The pH scale ranges from 0-14. Why do we choose to use this scale to represent hydrogen ion concentration in a solution? How do we convert hydrogen ion concentration into this scale? What does a low number on the pH scale mean? High? Between which numbers do biological reactions take place?

In the following neutralization reaction, label each compound as the Arrhenius acid, Arrhenius base, salt or water. Mg(OH)2 + HCI MgCl2 + H2O Format BIU

Consider the following data on some weak acids and weak bases: name acetic acid hydrofluoric acid acid solution 0.1 M KCH3CO₂ 0.1 M CH3NH3Br 0.1 M NaI 0.1 M NaF Ka formula HCH3CO₂ 1.8 x 10 HF 6.8 × 10 Use this data to rank the following solutions in order of increasing pH. In other words, select a '1' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. X -4 pH choose one choose one choose one choose one base Ś Kb formula methylamine CH3NH₂ 4.4 x 107 CHN 1.7×10 9 name pyridine

What pH range is considered to be acidic? Basic? Neutral? Which pollutants are responsible for acid rain? Where do they come from?

Order these chemical species by increasing pH of an 0.1 M aqueous solution of each. That is, imagine making an 0.1 M solution of each species. Select 1 next to the species that makes the solution with the lowest pH. Select 2 next to the species that makes the solution with the next higher pH, and so on. Notice that some of the rankings have been filled in for you already. Also notice that water is on the list. For that particular case, just compare the pH of pure water to the pH of the other solutions. Note for advanced students: for all charged species, you may assume the necessary counterions act as neither acids nor bases. species + H₂O* HCIO2 HCOOH HCOO H₂O 2- SO 4 CIO₂ HSO4 relative pH of 0.1 M aqueous solution (Choose one) 3 (Choose one) ▼ 8 (highest) 5 (Choose one) (Choose one) 2 X Ś ? 000 Ar

Order these chemical species by increasing pH of an 0.1 M aqueous solution of each. That is, imagine making an 0.1 M solution of each species. Select 1 next to the species that makes the solution with the lowest pH. Select 2 next to the species that makes the solution with the next higher pH, and so on. Notice that some of the rankings have been filled in for you already. Also notice that water is on the list. For that particular case, just compare the pH of pure water to the pH of the other solutions. Note for advanced students: for all charged species, you may assume the necessary counterions act as neither acids nor bases. species ОН HIO H₂O CH₂CICOO CH₂CICOOH CH₂O ΙΟ CH₂OH relative pH of 0.1 M aqueous solution 8 (highest) (Choose one) (Choose one) (Choose one) 1 (lowest) (Choose one) 7 2 X Ś

Order these chemical species by increasing pH of an 0.1 M aqueous solution of each. That is, imagine making an 0.1 M solution of each species. Select 1 next to the species that makes the solution with the lowest pH. Select 2 next to the species that makes the solution with the next higher pH, and so on. Notice that some of the rankings have been filled in for you already. Also notice that water is on the list. For that particular case, just compare the pH of pure water to the pH of the other solutions. Note for advanced students: for all charged species, you may assume the necessary counterions act as neither acids nor bases. species ОН IO C10₂ HCOOH HCIO₂ HIO HCOO relative pH of 0.1 M aqueous solution (Choose one) 7 (Choose one) 2 1 (lowest) (Choose one) (Choose one) X Ś olo 18 Ar

A chemist dissolves 715. mg of pure sodium hydroxide in enough water to make up 110. mL of solution. Calculate the pH of the solution. (The temperature of the solution is 25 °C.) Round your answer to 3 significant decimal places.

Let's say you are doing an experiment that has you measuring the pH values of different substances. When comparing your data you notice that the value you got for the pH is not the same when comparing it to the pH chart. What could have caused the difference in the values you got and what is on the pH chart?

Consider the following data on some weak acids and weak bases: base acid K₁ name formula name formula nitrous acid HNO₂ 4.5 × 10 4 hypochlorous acid HC1O 3.0 × 108 ammonia aniline C6H5NH24.3 × 10-10 NH, 1.8 × 10-5 Use this data to rank the following solutions in order of increasing pH. In other words, select a '1' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. solution PH 0.1 M KCIO choose one 0.1 M NH4Cl choose one 0.1 M KBr choose one 0.1 M C6H5NH3Br choose one G