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The concentration of a solution is expre...

The concentration of a solution is expressed in terms of mole fraction, molarity, molality and in____

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The concentration of solutions can be expressed in number of ways such that Normality, Molarity, Molality, Mole fractions, Strength, % by weight, % by volume and % by strength. The molarity of ionic compound is usually expressed as formality beacuse we use formula weight of ionic compound. Addition of water to a solution changes all these terms, however increase in temperature does not change molality, mole fraction and % by weight terms. Volume of water required to convert 100 mL 0.5M NaOH solutions to 0.2M NaOH solution is:

The concentration of solutions can be expressed in number of ways such that Normality, Molarity, Molality, Mole fractions, Strength, % by weight, % by volume and % by strength. The molarity of ionic compound is usually expressed as formality beacuse we use formula weight of ionic compound. Addition of water to a solution changes all these terms, however increase in temperature does not change molality, mole fraction and % by weight terms. The normality of 0.3N H_(3) BO_(3) is:

The concentration of solutions can be expressed in number of ways such that Normality, Molarity, Molality, Mole fractions, Strength, % by weight, % by volume and % by strength. The molarity of ionic compound is usually expressed as formality beacuse we use formula weight of ionic compound. Addition of water to a solution changes all these terms, however increase in temperature does not change molality, mole fraction and % by weight terms. Number of oxalate ions in 100 mL of 0.1N oxalic acis is:

The concentration of solutions can be expressed in number of ways such that Normality, Molarity, Molality, Mole fractions, Strength, % by weight, % by volume and % by strength. The molarity of ionic compound is usually expressed as formality beacuse we use formula weight of ionic compound. Addition of water to a solution changes all these terms, however increase in temperature does not change molality, mole fraction and % by weight terms. Molecular weight of O_(3) in the reaction, 2O_(3)hArr3O_(2) is:

The concentration of solutions can be expressed in number of ways such that Normality, Molarity, Molality, Mole fractions, Strength, % by weight, % by volume and % by strength. The molarity of ionic compound is usually expressed as formality beacuse we use formula weight of ionic compound. Addition of water to a solution changes all these terms, however increase in temperature does not change molality, mole fraction and % by weight terms. Which is not a molecular formula?

The concentration of solutions can be expressed in number of ways such that Normality, Molarity, Molality, Mole fractions, Strength, % by weight, % by volume and % by strength. The molarity of ionic compound is usually expressed as formality beacuse we use formula weight of ionic compound. Addition of water to a solution changes all these terms, however increase in temperature does not change molality, mole fraction and % by weight terms. Two litre of NH_(3) at 30^(@)C and 0.20 atm is neutralised by 134 mL of acid (H_(2)SO_(4)) . The molarity of H_(2)SO_(4) is:

The concentration of solutions can be expressed in number of ways such that Normality, Molarity, Molality, Mole fractions, Strength, % by weight, % by volume and % by strength. The molarity of ionic compound is usually expressed as formality beacuse we use formula weight of ionic compound. Addition of water to a solution changes all these terms, however increase in temperature does not change molality, mole fraction and % by weight terms. The weight of Na_(2)CO_(3) sample of 95% purity required to neutralise 45.6 mL of 0.235 N acid is:

Express the concentration of 5% mass of solution of Na_(2)S_(2)O_(3) in terms of (a) molarity (b) molality and © mole fraction of solution. The density of solution at 25^(@)C is gm L^(-1)

The concentrations of soluitons can be expressed in number of ways , viz : mass fraction of solute (or mass percent), Molar concentration (Molarity ) and Molal concentration (molality). These terms are known as concentration terms and also they are related with each otehr i.e., knowing one concentration terms for the solution, we can find other concentration terms also. the definition of different cencentration terms are given below: Molarity : It is number of moles of solute present in one litre of the solution. Molality : It is the number of moles of solute present in one kg of the solvent. Mole fraction =("Mole of solute")/("Moles of solute" + "Moles of solvent") If molality of the solution is given as a, then mole fraction of the solute can be calculated by Mole Fraction =(a)/(a+(100)/(M_("solvent"))),=(axxM_("solvent"))/((a xx M_("solvent")+1000)0 where a=molality and M_("solvent") =Molar mass of solvent We can change : Mole fraction hArr Molality hArr Molarity What is the mole fraction of the solute?