a) Select any two items off the diagram above and list their pH level:pH LevelpH LevelItem #1Item #2How many times as acidic is Item #1 than Item #2?b) One particular solution has a pH of 3.6. Its hydrogen ion concentrationis twice as high as another solutions hydrogen ion concentration. Whatcould both solutions possibly be? In chemistry, the pH scale measures the acidity of a solution. Solutions with pH lessthan 7 are considered acidic, while solutions with pH greater than 7 are consideredalkaline. A pH of 7 is considered neutral. The formula of pH is pH = -logx, wherex represents the concentration of hydrogen ions in mol/L. Below is a diagram thatconveys the pH of a few common foods and chemicals:ACIDICNEUTRALBASIC OR ALKALINE1234.6791011121314Battery AcidStomach Acid - 1.0Lime Juice - 1.8-2.0Vinegar- 2.0-3.4Lemon Juice – 2.2-2.4Coca-Cola - 2.5Cider – 2.9-3.3Strawberries - 3.0-3.5Yeasts - 3.0-3.5Jams/Jellies - 3.1-3.5Apples- 3.3-4.0Honey - 3.9Tomatoes – 4.2-4.1Sugar – 5.0-6.0Beef - 5.1-6.2Pork - 5.3-6.9Onions - 5.3-5.8Lettuce - 5.8-6.0Rice - 6.0-6.7Butter - 6.1-6.48g Yolk - 6.4Pure Water - 7.0Milk – 6.3-8.5Crackers - 7.0-8.5Egg White - 7.0-9.0Baking Soda - 9.0AntacidsAmmoniaCalcium HydroxideLyePotassium Hydroxide

The diagram and the pH scale is given as:

a) Select any two items off the diagram above and list their pH level: pH Level pH Level Item #1 Item #2 How many times as acidic is Item #1 than Item #2? b) One particular solution has a pH of 3.6. Its hydrogen ion concentration is twice as high as another solutions hydrogen ion concentration. What could both solutions possibly be?

a) Select any two items off the diagram above and list their pH level: pH Level pH Level Item #1 Item #2 How many times as acidic is Item #1 than Item #2? b) One particular solution has a pH of 3.6. Its hydrogen ion concentration is twice as high as another solutions hydrogen ion concentration. What could both solutions possibly be?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 6RQ: Two strategies are also followed when solving for the pH of a base in water. What is the strategy...

See similar textbooks

Similar questions

A solution of sodium cyanide, NaCN, has a pH of 12.10. How many grams of NaCN are in 425 mL of a solution with the same pH?
Follow the directions of Question 19 for the following acids: (a) hypochlorous acid (b) formic acid, HCHO2 (c) acetic acid, HC2H3O2 (d) hydrobromic acid (e) sulfurous acid
Assuming that the conductivity of an acid solution is proportional to the concentration of H3O+, sketch plots of conductivity versus concentration for HCl and HF over the 0- to 0.020 M concentration range.
12.62 Write the formula of the conjugate acid of each of the following bases, (a) OH-, (b) NHj, (c) CHjNHt, (d) HPO/-, (e) CO.,2’
Two strategies are also followed when solving for the pH of a base in water. What is the strategy for calculating the pH of a strong base in water? List the strong bases mentioned in the text that should be committed to memory. Why is calculating the pH of Ca(OH)2 solutions a little more difficult than calculating the pH of NaOH solutions? Most bases are weak bases. The presence of what element most commonly results in basic properties for an organic compound? What is present on this element in compounds that allows it to accept a proton? Table 13-3 and Appendix 5 of the text list Kb values for some weak bases. What strategy is used to solve for the pH of a weak base in water? What assumptions are made when solving for the pH of weak base solutions? If the 5% rule fails, how do you calculate the pH of a weak base in water?
Explain the difference between a monoprotic acid, a diprotic acid, and a triprotic acid. Give an example of each.
3.102 Classify the following compounds as acids or bases, weak or strong. (a) perchloric acid, (b) cesium hydroxide, (c) carbonic acid, H2CO3, (d) ethylamine, C2H5NH2
Acids You make a solution by dissolving 0.0010 mol of HCl in enough water to make 1.0 L of solution. a Write the chemical equation for the reaction of HCl(aq) and water. b Without performing calculations, give a rough estimate of the pH of the HCl solution. Justify your answer. c Calculate the H3O+ concentration and the pH of the solution. d Is there any concentration of the base OH present in this solution of HCl(aq)? If so, where did it come from? e If you increase the OH concentration of the solution by adding NaOH, does the H3O+ concentration change? If you think it does, explain why this change occurs and whether the H3O+ concentration increases or decreases. f If you were to measure the pH of 10 drops of the original HCl solution, would you expect it to be different from the pH of the entire sample? Explain. g Explain how two different volumes of your original HCl solution can have the same pH yet contain different moles of H3O+. h If 1.0 L of pure water were added to the HCl solution, would this have any impact on the pH? Explain.
Write two BrnstedLowry acid-base reactions and show how they represent proton-transfer reactions.
Which of the following conditions indicate an acidic solution? pH = 3.04 (H+| > 1.0 X IO’7 A/ pOH = 4.51 |OH-J = 3.21 X 10"12 M
The elements sodium, aluminum, and chlorine are in the same period.. (a) Which has the greatest electronegativity?. (b) Which of the atoms is smallest?. (c) Write the Lewis structure for the simplest covalent compound that can form between aluminum and chlorine. (d) Will the oxide of each element be acidic, basic, or amphoteric?
Leucine is an amino acid with this Lewis structure: Write the Lewis structure for the zwitterion form of leucine.