{[ promptMessage ]}

Bookmark it

{[ promptMessage ]}

chem test 3 notes - Chapter 17 The Chemistry of Acids and...

Info icon This preview shows pages 1–2. Sign up to view the full content.

View Full Document Right Arrow Icon
Chapter 17: The Chemistry of Acids and Bases Acids or bases that ionize extensively (K>1) are strong Acids or bases that don’t ionize extensively (K<1) are weak Brønsted: an acid is any substance that can donate a proton; HF, HCl, HNO3, CH3CO2H, HSO4 Brønsted: a base is a substance that can accept a proton Monoprotic acid: donate one proton Polyprotic acid: capable of donating two or more protons Polyprotic base: accept more than one proton; SO4, PO4, CO3, C2O4 Brønsted amphiprotic: can act as either an acid or base; HPO4, H2O Conjugate Acid-Base Pairs: a pair of compounds or ions that differ by the presence of one H+ ion Name Acid 1 Base 2 Conj. base Conj. acid Hydrochloric acid HCl + H O > Cl + H O Nitric acid HNO + H O > NO ₃⁻ + H O Hydrogen carbonate HCO ₃⁻ + H O <> CO ² + H O Acetic acid CH CO H + H O <> CH CO + H O Hydrocyanic acid HCN + H O <> CN + H O Hydrogen sulfide H S + H O <> HS + H O Ammonia H O + NH <> OH + NH ₄⁺ Carbonate ion H O + CO <> OH + HCO ₃⁻ Water H O + H O <> OH + H O Autoionization: two water molecules interact to produce hydronium and hydroxide ions; K= [H O ][ OH ]/[ H O] ² Kw=[H O ][ OH ]=1.0x10 ¹ ⁻ ⁴ In a neutral solution [H O ]=[ OH ]=1.0x10 ⁻⁷ In an acidic solution [H O ]>[ OH ] In a basic solution [H O ]<[ OH ] pH: the negative log of the hydronium ion concentration; pH=-log[H O ]
Image of page 1

Info icon This preview has intentionally blurred sections. Sign up to view the full version.

View Full Document Right Arrow Icon
Image of page 2
This is the end of the preview. Sign up to access the rest of the document.

{[ snackBarMessage ]}