ࡱ> %` bjbj 2̟̟r*& 0 0 0 T ! r r r8DrlrD,htt""t"t"tw1w =w׌ٌٌٌG Ȩ$hj0 uxv|wuxux "t"tumS}S}S}ux6 R"t0 "t׌S}ux׌S}S}rcT "0 Ӈ"ts PԠO ryS0Ň|vӇ0 ӇEw>w,S}w$wEwEwEw=}EwEwEwuxuxuxux,,,$E r,,, rD hP   Honors Chemistry Chapter 19 Notes Part 2 Acids, Bases, and Salts (Student edition) Chapter 19 Part 2 problem set: 65, 69, 89, 93, 94, 96, 98, 99 19.2 Hydrogen Ions and Acidity Tap water . Why? Tap water contains many ( ) Distilled water appears to conduct electricity, but it does just a little, tiny bit. H2O + H2O ( The reaction happens 0.0000002% in the direction and 99.9999998% in the direction. The equilibrium constant for the self ionization of water: Keq = dont include we call this constant At 25 C0, [H3O+1] = so [OH-1] = so. Kw = Example: If the [H3O+1] is 1 x 10-3M, then what is the [OH-1]? The solution is because the hydronium ion concentration is than the hydroxide concentration. Fill in the table below: Beaker #[H3O+1][OH-1]Acid or Base11 x 10-521 x 10-232 x 10-444.16 x 10-6 Of course, all these numbers are confusing so The pH of a Solution: pH = pH stands for . logs are functions of . For example, the log of 1000 is (like ) and the log of .01 is (like ). Acid Base scale: Acid Neutral Base 0--------------------------------------7------------------------------------14 really it is from 2 to 16 since no acids/bases ever get more than 100 M solutions To convert [H3O+1] to pH: Formula: pH = - log [H3O+1] Calculator: Press the (-) key, the log key, enter the [H3O+1], and press the enter key. Fill in the following table: [H3O+1]pHAcid or Base1 x10 11 x 10 93.00 x 10 4 To convert pH to [H3O+1]: Formula: [H3O+1] = Antilog -pH Calculator: Press the 2nd key, the log key, the (-) key, enter pH, and press the enter key. Fill in the following table: [H3O+1]pHAcid or Base2115.22 Another formula to know: pH + pOH = 14 [H3O+1][OH-1]pHpOHAcid or Base2.00 x 10-54.10 x 10-56.8011.2NIB - Gram Equivalent Mass Chemical Equivalents: quantities of solutes that have . Ex1: HCl + NaOH ( NaCl + H2O To achieve a balance, 1 mole H+ needs to cancel out 1 mole OH-1. So, for the above reaction: 1 mole of HCl is necessary to balance 1 mole of NaOH. 1 mole HCl = ( Ex2: H2SO4 + 2 NaOH ( Na2SO4 + 2 H2O To achieve a balance, 1 mole H+ needs to cancel out 1 mole OH-1. So, for the above reaction: mole of H2SO4 is necessary to balance 1 mole of NaOH. mole H2SO4 = ( Ex3: To make H3PO4 chemically equivalent to NaOH, 1/3 mole of H3PO4 balances 1 mole NaOH Equivalent Weight: the # of grams of acid or base that will provide of protons or hydroxide ions. HClH2SO4H3PO4Moles of Acid1 1/3 Moles of Hydrogen111Equivalent Weights36.549.0532.7 Formula for calculating equivalent weight: eq. wt. = mw/equivalents : the # of hydrogen moles or hydroxide moles. Formula for calculating equivalents: # equivalents = (moles)(n) n = # of H or OH in the chemical formula Ex1a: Calculate the molecular weight of H2CO3: mw = Ex1b: Calculate the # of moles in 9.30 g of H2CO3: Ex1c: Calculate the equivalent weight of H2CO3: Ex1d: How many equivalents in 9.30 g of H2CO3? Ex1e: How many grams of H2CO3 would equal .290 equivalents? NIB - Normality In the past, we have used for concentration. M = moles / L A more useful form of concentration for acid/base reactions is Normality. N = Also, in calculating pH, normality is used instead of molarity. but, Normality is related to Molarity: N = Ex1: Calculate the Normality and Molarity if 1.80 g of H2C2O4 is dissolved in 150 mL of solution. Section 20.11 is not yet finished, but well finish it later. NIB problems involving mixing unequal amounts of acid and base Find the pH of a solution made by mixing 50.0 mL of .10 M HCl with 49.0 mL of .10 M NaOH Find the pH when mixing 50.0 mL of .10 M sulfuric acid with 50 mL of 1.0 M NaOH 19.2 Indicators Indicators: dyes where the color depends on the amount of ion present. They are used to show the of solutions. Indicators are usually made up of . The general formula is HIn ( H+ + In-1 Color 1 Color 2 (acid color) (base color) How do they work? If the solution is basic solution (lots of ): When