Equation Writing for a Neutralization Reaction

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1 Equation Writing for a Neutralization Reaction An Acid-Base reaction is also called a Neutralization reaction because the acid (generates H + or H 3 O + ) and base (generates OH ) properties of the reactants are neutralized or cancelled out. In general, we can write: Acid + Base Salt (ionic cmpd) + Water We write the equations for a neutralization reaction using the same double displacement steps we use for precipitation reaction, but water is formed instead of a solid. This is the driving force for the reaction. Be especially careful to distinguish between strong acids and weak acids. o Strong Acids ionize in water 100%, so show H 3 O + as a reactant in ionic equations (TIE and NIE), and add a water molecule to the product side for each hydronium. Strong Acids: HCl, HBr, HI, H 2 SO 4, HNO 3, and HClO 4 o Weak acids do not ionize (well, VERY little), so we write these as neutral molecules in the ionic equations. But they do lose an H + in the reaction! Mol Eqn: HBr(aq) + KOH TIE: NIE: Chem Fall 2018

2 H 3 PO 4 (aq) + NaOH(aq) HCl(aq) + AgOH(s) Chem Fall 2018

3 Chapter 7: Quantitative Composition of Compounds 7.1 The Mole Atoms and molecules are incredibly small particles, yet we need a way to reliably measure out known quantities in the lab. Since chemical equations relate numbers of atoms and molecules, we need a way to count these in the lab when doing reactions. We have the following SI definitions to help us: o The mass of 1 atom of 12 6 C = 12 u exactly o The number of atoms in exactly 12 g of C is exactly 1 mole. C 6 mole is abbreviated mol 12 1 mol of contains C atoms. C is Avogadro s number. A mole tells us how many, just like a dozen or a gross. Since all atomic weights in the periodic table are determined relative to C-12, we have the following perspectives: Mass of an atom of an element = atomic weight number + units u Mass of 1 mole of an element = atomic weight number + units g 6 6 Chem Fall 2018

4 We can convert among number, moles, and mass of an element by noting the following: atoms = 1 mole = molar mass (g) o Many conversion factors may be created from these equivalences, but get in the habit of always including moles in your conversion factor. (Avoid, for example, converting directly from atoms mass.) What is the mass of mol of copper? How many atoms are present in mol of iron? How many magnesium atoms are contained in 5.00 g of Mg? 7.2 Molar Mass of Compounds One mole of a compound contains Avogadro s number of formula units ( molecules ) of that compound. The molar mass of a compound can be calculated by adding the molar masses of all the elements in the chemical formula. o Be careful counting the numbers of atoms in the formula! o Be careful when dealing with naturally-occurring diatomics! Chem Fall 2018

5 What is the molar mass of water? What is the molar mass of oxygen gas? What is the molar mass of Na 2 SO 4? What is the mass of mol of Na 2 SO 4. Chem Fall 2018

6 14.1 General Properties of Solutions A solution is a homogeneous mixture composed of one solvent and one or more solutes. o The solvent is the most abundant component of the solution. o The solutes are the least abundant components in the solution. Solutions come in all states of matter: Solutions exhibit the following properties Solubility Solubility describes the amount of solute that will dissolve in a specified amount of solvent under stated conditions (usually temperature). o Data is typically shown in tables of graphs. Chem Fall 2018

7 As the temperature increases, the solubility of: o Solids and Liquids o Gases As the pressure increases: o Solids and Liquids o Gases The nature of the solute and the solvent: Like dissolves like. Chem Fall 2018

8 Solutions may be saturated, unsaturated, or supersaturated. o Saturated: the solution contains the maximum amount of solute that can dissolve at a given temperature. o Unsaturated: the solution contains less solute than the solute can dissolve at a given temperature. o Supersaturated: the solution contains an amount of solute greater than the amount dissolved at saturation. This solution is unstable relative to the saturated solution if the solution is disturbed the excess solute will come out of solution leaving a saturated solution with solid solute at the bottom. Molarity (from section 14.4, pages ) Molarity is the unit of concentration most frequently used by chemists. molarity = M = number of moles of solute one liter of solution = moles liter Molar solution are prepared using a volumetric flask, a piece of lab glassware designed to contain one, precisely-known volume. Chem Fall 2018

9 o The OCC chemistry stockroom has volumetric flasks for many different volumes, ranging from 10 ml up to 4 L. If using other than 1 mole of solute, or a volume other than 1 L, simply plug the given moles and liters into the equation above to solve for molarity. o If not given moles and liters, place solute over solution and convert the given quantities to moles and liters. Calculate the molarity of the following solution: 1.75 mol of KBr in 0.75 L of solution. What is the molarity of a solution made by dissolving 2.00 g of potassium chlorate in enough water to make 150. ml of solution? Molarity can also be used as a conversion factor to solve other problems related to solutions. M = mmm L mml = M L L = mmm M How many grams of sodium chloride are needed to prepare 125 ml of M NaCl solution? Chem Fall 2018

