Introduction to Solutions & Concentration

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Presentation transcript:

Introduction to Solutions & Concentration October 2017

the substance that gets dissolved can be solid, liquid or gas Solutions Solute: the substance that gets dissolved can be solid, liquid or gas Solvent: the substance that does the dissolving we will be using water as the solvent

CONCENTRATION: Describes the amount of solute in a given volume of solution Can be expressed as: percent, ppm or molar concentration

1) Percent: volume per volume (v/v) 3% v/v means: 3 mL of H2O2(l) / 100 mL hydrogen peroxide solution

Percent: mass per volume (m/v) 2% m/v means: 2 grams of milk fat/ 100 mL milk solution

Percent: mass per mass (m/m) Brass: 67% copper 33% zinc

14 karat gold 14 parts pure gold 10 parts other metals (copper, silver zinc) 24 kt

2) Parts per million and parts per billion Used when concentrations are very low 50 ppm calcium => 50 drops of calcium for every 1000000 drops of water

3) MOLAR CONCENTRATION This is the one used in chemistry. Is the number of moles of solute in 1 L of solution Units are mol/L C = n/V

Calculate the molar concentration of the following solutions: A 1.0 L Windex solution contains 0.143 moles of ammonium hydroxide, NH4OH.

Calculate the molar concentration of the following solutions: A 250 mL bottle of apple juice contains 0.139 moles of sugar, C6H12O6.

Calculate the molar concentration of the following solutions: A 1.0 L saline solution contains 0.900 g of NaCl.

Calculate the molar concentration of the following solutions: A 3.75 L container of typical household bleach contains 196.88 g of sodium hypochlorite, NaOCl.

Calculate the molar concentration of the following solutions: A 360 mL serving of coke contains 39 g of fructose, C6H12O6.

You are asked to make 150. 00 mL of 0 You are asked to make 150.00 mL of 0.500 mol/L nickel (II) chloride solution. How many grams of nickel (II) chloride would you need to mass out?