: It s often expressed grams per 100 grams of water, but since water s density is 1 gram / ml it s often easier to think of it as grams per 100 ml of water. The temperature of the solvent effects saturation point. Generally speaking the higher the temperature the higher the saturation point of solid solutes. The reverse is true for gas solutes Pressure can also effect saturation point. Soda bottles are around ~2 atm of pressure which increase the saturation point of CO 2. When the soda bottle is open the pressure is released. This causes the saturation point of CO 2 to drop and some of the CO 2 to bubble out.

8 Some examples of Substances and Their Solubility's Table Salt: NaCl Soluble with a saturation point of 25 C Sugar: C 6 H 12 O 6 Soluble with a saturation point of 25 C Calcium Hydroxide: Ca(OH) 2 slightly soluble Starch (flour) C 6 H 10 O 5 insoluble Sand: SiO 2 insoluble Ethanol C 2 H 6 O miscible

9 Solubility Curve of Selected Ionic Compounds in Water

10 Solubility Curve of Selected Ionic Compounds in Water

11 VIDEOS! VIDEOS WE ARE GOING TO WATCH IN CLASS: Fuse School Video: Solubility Curves Chemistry for All VIDEOS YOU CAN WATCH AT HOME FOR HELP OR REVIEW: Chem Academy Video: Solubility Curves Explained SciencePost Video: Solubility Curves Saturated, Unsaturated, & Supersaturated Solutions The Organic Chemistry Tutor Video: Solubility Curves Basic Introduction Chemistry Problems

12 A Few more Things on Solubility There is also slightly soluble which generally means you can t get more than a gram to dissolve in a entire liter of water. While a gram doesn t seem like much keep in mind that vast majority of drugs only require milligrams to work and will dissolve just fine when taken with a full glass of water. And finally there is a supersaturated solution. A supersaturated solution is when there is more of a solute dissolved than the saturation point allows. This usually occurs because the solute is dissolved at a higher temperature and then the solution is cooled down. The solute will eventually precipitate out of the solution. If the solute is a gas it will bubble out and if the solute is a solid crystal will form at the bottom of the solution (see KNO 3 demo).

13 VIDEOS! VIDEOS YOU CAN WATCH AT HOME FOR HELP OR REVIEW: The Organic Chemistry Tutor Video: Saturated, Unsaturated, & Supersaturate Solutions Concentration vs. Solubility

14 Ion-Dipole Interactions & The Dissolving Process Note that even though it takes very high temperatures to separate NaCl Units from one another, Salt and most other ionic compounds easily dissolve in water. In other words, it take tremendous heat to break apart the crystal lattice of table salt and get it to melt, but the crystal lattice can just as easily be broken apart by simply placing the table salt in some water. This is because the positive Ion in the compound is attracted to the negative dipole of the water molecule, and the negative ion is attracted to the positive dipole. The dissolving process can be modeled using chemical equations: NaCl(s) Na + (aq) + Cl - (aq) CaCl 2 (s) Ca 2+( aq) + 2 Cl - (aq) Na 3 PO 4 (s) 3 Na + (aq) + PO 4 3- (aq) Substances that form ions in solutions are called electrolytes because the ions help water to conduct electricity. Many molecular compounds that dissolve in water like sugar and alcohol are not electrolytes and do not form ions in water. We won t worry about the equations for these substances in Chem B.

15 VIDEOS! VIDEOS WE ARE GOING TO WATCH IN CLASS: McGraw Hill Video: NaCl Dissolving in Water CCC #7 Video: Dirty Laundry Note: Only watch till 8:45 CCC #27 Video: Solutions Note: Molality, Mass Percent, & Henry s Law are not apart of our learning objectives VIDEOS YOU CAN WATCH AT HOME FOR EXTRA HELP Tyler Dewitt Video: What happens when stuff dissolves?

16 Images Depicting Ion Dipole Interactions & The Dissolving Process

17 Image Depicting Ion-Dipole Interactions & the Dissolving Process

18 Practice Problems: Ionic Compounds Dissolving in Water Directions: Write the Equation for the following Ionic Compounds dissolving in water. Be Sure to include physical states and correct coefficients. 1) LiBr 2) Na 2 CO 3 3) FeCl 3 4) Ba(NO 3 ) 2 5) NiBr 3 6) Ti(NO 3 ) 4 7) K 2 SO 4 8) MgI 2

19 Solution Concentration Concentration is a measurement how much solute is dissolved in a given amount of solvent. There are several ways of expressing the concentration of a solution: Grams per liter (g/l); very common for expressing saturation points Parts Per Million (ppm); used for very low concentrations Pars Per Billion (ppb); use for very, very low concentrations Percentages; very common for substances that are miscible Molarity (mol/l or M ); very common in science & chemistry We are only going to worry about Molarity calculations in Chem B.