10 Dilution (14.4, pages ) Dilution has the same meaning in chemistry as in everyday life: to make a solution less concentrated. o Technically, dilution reduces the molarity of the solution. o We typically start with a sample of solution of known volume and known molarity, and then add more solvent to bring the sample up to a new volume. M initial V initial = M final V final (in general, M 1 V 1 = M 2 V 2 ) o Why does it work? Find the concentration when 125 ml of 5.0 M H 3 PO 4 are diluted to a final volume of 775 ml. Calculate the volume of 16 M HNO 3 required to prepare 250 ml of 0.50 M HNO 3. Calculate the molarity of a solution prepared by diluting 125 ml of M K 2 Cr 2 O 7 (aq) with 875 ml of water. Assume the volumes are additive. Chem Fall 2018

11 Chapter 9: Calculations from Chemical Equations 9.1 Introduction to Stoichiometry Stoichiometry is the art of calculating the amounts of products or reactants using a balanced chemical equation. At the heart of stoichiometry is using a ratio of coefficients from the balanced equation to convert the moles of one species into the moles of another. o Dimensional analysis skills are used here! Consider the balanced equation for the combustion of propane: 1 C 3 H 8 (g) + 5 O 2 (g) 3 CO 2 (g) + 4 H 2 O(g) Let s see how stoichiometry works! When 0.5 mol of propane combusts, how many mol of H 2 O are made? How many mol of oxygen are need to combust 5.0 mol of propane? How many mol of CO 2 are produced when 6.0 mol of water forms? Chem Fall 2018

12 Acid-Base Titration (15.5, pp ) An acid-base titration uses a buret to carefully add a measured amount of base to a sample of acid (or vice versa) so that a neutralization reaction occurs. Typically the molarity and volume of the base are known, and the concentration of the acid is determined by stoichiometry. o The goal is to titrate until the equivalence point is reached; this is the point at which both acid and base are completely neutralized. At the equivalence point, we say that both acid and base are present in stoichiometric quantity; no limiting reactant calculation is needed. o In practice, both acid and base solutions are often clear and colorless, so the equivalence point cannot be visually determined. A small amount of an indicator solution, which changes color in base, is added to the acid at the start of the titration. When the solution changes color, it tells us we have gone past the equivalence point and are at the end point. o Titrations should be done slowly when the end point is neared such that one drop or less from the buret causes the solution to transition from colorless to colored. Chem Fall 2018

13 A 50.0 ml sample of HCl(aq) required ml of M NaOH(aq) for neutralization. What is the molarity of the acid? In an acid-base titration, ml of H 2 SO 4 were used to neutralize ml of M NaOH. What is the molarity of the H 2 SO 4 solution? Chem Fall 2018

14 To get everyone on the same λ for the Conductivity Lab, let s detour to Ch Electrolytes and Nonelectrolytes An aqueous solution, state (aq), is a homogeneous mixture made by dissolving a soluble substance in water. For example, H 2 O(l) NaCl(s) NaCl(aq) The water is drawn over the arrow to signify that it is not reacting with the water but only mixing with it, or dissolving in the water. An electrolyte is a substance whose aqueous solution conducts electricity (the subject of our lab!). We divide soluble substances into three types of electrolytes based on how well their aqueous solutions conduct electricity: o Nonelectrolyte: the aqueous solution does not conduct electricity. o Weak electrolyte: the aqueous solution conducts a small amount of electricity because the concentration of ions in solution is low. o Strong electrolyte: the aqueous solution conducts electricity well, indicating a large number of ions are in solution. Pure Water Nonelectrolyte Weak electrolyte Strong electrolyte Chem Fall 2018

15 Writing Dissociation Equations for Strong Electrolytes Soluble ionic compounds are strong electrolytes, and 100% of the molecules dissociate (separate) into their ions when dissolved in water. o The large number of ions generated allows the solution to conduct electricity strongly. We can write dissociation equations to show the ions generated. H 2 O(l) NaCl(s) Na + (aq) + Cl (aq) H 2 O(l) CaCl 2 (s) Ca 2+ (aq) + 2 Cl (aq) H 2 O(l) Al 2 (SO 4 ) 3 (s) 2 Al 3+ (aq) + 3 SO 2 4 (aq) H 2 O(l) AgCl(s) no dissociation, no ions; this salt is insoluble in water We will shortly see Solubility Rules which will allow us to predict which combinations of cation and anion will produce a soluble salt. The ions of soluble salts are surrounded by polar water molecules. This stabilizes the ions and keeps them in solution. o The ions of insoluble salts are not sufficiently stabilized by this hydration to remain in solution, so these salts do not dissolve. Chem Fall 2018

16 What about nonelectrolytes and weak electrolytes? Nonelectrolytes do not generate any ions when they dissolve in water, and since there are no ions, no electricity is conducted. Since there are no ions to separate, we refer to the dissolving equation for a nonelectrolyte. H 2 O(l) C 12 H 22 O 11 (s) C 12 H 22 O 11 (aq) H 2 O(l) C 2 H 5 OH(l) C 2 H 5 OH (aq) Weak electrolytes are covalent (nonionic) compounds that react with water to generate a small number of ions resulting in weak conductivity. o Weak acids and weak bases are weak electrolytes. We say these substances ionize in water, creating ions where none existed before. Here are some ionization equations of weak electrolytes; note that water is a reactant in these equations. Acetic acid,weak acid: CH 3 COOH(aq) + H 2 O(l) H 3 O + (aq) + CH 3 COO (aq) Ammonia, weak base: NH 3 (aq) + H 2 O(l) NH 4 + (aq) + OH (aq) Chem Fall 2018

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