Exam 2 Cheat Sheet Ch.4-6

Exam 2 Cheat Sheet Ch.4-6 - Avogadro's = 6.022 x 1023 1 mL...

Info iconThis preview shows page 1. Sign up to view the full content.

View Full Document Right Arrow Icon
Avogadro’s # = 6.022 x 10 23 1 mL = 1 cm 3 Kelvins = C + 273.15 F = 9/5 x C +32 C = 5/9 (F – 32) Ionic Equation shows break down of compounds – polyatomics are together. Net Ionic cancels out some (spectators) to show precipitate and both reactants only. % comp. = # moles x molar mass of element x 100 Molar mass of compound Unknown -Find the % comp. of element in known compound. Take %, convert to 0. and multiply by given mass of known compound. Take that # & plug it for numerator into % comp formula with given unknown’s mass on bottom. Molarity = moles of solute Liters of solution Titration- Whatever element needs concent. found, convert the given grams to mol. Than # goes in numerator in molarity equation. Mol/L = M MiVi = MfVf Bronsted acid- proton donor NH 4 + ammonium H 2 PO 3 - dihydrogen phosphite H 3 O + hydronium H 2 PO 4 - dihydrogen phosphate Hg 2 2+ mercury(I) HCO 3 - hydrogen carbonate CNO - cyanate HSO 3 - hydrogen sulfite CNS - thiocyanate HSO 4 - hydrogen sulfate MnO 4 -
Background image of page 1
This is the end of the preview. Sign up to access the rest of the document.

This note was uploaded on 04/07/2008 for the course CHEM 111 taught by Professor Stauffer during the Fall '08 term at Pittsburgh.

Ask a homework question - tutors are online