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Method of expressing of concentration
The document presents different methods for expressing concentrations of solutions, including normality, molarity, molality, percent solutions, formal concentration, and parts per million (ppm). Each method is defined with examples, particularly using sodium hydroxide (NaOH) and hydrochloric acid (HCl). References for further reading on the topic are also provided.
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Presentation introduction by Mr. Prashant B. Patil on expressing solution concentrations.
Overview of techniques for expression including Normality, Molarity, Molality, Percent Solution, Formal Concentration, and PPM.
Definition of Normality (N) with examples for NaOH concentrations at 1N, 0.1N, and 0.01N.
Definition of Molarity (M) with NaOH and HCl examples at 1M, 0.1M, and 0.01M.
Definition of Molality with examples for NaOH indicating concentrations based on kg of solution.
Different types of percent concentrations (%W/W, %V/V, %W/V) with KCl examples.
Definition of Formal Concentration (F) with example calculation for CaCO3 concentration.
Definition of Parts Per Million (PPM) with formula for concentration in dilute solutions.
List of references used including textbooks on pharmaceutical and analytical chemistry.
Closing slide with thank you note to the audience.
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Method of expressing of concentration
- 1. Method of ExpressingConcentrations Presentation by, Mr. Prashant B. Patil Assistant Professor H R Patel Institute of Pharmaceutical Education and Research, Shirpur
- 2. Normality, Morality Molality, %Solution, Formal Concentration Equivalent Weight & PPM REFERENCES
- 3. In allthe techniques of quantitative analysis the use of solutions requires some basis for the expression of solution concentration. 1. Normality 2. Molarity 3. Molality 4. Percent Solution 5. Formal Concentration 6. Parts per Million (PPM)
- 4. Normality- Numberof gram equivalent of solute (Substance) dissolved in one litre (1000 ml) of solution is called as Normality. Normality is indicated by N Normality Examples- Molecular weight of NaOH (Sodium Hydroxide)= Atomic Weight of Na = 22.99 Atomic Weight of O = 16 Atomic Weight of H = 1 40 Gram equivalent Weight of Solute Equivalent Weight = --------------------------------------------- No. of replaceable H + & OH -
- 5. - 1N =40 gm of NaOH is Dissolved in 1000 ml of water (H2O) - 0.1 N = 4 gm of NaOH is Dissolved in 1000 ml of water (H2O) - 0.01N = 0.4 gm of NaOH is Dissolved in 1000 ml of water (H2O)
- 6. Molarity -Number of moles of solute (Substance) dissolved in one litre (1000 mL) of Solution is called as Molarity. 1 gm in 1000 ml = 1 mol. Molarity is indicated by M Molarity Examples- Molecular weight of NaOH (Sodium Hydroxide)= Atomic Weight of Na= 22.99 Atomic Weight of O= 16 Atomic Weight of H= 1 40 Number of moles of Solute M = ------------------------------------ 1000 mL of Solution
- 7. - 1M= 40gm of NaOH is Dissolved in 1000 mL of water (H2O) - 0.1 M= 4 gm of NaOH is Dissolved in 1000 mL of water (H2O) - 0.01M= 0.4 gm of NaOH is Dissolved in 1000 mL of water (H2O) Molarity Examples- Molecular weight of HCl (Hydrochloric acid)= Atomic Weight of Cl = 35.5 Atomic Weight of H = 1 36.5 - 1M = 36.5 gm of HCl is Dissolved in 1000 mL of water (H2O) - 0.1 M = 3.65 gm of HCl is Dissolved in 1000 mL of water (H2O) - 0.01M = 0.365 gm of HCl is Dissolved in 1000 mL of water (H2O)
- 8. Molality- Amolal solution contains 1 mole of solute per one kilogram of solution ( 1 lit. of solvent) is called as Molality. Molality is indicated by M Molality Examples- Molecular weight of NaOH (Sodium Hydroxide)= Atomic Weight of Na = 22.99 Atomic Weight of O = 16 Atomic Weight of H = 1 40 Number of mol. Wt. of substance N = --------------------------------------- 1000 gm of Solution (1Kg)
- 9. - 1 M= 40 gm of NaOH is Dissolved in 1000 gm of water (H2O) - 0.1 M = 4 gm of NaOH is Dissolved in 1000 gm of water (H2O) - 0.01 M= 0.4 gm of NaOH is Dissolved in 1000 gm of water (H2O) - 1.5 M= 60 gm of NaOH is Dissolved in 1000 gm of water (H2O)
- 10. Percent (%)Solution Sometimes the concentration is expressed in terms of per cent (parts per hundred) also. Per cent Composition of a solution can be expressed as: 1. Per cent W/W = Weight of solute/ Weight of solution X 100 2. Per cent V/V = Volume of solute/ Volume of solution X 100 3. Per cent W/V= Weight of solute/ Volume of solution X 100 1 %= 1gm of KCl ----------- in 100 ml of water 10 % = 10 gm of KCl ----------- in 100 ml of water 100 % = 100 gm of KCl ----------- in 100 ml of water
- 11. Formal Concentration The concentration unit, formal, is similar to the more familiar molar concentration in that it is calculated as the number of moles of a substance in a liter of solution. Formal concentrations are notated with the symbol F. The formal Concentration (Formality) is applicable to the ionic substances Ex. We'll use calcium carbonate because it has a simple formula weight (100 g/mole). If one has 1 g CaCO3 in 1 L aqueous solution, the concentration of CaCO3, in formal, is... 1 g CaCO3/(100 g CaCO3/mole)/(1 L) = 0.01 F CaCO3
- 12. Parts PerMillion Parts per million is frequently employed to express the concentration of very dilute solutions and is express as PPM Conc. In PPM = Mass of solute / mass of solution X 106 PPM 1 PPPM = 1 mg/it.
- 13. References • A.H.Beckett & J.B. Stenlake's, Practical Pharmaceutical Chemistry Vol I & II, Stahlone Press of University of London • A.I. Vogel, Text Book of Quantitative Inorganic analysis • P. Gundu Rao, Inorganic Pharmaceutical Chemistry • Bentley and Driver's Textbook of Pharmaceutical Chemistry • John H. Kennedy, Analytical chemistry principles • Indian Pharmacopoeia
- 14.