an indicator is added, H+ from the indicator reacts with OH- to make . Now, all the H+ on the right side is . Since the equilibrium is disturbed (Le Chatelier), the reaction shifts to the . This makes more . More means more color. If the solution is acidic (lots of ): When the indicator is added to the solution, the high amount of H+ causes the equilibrium to shift . This makes more . More means more like the color. Indicators and colors to know: Phenolphthalein, Bromthymol Blue, Methyl Orange, Litmus Paper Indicators change over small ranges (Phenolphthalein changes 8.2 - 10.6) : pH range over which an indicator changes . 19.4 Acid Base Neutralization Acid + Base ( Ex1: Write the molecular, total ionic, and net ionic equations for the neutralization of HCl with NaOH. (molecular) (total ionic) (net ionic) Note: getting a perfect match of H3O+1 and OH-1 is next to impossible, so most neutral solutions are slightly acidic or basic. Ex2: Write the molecular, total ionic, and net ionic equations for the neutralization of H2SO4 with NaOH. (molecular) (total ionic) (net ionic) Acid Base Titration: The object of titration is to get the amount of to equal the amount of . Titration: the controlled addition of a solution of concentration to a solution of concentration. Standard Solution: the solution with a concentration. A graph of the titration of HCl with NaOH:   Titration Examples: Ex1: A 15.5 mL sample of .215 M KOH requires 21.2 mL of acetic acid to titrate to the end point. What is the Molarity of the acid? That was the difficult way. The easy way Normality and Titration: NaVa =NbVb Ex2: A 15.5 mL sample of .215 M KOH requires 21.2 mL of acetic acid to titrate to the end point. What is the Molarity of the acid? Ex3: If 15.7 mL of sulfuric acid is titrated to the end point by 17.4 mL of .0150 M NaOH, what is the Molarity of the acid? Percent problems: Ex4: If 18.75 mL of .750 N NaOH is required to titrate 20.30 mL of acetic acid, calculate the % acetic acid in solution. That was the difficult way. The easy way Ex5: If 18.75 mL of .750 N NaOH is required to titrate 20.30 mL of acetic acid, calculate the % acetic acid in solution. now lets go backwards Ex6: How many mL of a 1.20 % HCl solution are needed to titrate 25.50 mL of 0.100 M magnesium hydroxide? 19.5 Salts in Solution Hydrolysis the reaction of a substance with water acids acidic bases basic salts neutral? Sometimes, but they can lead to acidic/basic solutions hydrolysis of the salt of a strong base and weak acid NaC2H3O2 + H2O ! Na+ + C2H3O2-1 Since NaOH is a strong base, there is no attraction of sodium ion for the hydroxide ion produced from the self ionization of water, but& . C2H3O2-1 is the salt of a weak acid so H+ (from the self ionization of water) is attracted to the acetate ion. H+ + C2H3O2-1 ! HC2H3O2 Now since there is less H+, more H2O will self ionize creating more H+ (which will also get removed) and more OH-1 making the solution basic. Hydrolysis of the salt of a strong acid and weak base NH4Cl + H2O ! NH4+ + Cl-1 NH4+ + OH-1 ! H2O + NH3 so& hydroxide is taken out of solution. The equilibrium will shift when water self ionizes creating more OH- (which will also get removed) and more H+1 making the solution acidic. Hydrolysis of the salt of a weak base and weak acid (NH4)2CO3 - son of NH4OH and H2CO3 ( could produce a solution that is acidic, basic or neutral) NH4+ + OH-1 ! NH3 + H2O CO3-2 + H+1 ! HCO3-1 Since both of these reactions happen to some degree, it is hard to tell which happens more  therefore this solution can be acidic , basic, or neutral. Hydrolysis of the salt of a strong acid and strong base Cl-1 + H+1 does not yield HCl Na+1 + OH-1 does not yield NaOH Neither of these reactions happen because nature does not favor the production of strong acids/bases. Therefore, the amount of H+1 and OH-1 ions created from the self ionization of water does not change. A neutral solution results. What kind of solution would be produced by the hydrolysis of the following salts? 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