<p>ACID/BASE PROBLEM SET Name______Hr___ pH of Solutions 1. What is the pH scale?</p><p>2. What is the pH range for acids? ______bases?______</p><p>3. Arrange these groups in order from the most acidic to the most basic. The pH of each item is listed. a) bleach: 12.0, lemons: 2.3, milk of magnesia: 10.5, urine: 6.0, blood: 7.4 </p><p>Arrange these groups in order from the most basic to the most acidic. The pH of each item is listed. b) 1.0M NaOH: 14.0, seawater: 8.5, bananas: 4.6, 1.0M HCl: 0, tap water: 7.2 </p><p>4. Why is pure water considered neutral on the pH scale?</p><p>5. Classify each of the following as acidic, neutral, or basic. The pH of each item is listed. a) tomatoes, 4.2 ______d) soil, 5.5 ______b) eggs, 7.8 ______e) milk, 6.4 ______c) ammonia, 11.0 ______f) baking soda, 9.5 ______</p><p>6. Name each of the following acids and bases: </p><p> a) HCl ______f) NaOH ______</p><p> b) HNO3 ______g) KOH ______</p><p> c) H2SO4 ______h) HC2H3O2 ______</p><p> d) NH3 ______i) H3PO4 ______</p><p> e) H2CO3 ______j) Mg(OH)2 ______</p><p>7. a) Which of the above is the acid used in car batteries? ______b) Which of the above is stomach acid? ______c) Which of the above “acts upon copper”? ______d) Which of the above is commonly known as vinegar? ______e) Which of the above is the active ingredient in Drain-o, a.k.a. ‘lye’? ______f) Which of the above acids are found in soda? ______and ______g) Which of the above is used as a glass cleaner? ______pH & pOH 1. What is pH a measure of? ______</p><p>2. What is the equation used for finding pH? ______3. What is the equation that relates to pH and pOH? ______4. Are the following solutions acidic, neutral, or basic? </p><p> a) [H+] = 1 x 10-8 M ______d) [H+] = 0.1 M ______b) [OH-] = 1 x 10-10 M ______e) [H+] = 1 x 10-5 M ______c) [OH-] = 1 x 10-6 M ______f) [OH-] = 0.00001 M ______</p><p> g) Complete the following table:</p><p>+ - acidic, basic, or [H ] [OH ] pH pOH neutral 1.0 x 10-3 M 1.0 x 10-11 M 3 11 Acidic</p><p>1.0 x 10-5</p><p>6.37</p><p>0.045</p><p>0.00000096</p><p>4.31</p><p>7.00</p><p>5. What is the pH of each of the following? a) 0.0010 M HCl ______g) 0.024 M HCl ______</p><p> b) 0.0010 M HNO3 ______h) 0.075 M KOH ______c) 0.010 M NaOH ______i) 0.000034 M HCl ______d) 0.0035 M HCl ______j) 0.0001M HCl ______</p><p>6) What is the pH and pOH of a 1.20 x 10-3 M HBr solution?</p><p>7) What is the pH and pOH of a 2.34 x 10-5 M NaOH solution?</p><p>8) What is the pH and pOH of 120.0mL of a solution containing 0.00500grams of hydrochloric acid?</p><p>9) What is the pH and pOH of 660.0L of a solution containing 0.00740moles of nitric acid? 10) What is the pH and pOH of a solution made by adding water to 15.0 grams of hydroiodic acid (HI) until the volume of the solution is 2500.0 mL?</p><p>11) What is the pH and pOH of a solution that was made by adding 400.0 mL of water to 350.0 mL of 5.00 x 10-3 M NaOH solution?</p><p>12) What is the pH and pOH of a solution with a volume of 5.04 L that contains 15.0 grams of hydrochloric acid and 25.0 grams of nitric acid?</p><p>Brønsted-Lowry Acids and Bases 1. What is the Brønsted definition of an acid? ______2. What is the Brønsted definition of a base? ______</p><p>+ 3. What is the correct name for the H3O ion? ______4. Determine the conjugate base for the following acids:</p><p>-1 +1 HF: ______HNO2 : ______NH4 : ______H2O: ______H3PO4: ______5. Determine the conjugate acid for the following bases:</p><p>OH-1: ______Br -1: ______NH3: ______H2O: ______CO3 -2: ______6. Identify the conjugate acid/base pairs in the following reactions:</p><p>+1 -1 a) HCN + H2O <---> H3O + CN acid:______base: ______conjugate base: ______conjugate acid: ______</p><p>-1 -2 +1 b) H2O + HSO4 <---> SO4 + H3O acid: ______base: ______conjugate base: ______conjugate acid: ______</p><p>7. Write the equation for the hydrolysis of HNO2 (a weak acid) in water, labeling each acid/base pair:</p><p>8. Write the equation for the hydrolysis of NH3 (a weak base) in water, labeling each acid/base pair: 9. Some acids have a unique property: the ability to donate more than one proton (H+) per molecule. A molecule that can donate 1 proton is called a monoprotic acid. Example = ______A molecule that donates 2 protons is a ____protic acid. Example = ______A molecule that donates 3 protons is called a _____protic acid. Example = ______</p><p>Ionization 1. Describe what occurs when water ionizes (“self-ionization of water”). Include an equation and an explanation.</p><p>2. What are the molar concentrations of [H+] and [OH-] in pure water at 25°C?</p><p>3. What is the ion-product constant, Kw? ______</p><p>4. Find [H+] for solutions having the following [OH-] value: a) [OH-] = 1 x 10-13 b) [OH-] = 2.7 x 10- 4 c) [OH-] = 1 x 10- 3 d) [OH-] = 6.3 x 10-10 5. Calculate [OH-] of a solution when its [H+] has the following values: a) [H+] = 1 x 10-13 b) [H+] = 3.6 x 10- 5 c) [H+] = 1 x 10- 2 d) [H+] = 7.8 x 10- 8</p><p>6. A solution contains 0.635 g NaOH in 236 mL solution. a) Write the equation for the dissociation of NaOH:</p><p> b) What is the [OH-]?</p><p> c) What is the [H+]?</p><p>7. A solution contains 0.737 g HNO3 in 934 mL solution. a) Write the equation for the dissociation of HNO3:</p><p> b) What is the [H+]?</p><p> c) What is the [OH-]?</p>