{[ promptMessage ]}

Bookmark it

{[ promptMessage ]}

11 - usually start with volume of liquid given 115 mL...

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

View Full Document Right Arrow Icon
Percent yield: Actual/theoretical x 100% All reactions usually occur in water Solution: homogenous ( purely visual) mixture Solvent: the majority solution component, retains its state Solute: the minority solution component, becomes the state of the solvent Salt: any ionic compound or NaCl Ex. For bronze, copper is solvent and solute is tin For wine, solvent is water, solute is alcohol Molarity (M) is moles of solute/ liters of solution Molarity calculations: Ex: determine molarity of 45.5 mg of NaCl is dissolved in enough solvent to make 154.4 mL of solution (45.5 mg NaCl/154.4 mL solution) x (1000 mL sol/ 1 L sol) x (1 g NaCl/1000 mg NaCl) x (I mol NaCl/58.44 g NaCl) = 5.04 x 10^-3 M how many mol of Cl- ions are contained in 114 mL of a 1.85 M CaCl2 solution?
Background image of page 1

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

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

Unformatted text preview: usually start with volume of liquid given 115 mL solution x (1 L/ 1000 mL) x (1.85 mol CaCl2/ 1 L sol) x (2 mol Cl-/ 1 mol CaCl2) = 0.422 mol Cl- electrolyte ionizes to some extent what dissolves in water nonelectrolytes dissolve in water but don’t ionize strong salts: NaCl, KBr, LiNO3, strong acids: HCl, HNO3, H2SO4, HClO4 strong bases: NaOH, KOH weak electrolyte only slightly ionizes in water ex: HC2H3O2 and NH3 dissolution occurs if interactions between solvent and solute particles overcome interactions of the solute to itself just because a compound is ionic doesn’t automatically mean it dissolves in water (ch 16) predict this based on structure...
View Full Document

{[ snackBarMessage ]}