20 Molarity The Equation for Molarity: If the Molarity is known, and you are trying to convert either liters to moles or moles to liters, you can use Dimensional analysis. Or you can plug into the Molarity equation and solve using algebra, either way will work. Examples of Molarity written as a conversion factor: 6 M KBr solution could be written; 6 mol KBr = 1 L 2.55 M C 6 H 12 O 6 solution could be written; 2.55 mol C 6 H 12 O 6 = 1 L If you are trying to determine the molarity of a solution you made, you must plug the moles and Liters into the molarity equation.

21 Practice Problems: Molarity if 5.4 moles of NaCl is dissolved in water to make a 2 Liter solution, what is the Molarity of the Solution? If 88 grams of NaCl is dissolved in water to make a 3 Liter solution, what is the Molarity of the solution?

22 Practice Problems: Molarity Your doing a lab and your instructor pours you.155 Liters of a 2.5 M HCl solution. How many moles of HCl do you have? Your getting ready to run a chemical reaction and you calculate you need.640 moles of LiNO 3. You got some Lithium Nitrate but it s already dissolved in solution and the Molarity is 1.5 M. How many liters should you pour yourself?

23 Section 1 Additional Resources Khan Academy Page: Molarity Tyler Dewitt s Video: Molarity: Practice Problems Tyler Dewitt s Video: Molarity: Practice Problems (Part 2)

24 Section 2: Solution Stoichiometry This part of the Unit is covered on pages X-Y in your textbook

25 Section 2: Solution Stoichiometry / Objectives After this lesson I can solve stoichiometry problems involving molarity and solutions.

26 Solution Stoichiometry Previously we learned how to perform stoichiometry calculations when given grams of a substance or Liters of gas. The last type of stoichiometry problems we need to look at are those that involve liters of solution and molarity. Like with the previous problems, it s all about getting the substance in moles and looking at the ratio of coefficients in a balanced equation. The only difference now is that instead of converting back and forth between grams and moles using molar mass, or converting back and forth between liters of gas using PV=nRT, we will be using Molarity to get the moles.

27 Practice Problems: Solution Stoichiometry Suppose.090 Liters of a 1.75 M CuSO 4 solution are used. What is the theoretical yield of Copper Phosphate assuming an excess of Sodium Phosphate is used? 3 CuSO 4 (aq) + 2 Na 3 PO 4 (aq) Cu 3 (PO 4 ) 2 (s) + 3 Na 2 SO 4 (aq)

28 Practice Problems: Solution Stoichiometry How many liters of a 0.50 M H 3 PO 4 solution are needed to react with.440 Liters of a 0.35 M NaOH solution? H 3 PO 4 (aq) + 3 NaOH(aq) Na 3 PO 4 (aq) + 3 H 2 O(l)

29 Practice Problems: Solution Stoichiometry Suppose 2.4 Liters of a 6 M HCl solution is used in the reaction below. Assuming excess Aluminum, what is the theoretical Yield of Hydrogen gas in Liters at 25 C & 1 atm? 6 HCl(aq) + 2 Al 2 AlCl 3 (aq) + 3 H 2 (g)

30 Practice Problems: Solution Stoichiometry Sea water is about 0.50 M NaCl. To produce Cl 2 gas, a company evaporates sea water, melts the NaCl, and runs electricity through How many liters of sea water are needed to fill a tank with 15,000 liters of chlorine gas at STP? 2 NaCl(aq) 2 Na(s) + Cl 2 (g)

31 Practice Problems: Solution Stoichiometry If 22.5 ml of a 1.55 M CaCl 2 solution reacts with 60 ml of a 1.2 M Na 3 PO 4 solution, what s the theoretical yield of Ca 3 (PO 4 ) 2 in grams? What is the limiting reactant? 2 Na 3 PO 4 (aq) + 3 CaCl 2 (aq) Ca 3 (PO 4 ) 2 (s) + 6 NaCl(aq)

