Acids+&+Bases

__**Directions:**__ a) list and define all vocabulary from the chapter b) type at least 4 sample problems with step-by-step directions of how to solve the problem; list the correct answers (if your chapter doesn't have math, there are still problems and concepts we learned.) c) link at least 3 websites for additional resources to help with studying d) develop your own LEQ questions for the section - what did you think were the key points we learned? e) Once your page is done, visit 4 other chapters and answer their LEQ's. (This can be done on a separate piece of paper.)

a) Acid - pH from 0-7
Base - pH from 7-14 Neutral - pH of 7 Arrheinius Acid - A compound that has an H+ Arrheinius Base - Compound that OH- Bronsted-Lowry Acid - H+ donor Bronsted-Lowry Base - H+ acceptor Lewis Acid - Accepts e- Lewis Base - Donate e- Strong Acid - Lowest pH Weak Acid - pH less to 7 but close to it Strong Base - Highest pH Weak Base - pH greater than 7 but close to it pH - the measure of the acidity of a solution pOH - the opposite of pH, whatever adds up to 14 with the pH

b) Identify the pH, pOH, [H3O+], [OH-] 1) A 0.001 M solution of HCl. [H3O+]: 0.001M pH: 3 [OH-]: 10^-11 pOH: 11 2) 792 mL of a solution containing .344 grams of hydrochloric acid. [H3O+]: 0.0119M pH: 1.92 [OH-]: 10^-12.08 pOH: 12.08 3) 8.7 L of a solution containing 1.1 grams of nitric acid. [H3O+]: .002M pH:2.70 [OH-]: 10^-11.30 pOH:11.30 4) 10.7 L of a solution containing .01 grams of hydrochloric acid. [H3O+]: 0.00025M pH:4.60 [OH-]: 10^-9.40 pOH:9.40

EXPLANATION: Get your units into Mols per Liter by converting if necessary. The H3O+ is the Molarity of the solution, to find the pH you must take the negative log of the H3O+, after you find the pH you subtract that by 14 to get the pOH, then to find the OH- you take ten and raise it to the power of the negative pOH.

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d) How do you solve to find the pH of compounds and how do you determine what is a weak and strong acid?