OMe ☆ OMe B 1. NaOMe/MeOH 2. H₂O* D Minimize

*** CALULATE FINL CONCENTRATION USING 2 IG FIGS AND APPROPRIATE UNITS A 6.0 mLmsample of a 50.0 % (mm/vv) acetic acid (HC2H3O2) solution is added to water to give a final volume of 34 mL.

10A Complete the figure below. Br NaCN DMSO B A NH₂ C 1. Br₂, NaOH 2. H₂O/H* TT. H₂SO4

Consider these compounds: A. CaSO4 B. CrPO4 C. CaF2 D. PbI2 Complete the following statements by entering the letter corresponding to the correct compound. Without doing any calculations it is possible to determine that nickel(II) carbonate is more soluble than ---------, and nickel(II) carbonate is less soluble than--------- It is not possible to determine whether nickel(II) carbonate is more or less soluble than ---------- by simply comparing Ksp values.

3. Determine the number of components in each of the following systems a. CH3COOH + CHẠOH + CH3COOC2Hs + H2O b. Aqueous solution of sodium acetate (NaC₂H5O₂)

Hydrobromic acid can be purchased as 50.0% solution. The density of this solution is 1.07 g mL-1. What is the molar concentration of hydrobromic acid in this solution? The molar concentration = i M

Which solution would you use to precipitate Mg2+ from an aqueous solution of MgCl2? KNO3 H3PO4 H2SO4 HC2H302

a) How many mL of concentrated HCl solution are needed to prepare 250 mL of a 0.36 M HCl solution? Concentrated HCl solution is 35.0% HCl by weight and has a density of 1.19 g/mL. (H: 1, Cl: 35.5 g/mol) b) To standardization of this hydrochloric acid solution, 0.2548 g of sodium carbonate requires 14.0 mL of HCl solution for titration to the equivalence point with methyl orange as indicator. What is the molarity of the HCl solution? (H:1, O:16, Cl: 35.5, Na: 23, C: 12 g/mol)

coulbonug9 oinihe olni bouogmoOB QU llaa of word Solubility Rules: Water Soluble Compounds EXSube sCHcood) or etosiq 1. Salts of ammonium (NH4*) and Group IA are always soluble. 2. Salts containing nitrate (N03-), acetate (C2H3O2-), or chlorate (CIO3-) ions are always soluble. enoiteo 1ol ooJ 3. Salts of the halides are soluble with the following exception: a. Compound containing Ag*, Hg2*, Pb²* prirdolaw Jon er Es i olnol the exception of: 4. Salts containing the sulfate ion (SO42-) are soluble elgmsx3 a. Compounds containing Ag*, Hg2*, Pb²+, Ca2*, Sr2*, or Ba2+ Water Insoluble Compounds Juloe ent! 1. Salts of the carbonate (CO32-), phosphate (PO43-), chromate (CrO42-), or sulfides (S2-) ions are insoluble with the exception of compound containing group 1A or ammonium cations. 2. Salts containing the hydroxide ion (OH-) are insoluble with the exception of compounds containing group 1A, ammonium cations, or Ba2+. biup Inot luo tneioliteoo belon Soluble means that it dissolves in water…

Potassium nitrate (KNO3) occurs naturally as the mineral saltpeter in Italy, and many other places. It is easy to mine, and highly endothermic when it is dissolved in water. Because of this, members of the Roman nobility often dissolved saltpeter in large urn when they had parties. Which of the following is the most likely application of this technology? Oa. a. The Romans used saltpeter to chill their wine. Ob. The Romans used saltpeter to light their dining halls. Oc. The Romans used saltpeter to cook their fish course. Od. The Romans used saltpeter as a warm soak for their guests' feet.