PPT-Molarity or Concentration

Water as a Polar Solvent Water is a polar molecule since it has uneven electron distribution and a bent molecular shape Due to its polar nature water interacts strongly with its solutes and often plays an active role in aqueous reactions. CllibdMli C a l at on M o l theconcentrationofchemicalsinsolution. the of solution. Thedefinitionofmolarityis: of Molarity M Molesofsolute Molarity Litersofsolution using molarity. If I have 0.075 m n V C = concentration (moles/L= molarity) V = volume of solution in L 1. In 10.0 mL of a certain solution, there are 0.050 g of KF. Find the molarity of the solution (moles/L) 0.050 g KF(mole/ 2. Molarity The concentration of a solution is a measure of the amount of solute that is dissolved in a given quantity of solvent. – A dilute solution is one that contains a small amount of Solutions. A.  . solution.  . is a homogeneous mixture of two or more substance. A solution is generally composed of two substances. Solute: substance that is being dissolved and is in smaller quantity. Units of Concentration . Molality (. m. ) . aka “. molal. concentration”. . Solvent= does not include solute. Molarity (. M. ) . aka “molar concentration”. Most common concentration unit in Chemistry. Ch. . 10– . The Mole. Molarity. Concentration of a solution.. total combined volume. substance being dissolved. Molarity. 2. M HCl. What does this mean?. Molarity. . Calculations. molar mass. (. g/mol. Assign oxidation numbers. Which is being oxidised? Reduced?. Which is the oxidising agent/ reducing agent?. . I. 2(. aq. ) . + 2S. 2. O. 3. 2-. (. aq. ) . . . 2I. -. (. aq. ) . + S. 4. O. 6. “From Scratch” Formula. Sometimes you begin making a solution from solid crystal rather than diluting an already made solution.. This is the formula you will need!. Molarity= moles of solute/liters of solution. Ex. 1. What is the molarity of a solution that was prepared by dissolving 11.5g of solid sodium hydroxide in 1.50L of water?. Ex. 2. Calculate the molarity of a solution prepared by dissolving 1.56g of gaseous HCl in enough water to make 26.8 mL of solution.. Part I. I. Properties of Liquids. A. Water. 1. Water is a . triatomic. molecule with covalent H-O bonds.. 2. Water experiences high surface tension and hydrogen bonding.. 3. Water molecules are polar.. H. 5. OH. 3. H. 2. SO. 4. 4. . NaOH. 5. . C. 12. H. 22. O. 11. 6. CaI. 2. 7. HF. 8. Mg(OH). 2. 9. NH. 3. 10.CH. 3. COOH. Do Now: Identify as acid, base, salt, or covalent. Electrolyte or Not. 1. SALT - ELECTROLYTE. Mixture: a . combination of two or more substances that do not combine chemically, but remain the same individual substances; can be separated by physical . means.. Two types:. Heterogeneous. Homogeneous. . a. K. + . , . a. H. + . , a. H4SiO4. . Which chemical . concen. -. trations. from a water . analysis will give . you this information?. m. K. + . , m. H4SiO4 . , pH. Let’s review units commonly used to describe water composition at Earth’s surface.. Molarity = moles of solute / Liters of solution. Concentration. ~How much solute is present in a solution compared to the solvent.. Molarity (M)- moles of solute per liter of solution. M = mol/L. 2.1 M AgNO.