REACTIONS IN AQUEOUS SOLUTIONS

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1 REACTIONS IN AQUEOUS SOLUTIONS [ MH5; Ch. 4] Most reactions in water involve hydrated, charged species [ (aq) ]. Any substance which is ionic in the solid state will form ions in solution. EXAMPLE: KCR (s)! KCR (aq)! K + (aq) + CR (aq) When we write an ionic compound as (aq), we really mean that it is hydrated (or dissolved in water) and has formed ions. Some covalent substances give ions in solution: EXAMPLE: HCR (g)! H + (aq) + CR (aq) HCR is a strong acid; it is completely ionized in solution. Some other covalent substances are only partially ionized in solution: CH 3 COOH (aq) º CH 3 COO (aq) + ~ 99 % ~ 1% H + (aq) CH 3 COOH is a weak acid - not completely ionized... Recall that any substance which gives ions in solution is called an ELECTROLYTE; a solution containing ions will conduct electric current! A strong electrolyte solution contains lots of ions; a weak electrolyte has fewer ions. 50

2 CONCENTRATION UNITS[ MH5: 10.1] As much of the work in this course involves reactions of species in solution, we need to be able to describe the amounts of these species present. A solution consists of the solvent (the main liquid part; in most cases water) and one or more solutes (the things that are dissolved in the liquid). We have already done calculations to determine the amounts of reactants and products in reactions; so far these amounts have been in grams... But measuring the mass of solutions is usually messy... So, with solutions, we find it more convenient to measure the volume, instead of the mass. But we need to know more than the volume... We need to know how much solute (the dissolved stuff) is present, because it is usually the solute that is doing the reacting... How much solute is contained in a certain volume of solution is described by CONCENTRATION. There are many ways of expressing concentration; what we use usually depends on what we are actually interested in... The most useful for us is to know (or be able to figure out) the number of moles of solute present in a given volume. This way of expressing concentration is called MOLARITY... defined as: " moles of solute per L of solution; Units are mol L 1, or M " often denoted by [ ] about the solute 51

3 How do we determine and use Molarity? EXAMPLE 1: What is the Molarity of a solution which contains 1.65 mole of solute in 850 ml of solution? EXAMPLE 2: Determine the number of moles of solute present in 45.0 ml of a 2.75 moll 1 solution. EXAMPLE 3: What volume of this solution contains 3.50 moles of solute? 52

4 Other ways of expressing concentration are: Mass per cent, parts per million, parts per billion, etc: mass per cent = mass of solute x 100 % total mass of solution ppm (of solute) = mass of solute (mg) total mass of solution (kg). mass of solute (mg) vol of solution (L) (in very dilute aqueous solution, as 1 g of H 2 O has volume. 1 ml) ppb (of solute) = ppm x 1000 Mole fraction: moles (of solute) total moles (solute and solvent) There are no units for mole fraction!! Sometimes we have to be able to convert between units... If we are going to convert from units with mass to units with volume (or vice-versa) we need the density of the solution. Density = mass of solution (usually g) Volume of solution (usually ml) 53

5 EXAMPLE: A jug of commercial concentrated hydrochloric acid is labeled: 37.5 % HCR by mass. If the density of the solution is 1.19 g ml 1, what volume of this concentrated solution would be required to obtain 7.45 moles of HCR? 54

6 SOLUBILITY Water is generally the best solvent for ionic solids, many of which are salts (product of reaction of an acid and a base). It is very useful to be able to predict what compounds will ionize when placed in water, and also to know what compounds will not even dissolve in water to any great extent. SOLUBILITY RULES Soluble Compounds Nitrates (NO 3 ) Na +, K +, NH + 4 (to be Memorized!!) Exceptions None None Halides (CR, Br, I ) Except Ag, Hg 2 +, Cu +, Pb +2 Sulfates (SO 4 2 ) Except Ca +2, Sr +2, Ba +2, Pb +2 Sparingly Soluble Compounds Sulfides (S 2 ) Exceptions Except Group IA, IIA ions and NH 4 + Carbonates ( CO 3 2 ) Except Group IA ions and NH 4 + Phophates ( PO 4 3 ) Except Group IA ions and NH 4 + Hydroxides (OH ) Except Group IA ions, NH + 4 and Ba +2 55

7 WRITING EQUATIONS FOR REACTIONS IN SOLUTION Obviously, you need to write some reactants and products... But often, there species present other than those which are actually taking part in the reaction; these are often called spectator ions. For ionic substances, spectator ions are usually omitted from the equation. Examples of spectator ions are Na +, K+ (recall all salts containing Na + or K + are soluble) and CR. EXAMPLE 1: Na 2 SO 4 (aq) + Sr(NO 3 ) 2 (aq)! SrSO 4 (s) + 2 NaNO 3 (aq) Removing the spectator ions, we get: EXAMPLE 2: NaHCO 3 + CH 3 COOH! CH 3 COONa + CO 2 + H 2 O Removing the spectator ions, gives: 56

8 TYPES OF REACTIONS 1) Precipitation [MH5; 4.2] Reactions which give an insoluble product, called a precipitate. First write equation using ions for soluble species: Remove the spectator ions: 2) Neutralization (Acid-Base) Reactions [MH5; 4.3] What is an acid and what is a base??? Arrhenius said: An acid is a substance which increases the hydrogen ion concentration when dissolved in water. The Hydrogen ion, H +, is really just a proton and is never found as such in solution; the actual ion formed is H 3 O +, the hydronium ion. All the H + found in water is actually in this form... So we should write H 3 O +, but we get lazy and just write H +. EXAMPLES: 57

9 Arrhenius also said: A base is a substance which either: 1) increases the [OH ] in water OR 2) decreases the [H 3 O + ] in water To see how both these statements can be true, we will look at the strong base Sodium Hydroxide, NaOH: Bronstead and Lowry came up with another definition... According to Bronsted and Lowry: Acid = proton donor; gives away an H + (usually to water, giving H 3 O + ) Base = proton acceptor; takes an H + (usually from water, leaving OH ) Acid-base reactions are of the general type Acid + Base! Salt + Water In water, a strong acid is one whose acidic proton(s) is (are) fully ionized to H + (aq), by donation of its proton to the solvent, water. A strong base is one that is fully ionized to give OH (aq), which then acts as a Bronsted-Lowry base, so that the actual acid-base reaction between a strong acid and a strong base is: H + (aq) + OH (aq)! H 2 O (Any other ions present are Spectator Ions) 58

10 EXAMPLE: A neutralization reaction of a strong acid and a strong base involves equal numbers of mol of H + (aq) and OH (aq): EXAMPLES: The Equivalence Point of an acid-base reaction is a more general term than neutralization. The Equivalence Point occurs when the number of moles of acidic hydrogen (which is not necessarily fully ionized to H + (aq) ) is equal to the number of moles of the base (again not necessarily fully ionized to give OH ). 59

11 The neutralization point, in the reaction of a strong acid and a strong base, is a special case of the equivalence point. In this case both acid and base are fully ionized. 60

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