32 Section 3: Acids & Bases This part of the Unit is covered on pages X-Y in your textbook

33 Section 3: Acids & Bases / Objectives After this lesson I can give the two definitions acids and bases (bronstead-lowery & Arrhenius) explain the correlation between proton, H 3 O + & H + distinguish between strong and weak acids distinguish between strong and weak bases write equations for acids (strong or weak) and bases (strong or weak) dissolving in water. list the 3 observable properties of acids & 3 observable properties bases. compare and contrast acids & bases

34 Intro to Acids & Bases When we are talking about Acids & Bases we are talking about aqueous solutions. Substances can technically behave as an acid or base outside of water. However, for the most part acids and bases involve substances dissolved in water so that is where we will focus our study on in Chemistry B. Just like Ionic compounds (some bases are ionic compounds), acids and bases form ions when dissolved in water (meaning they are electrolytes). Acids & Bases always form the same ion. For acids, the Ion formed is always H + Side Note, that H + ion in turns reacts with a water molecule to form H 3 O +, so H 3 O + and H + can be used interchangeably when discussing acids. H + + H 2 O H 3 O + For bases, the Ion formed is always OH -

35 Image Showing How The H + Ion Attaches To a Water Molecule

36 Acids & Bases Definitions There are three different definitions for acids & bases and these definitions often overlap. We are only going to worry about two of them and you don t need to remember the dude s names that came up with these definitions. An Acid is a substance that donates H + Ions (proton donor) Produces H + / H 3 O + when dissolved in water A Base is a substance that Accepts H + Ions(proton acceptor) Produces OH - when dissolved in water

37 VIDEOS! VIDEOS WE ARE GOING TO WATCH IN CLASS: Fuse School Video: What is the Bronsted-Lowry Theory? CCC #8 Video: Acid Base Reactions in Solution Note: conjugate acids and bases are not in our objectives VIDEOS YOU CAN WATCH AT HOME FOR EXTRA HELP: Khan Academy Video: Acid-Base Definitions Note: Lewis Acids & Bases are not in our objectives

38 Examples of Acids & Bases Dissolving in Water Examples of Acids. (Notice how they donate or give up H + ions.) HCl(g) H + (aq) + Cl - (aq) or HCl(g) + H 2 O H 3 O + (aq) + Cl - (aq) HNO 3 (l) H + (aq) + NO 3- (aq) or HNO 3 (l) + H 2 O H 3 O + (aq) + NO 3- (aq) HBr(g) H + (aq) + Br - (aq) or HBr(g) + H 2 O H 3 O + (aq) + Br - (aq) Examples of Bases. (Notice how they give off OH- ions.) NaOH(s) Na + (aq) + OH - (aq) KOH(s) K + (aq) + OH - (aq) Note that as mentioned previously, acids and bases are both electrolytes because the produce ions in water. The bases in these examples are in fact ionic compounds and the equations are no different that what we looked at in the first section of the unit.

39 Strong vs Weak Acids A strong acid is an acid that fully ionizes in water. Meaning every last molecule splits off an H + ion. Sample equations for Strong Acids dissolving in water: HCl(g) H + (aq) + Cl - (aq) or HCl(g) + H 2 O H 3 O + (aq) + Cl - (aq) HNO 3 (l) H + (aq) + NO 3- (aq) or HNO 3 (l) + H 2 O H 3 O + (aq) + NO 3- (aq) A weak acid is an acid that partially ionizes in water. Meaning some, but not all, of the molecules split off H+ ions. To indicate that only some of the molecules dissociate their Hydrogen atom, a double arrow is used. Sample equations for Weak Acids dissolving in water: HCN H + (aq) + CN - (aq) Or HCN + H 2 O H 3 O + (aq) + CN - (aq) HNO 2 H + (aq) + NO 2- (aq) Or HNO 2 + H 2 O H 3 O + (aq) + NO 2- (aq) Note that strong and weak acids are molecules that contain at least 1 hydrogen atom.

40 Image Showing the Difference Between Strong Acids & Weak Acids

41 VIDEOS! VIDEOS WE ARE GOING TO WATCH IN CLASS: Mcgraw Hill Video: Acids Fuse School Video: What makes something Acidic? Fuse School Video: How are Strong and Weak Acids Different?

42 Strong vs Weak Bases A Strong Base is a base that fully ionizes OH - ions in water. Strong bases are Ionic compounds that contain an OH - in the chemical formula. In strong bases the compound literally adds OH- ions to water. Sample equations of Strong Bases dissolving in water: NaOH(s) Na + (aq) + OH - (aq) KOH(s) K + (aq) + OH - (aq) A weak base is a base that partially ionizes OH - ions in water. In weak bases the OH - ion is formed by taking a hydrogen from water. Sample equations of Weak Bases dissolving in water: NH 3 + H 2 O NH 4+ (aq) + OH - (aq) CH 5 N + H 2 O CH 6 N + (aq) + OH - (aq) Note that a weak base meets both our definitions of bases, while strong bases only meets the first definition. One more thing worth mentioning is that Bases are sometimes referred to as Alkalis.

