Acid and Base Review Game Chemistry

Name the Acid HNO2 H2SO4 HCl HBr HClO Nitrous Acid Sulfuric Acid Hydrochloric Acid HBr Hydrobromic Acid HClO Hypochlorous Acid

NaOH Ca(OH)2 Mg(OH)2 KOH Name the Base Sodium Hydroxide Calcium Hydroxide Mg(OH)2 Magnesium Hydroxide KOH Potassium Hydroxide

Nitric Acid Hydroiodidic Acid Phosphoric Acid Acetic Acid Write the Formula Nitric Acid HNO3 Hydroiodidic Acid HI Phosphoric Acid H3PO4 Acetic Acid HC2H3O2

Sodium carbonate Barium hydroxide Lithium hydroxide Write the Formula Na2CO3 Barium hydroxide Ba(OH)2 Lithium hydroxide LiOH

What is the definition of an acid? What is the definition of a base? Arrhenius What is the definition of an acid? A substance which produces H+ when put in water What is the definition of a base? A substance which produces OH- when put in water

Bronsted-Lowry – Label acid, base, conjugate acid, conjugate base H3PO4 + NO2-  HNO2 + H2PO4- Acid Base CA CB CN- + HCO3-  HCN + CO3-2 B A CA CB HCN + SO3-2  HSO3- + CN- A B CA CB H2O + HF  F- + H3O+ B A CB CA

If a soap has a hydrogen ion concentration of 2 If a soap has a hydrogen ion concentration of 2.0 x 10-6 M, what is the pH of the solution? The pOH? Is it an acid or a base? [H+] = 2 x 10-6M pH = -log(2 x 10-6) = 5.7 pOH = 14 – 5.7 = 8.3 Acid because pH < 7

What is the hydrogen ion concentration and hydroxide ion concentration of a solution with a pH of 2.3? Is the substance an acid or base? [H+] = 10-2.3 = 0.0050 M pOH = 14 – 2.3 = 11.7 [OH-] = 10-11.7 = 2.0 x 10-12 M Acid because pH < 7

What is the hydrogen ion concentration of a sample of phosphoric acid that has a pH of 4.9? What is the concentration of phosphoric acid? [H+] = 10-4.9 = 1.3 x 10-5M Since there are 3 H’s in each H3PO4 … the concentration of phosphoric acid would be a third of the concentration of H+ 1.3 x 10-5/3 = 4.2 x 10-6 M

Neutralization Reaction What is the neutralization reaction for nitrous acid reacting with potassium hydroxide? HNO2 + KOH  KNO2 + H2O

Neutralization Reaction Write the complete balanced equation for the neutralization of phosphoric acid with calcium hydroxide 2H3PO4 + 3Ca(OH)2  Ca3(PO4)2 + 6H2O

Write the ionization reaction for hydrophosphoric acid in water H3P + H2O  H2P- + H3O+

How many grams of copper (II) sulfate pentahydrate will be needed to make 75 mL of a 0.250 M solution? CM = n/V .25 = n/0.075 n = 0.01875 mol CuSO4 . 5H2O x 249.5 = 4.7 g

How many kilograms of sucrose C12H22O11 will be needed to make 3 How many kilograms of sucrose C12H22O11 will be needed to make 3.50 L of a 1.15 M solution? CM = n/v 1.15 = n/3.5 n = 4.025 mol x 342 = 1376.55 g / 1000 = 1.38 kg

What is the pH of a solution made with 0 What is the pH of a solution made with 0.15 grams of barium hydroxide in 4500 mL of water? 0.15 grams Ba(OH)2 / 171 = 8.77 x 10-4 mol / 4.5L = 1.95 x 10-4M [OH-] = 2(1.95 x 10-4)= 3.9 x 10-4 M pOH = -log (3.9 x 10-4) = 3.4 pH = 14 – 3.4 = 10.6

What is the molar concentration of a solution that contains 0 What is the molar concentration of a solution that contains 0.0750 moles of NaHCO3 in a volume of 115 mL CM = n/v CM = 0.075/.115 = 0.652 M

A solution has 3. 00 moles of solute in 2 A solution has 3.00 moles of solute in 2.00 L of solution, what is its molar concentration? How many moles would there be in 350 mL of solution? CM = n/V CM = 3/2 = 1.5M 1.5 = n/0.35 n = 0.53 mol

