7th Edition

ISBN: 9781119513216

Author: HYSLOP

Publisher: JOHN WILEY+SONS INC.

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Textbook Question

Chapter 16, Problem 169RQ

What would our pH scale look like if Arrhenius decided that pH = —ln [ H + ] ? What would the pH of a neutral solution be?

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Chapter 16, Problem 168RQ

Chapter 17, Problem 1PE

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In chemistry, the pH scale measures the acidity of a solution. Solutions with pH less than 7 are considered acidic, while solutions with pH greater than 7 are considered alkaline. A pH of 7 is considered neutral. The formula of pH is pH = -logx, where x represents the concentration of hydrogen ions in mol/L. Below is a diagram that conveys the pH of a few common foods and chemicals: ACIDIC NEUTRAL BASIC OR ALKALINE 1 2 3 4. 6 7 9 10 11 12 13 14 Battery Acid Stomach Acid - 1.0 Lime Juice - 1.8-2.0 Vinegar- 2.0-3.4 Lemon Juice – 2.2-2.4 Coca-Cola - 2.5 Cider – 2.9-3.3 Strawberries - 3.0-3.5 Yeasts - 3.0-3.5 Jams/Jellies - 3.1-3.5 Apples- 3.3-4.0 Honey - 3.9 Tomatoes – 4.2-4.1 Sugar – 5.0-6.0 Beef - 5.1-6.2 Pork - 5.3-6.9 Onions - 5.3-5.8 Lettuce - 5.8-6.0 Rice - 6.0-6.7 Butter - 6.1-6.4 8g Yolk - 6.4 Pure Water - 7.0 Milk – 6.3-8.5 Crackers - 7.0-8.5 Egg White - 7.0-9.0 Baking Soda - 9.0 Antacids Ammonia Calcium Hydroxide Lye Potassium Hydroxide

It turns out that Ba(OH)2 is also considered a strong base. What is the [OH-] concentration in 0.34 M Ba(OH)2(aq) solution?

Hydroiodic acid often is used to disinfect and sanitize medical tools and products. In an experiment, 5.0 mL of 0.75 mol/L HI(aq) is mixed with 20.0 mL of distilled water. (record only your final answer with the correct number of significant digits and the proper units.) 1. What is the hydronium ion concentration of the resulting diluted solution? 2. What is the pH of the resulting solution? 3. If 1.0 mL of the diluted solution is added to 9.0 mL of distilled water, what is the resulting pH of the solution? 4. If 1.0 mL of the diluted solution from #3 is added to 9.0 mL of distilled water, you should be able to predict the pH based on the trend you see and without doing any calculations. This is because every time the hydronium concentration a) increases b)decreases by a factor of 10, the pH goes up one full unit since the solution becomes a)more b)less acidic.

Chapter 16 Solutions

EBK CHEMISTRY: THE MOLECULAR NATURE OF

Ch. 16 - Prob. 1PE Ch. 16 - Practice Exercise 16.2 An aqueous solution of...Ch. 16 - Practice Exercise 16.3 Water draining from old...Ch. 16 - Because rain washes pollutants out of the air, the...Ch. 16 - Practice Exercise 16.5 Find the values of and ...Ch. 16 - Practice Exercise 16.6 Calculate the . (Hint: is...Ch. 16 - Practice Exercise 16.7 Calculate the , and pH in a...Ch. 16 - For each of the following acids, write the...Ch. 16 - For each of the following acids, write the...Ch. 16 - Practice Exercise 16.10 Use Table 16.2 to find all...

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