43 VIDEOS! VIDEOS WE ARE GOING TO WATCH IN CLASS: Mcgraw Hill Video: Bases Fuse School Video: What Makes things Alkali? Fuse School Video: Strong and Weak Alkalis TedED video: The Strength and Weakness of Acids and Bases

44 Practice Problems: Writing Equations for Acids Dissolving in Water Directions: Write the Equation for the following Acids dissolving in water. Strong Acids: 1) HI 2) HClO 4 3) HBr Weak Acids: 1) C 6 H 8 O 7 2) H 2 C 2 O 4 3) H 3 PO 4

45 Practice Problems: Writing Equations for Bases Dissolving in Water Directions: Write the Equation for the following Bases dissolving in water. Strong Bases: 1) Ba(OH) 2 2) LiOH 3) NaOH Weak Bases: 1) NH 3 2) C 6 H 7 N 3) C 5 H 5 N

46 Observable Properties As Mentioned in the previous videos, Acids & Bases have some easily observable properties Acids Turn blue litmus paper red Taste Sour React with Metals Bases Turn red litmus paper blue Taste Bitter Are slippery Both Acids & Bases are Electrolytes Corrosive

47 Section 3 Additional Resources

48 Section 4: Neutralization & ph This part of the Unit is covered on pages X-Y in your textbook

49 Section 4: Neutralization & ph / Objectives After this lesson I can calculate ph & poh from molarity and vice versa. explain poh, ph, how they are related to concentration of H + & OH - in water. explain & write the equation for the auto-ionization of water. recall where acids and bases are on the ph scale. calculate ph from poh and vice versa. explain neutralization & write acid/base neutralization equations. solve neutralization problems that involve ph. give a short list of methods for determining the acidity or basicity of a solution and explain how indicators can be used.

50 ph ph stands for power of hydrogen and is just another way to express the H + Molarity in a given solution. Because the H + Molarity in pond water, swimming pools, blood, and many other substances is often of a very low concentration, ph is used to avoid scientific notation or a bunch of zeros. For example, a ph of 5 corresponds to M H + or M H + The Equation for ph: ph = -log [H + ] Anytime you see something in brackets, it means molarity. So the ph of a solution is just the negative log of the H + molarity. Furthermore, since strong acids full ionize, the H + molarity of a strong acid solution is just the molarity of that strong acid solution; M H + = M of any strong acid Finding the ph of a weak acid solution is tricky because not all the acid molecules ionize. Thus H + molarity will always be less than the molarity of the weak acid solution. We won t worry about finding [H + ] for weak acid solutions in Chemistry B (or weak base solutions.)

51 Practice Problems: ph calculations Directions: calculate the following ph in the following solutions. Assume all acids are strong. 1).5 M HCl 2).002 M HNO 3 3) M HI 4) 5 M HBr 5) M HClO 4 Directions: calculate the Molarity of H + ions in solution given the following ph values. 1) ph 4.5 2) ph 1.2 3) ph 5.5

52 poh poh is sometimes called ph s evil twin. poh is determined by the concentration of OH - ions in solution. poh = -log [OH - ] It is basically the counterpart of ph. Just like with strong acids, strong bases fully ionize so OH - M = M of any strong base or [OH-] = [strong base] Most students have heard of ph but not poh. This is because basic solutions can be expressed on the ph scale as well (and conversely acidic solutions can be expressed on the poh scale). For whatever reason, ph has become the popular and common way to express the concentration of both acidic and basic solutions. In acidic solutions ph < 7 and in basic solutions ph > 7. Finally, it s often nessassary to find the poh of a basic solution before you can find the ph. The equation for those conversions is; 14 = ph + poh

53 Practice Problems: poh calculations Directions: calculate the poh in the following solutions. Assume all bases are strong. 1) 2.5 M NaOH 2) M LiOH 3) M KOH 4) 10 M LiOH 5) M RbOH Directions: calculate the Molarity of OH - ions in solution given the following ph values. 1) poh 4.1 2) poh 3.1 3) poh.54