Describe in your own words how you would prepare 1. 00L of a 0 Describe in your own words how you would prepare 1.00L of a 0.850 M solution of formic acid HCO2H? CM = n/v 0.85 = n/1 n = 0.85 mol x 46 = 39.1 g Take 39.1 grams of formic acid and dissolve in approximately 250 mL of water. Put into a 1.00 L volumetric flask and fill to the line with water

What is the molarity of a sulfuric acid solution which contains 5 What is the molarity of a sulfuric acid solution which contains 5.4 grams of sulfuric acid in 250 mL of water? What is the normality? 5.4g/98 = 0.055 mol CM = 0.055/0.25 = 0.22 M N = (eq)M = 2 x 0.22 = 0.44 N

What is the molarity of a potassium hydroxide solution which contains 0.94 moles of potassium hydroxide in 450 mL of water? What is the normality? CM = 0.94/0.45 = 2.1 M N = (eq)M = 1 x 2.1 = 2.1 N

In the titration of 35.0 mL of liquid drain cleaner containing NaOH, 50.0 mL of 0.400M H2SO3 must be added to reach the equivalence point. What is the molarity of the base in the cleaner? NaVa = NbVb (0.4)(2)(50) = Nb(35) Nb = 1.14 N / 1 = 1.14 M

Calculate how many milliliters of 0 Calculate how many milliliters of 0.250 M Ba(OH)2 must be added to titrate 46.0 mL of 0.400 M HClO4 NaVa = NbVb 0.4(46) = 0.5Vb Vb = 36.8 mL

A 15.5 mL sample of 0.215 M KOH was titrated with an acetic acid solution, It took 21.2 mL of the acid to reach the equivalence point. What is the molarity of the acetic acid? (0.215)(15.5) = Na(21.2) Na = 0.157 N / 1 = 0.157 M

What is the molarity of a solution of phosphoric acid with a pH of 2 [H+] = 10-2.65 = 2.24 x 10-3M [H3PO4] = 2.24 x 10-3 / 3 = 7.47 x 10-4M

A 20. mL sample of an HCl solution was titrated with 27 A 20. mL sample of an HCl solution was titrated with 27.4 mL of a standard solution of Ba(OH)2. The concentration of the standard is 0.0154 M. What is the molarity of the HCl? (0.0308)(27.4) = Na(20) Na = 0.042N / 1 = 0.042M

Buffer What is a buffer? A solution that resists changes in pH

What are buffers made of? Where can you find them? Weak acid and its conjugate base Weak base and its conjugate acid You can find them in your BLOOD

I want to dilute 20. 0 mL of a 6. 00M solution of acetic acid to a 3 I want to dilute 20.0 mL of a 6.00M solution of acetic acid to a 3.80M solution of acetic acid. How much water should I add to the 6.00M acetic acid to achieve this? 6(20) = 3.8V V = 31.6 mL ADD 11.6 mL of water

I mix 20. mL of 4. 5M NaCl with 40. mL of water I mix 20. mL of 4.5M NaCl with 40. mL of water. What is the new concentration of the NaCl? 4.5(20) = M(60) M = 1.5 M

A 450 mL solution of 1. 5 M HCl is sat out over night A 450 mL solution of 1.5 M HCl is sat out over night. 150 mL of the water evaporated. What is the new concentration of the HCl? 1.5 (450) = M (300) 2.3 M

What does the term “strong acid” mean? Strong acid means that the acid dissociates completely in water

I used 50. 0 grams of potassium chromate to make a 1. 40M solution I used 50.0 grams of potassium chromate to make a 1.40M solution. What is the volume of the solution? 50 g K2CrO4 / 194 = 0.26 mol 1.4 = .26/v V = 0.184 L

What is the pH of a solution made by putting 6 What is the pH of a solution made by putting 6.0 grams of phosphoric acid in 250 L of water? 6 g H3PO4 / 98 = 0.0612 mol [H3PO4] = 0.0612 / 250 = 2.45 x 10-4 [H+] = 3(2.45 x 10-4) = 7.35 x 10-4 pH = -log(7.35 x 10-4) = 3.1

What is the pH of a solution made by putting 3 What is the pH of a solution made by putting 3.25 grams of strontium hydroxide in 5000. L of water? 3.25 g Sr(OH)2 / 121.6 = 0.0267 mol [Sr(OH)2] = 0.0267/ 5000 = 5.34 x 10-6M [OH-] = 2(5.34 x 10-6) = 1.07 x 10-5 M pOH = -log(1.07 x 10-5) = 4.97 pH = 14 – 4.97 = 9.03