54 The Auto-ionization of water Water actually breaks apart into H + ions and OH - ions all on it s own. This only happens to a very, very, small percentage of the water molecules in a given sample. Less than.0001%. The chemical equation is below: H 2 O (aq) H + (aq) + OH - (aq) As previously mentioned, H + in water is really H 3 O + so the more appropriate equation is: 2 H 2 O (aq) H 3 O + (aq) + OH - (aq) In pure water, the concentration of H + and the concentration of OH - are exactly same; Thus, the ph in pure water or any neutral solutions is 7. When an acid is added to water, [H + ] increases and [OH - ] decreases. When a base is added to water, [H + ] decreases and [OH - ] increases. In conclusion, Hydrogen ions and Hydroxide ions are allways in water and aquous soltuions. Acids tip the balance towards the [H + ] and bases tip the balance towards [OH - ] This is after all, what acids and bases do! Produce H + or OH - in water, respectively.

55 ph Diagram (simple) Image Credit:

56 ph Diagram (showing H + M only) Image Credit:

57 ph Diagram (showing H + M & OH - M) Image Credit:

58 VIDEOS! VIDEOS WE ARE GOING TO TRY TO WATCH IN CLASS: Fuse School Video: What is ph? CCC #30 Video: ph & poh Videos you can watch at home for extra help or review: Science Post Video: Calculating ph & poh, [H+], [OH-], Acids & Bases CLEAR & SIMPLE Chem Academy Video: The ph Scale Explained Bozeman Science Video: Acids, Bases, & ph

59 Practice Problems: Harder ph problems What is the ph of a.15 M NaOH solution? 1.5 mol of a strong acid are added to water. The final of the solution is 10.6 Liters. What s the ph of the solution?

60 Practice Problems: Harder ph problems calculate the ph if the poh is 1.7 What s the ph of a solution if it contain Hydroxide ions? What s the Molarity of the Hydronium Ions in the solution?

61 Neutralization When you mix an acid and a base together, they neutralize each other forming water. H + + OH - H 2 O Some sample equations involving strong acids and strong bases are below. Notice that a short hand equation can be used by placing (aq) next to the acid and the base. Whenever this is done, you must remember than an acid or base when dissolved in water is in fact ionized. This ionization is shown using the complete equation. Short hand equation: NaOH(aq) + HCl(aq) H 2 O + NaCl(aq) More accurate or complete equation: Na + (aq) + OH - (aq) + H + (aq) + Cl - (aq) H 2 O + Na + (aq) + Cl - (aq) Short hand equation: KOH(aq) + HNO 3 (aq) H 2 O + KNO 3 (aq) More accurately or complete equation: K + (aq) + OH - (aq) H + (aq) + NO 3- (aq) H 2 O + K + (aq) + NO 3- (aq)

62 Practice Problems: Writing Acid & Base Neutralization Equations aqueous LiOH is used to neutralize aqueous HI. Write the short and complete equation for this. aqueous HBr, a strong acid is used to neutralize aqueous Calcium Hydroxide, which is a strong base. Write the short hand and complete equation for this.

63 Neutralization & ph To reach a ph of 7 and completely neutralize an acid solution, you will need as many moles of OH - are there are moles of H + in that solution. The reverse is true for basic solutions. In other words If a solution contains 2 moles of H + ions, you need 2 moles of OH - ions to completely neutralize. If a solution contains 10 moles of OH - ions you need 10 moles of H + ions to completely neutralize. If a solution contains moles of H + ions you need moles of OH - ions to completely neutralize.

64 Titration Knowing that equal amounts of H + & OH - are needed to neutralize acids & bases allows us to determine the ph of an unknown solution that is either acidic or basic. The process of technique for carrying this out is called titration or acid-base titration. Back in the day it was the best way to determine the ph of an unknown solution. Now a days we just use ph meters to find the ph of an unknown solution. However, titrations still persist in Chemistry classes because they are a great learning tool. The equation we use in titrations M A V A = M B V B M A = Molarity of H + V A = Volume of the solution containing the H + M B = Molarity of OH - V B = Volume of the solution containing OH -

65 VIDEOS! VIDEOS WE ARE GOING TO WATCH IN CLASS: Fuse School Video: How to do Titrations Fuse School Video: How to do Titration Calculations

66 Practice Problems: ph & Neutralization Problems You have 55ml of an unknown solution. It s tested with litmus paper and identified as acid. You titrate and it is neutralized with 24 ml of a.1 M NaOH solution. What is the ph of the acidic solution?

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