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One molar solution means 1 mole of solut...

One molar solution means 1 mole of solute present in

A

1000 g of solution

B

1 L of solvent

C

1 L of solution

D

1000 g of solution

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The correct Answer is:
C
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Assertion (A): A molar solution is more concentrated than molal solution. Reason (R): A molar solution contains one mole of solute in 1000 mL of solution.

1 gm molar solution is

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?

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 Percentage (weight/vol) of NaCl persent in the solution is :

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 molality of the above solution?

The concentrations of solutions are also expressed in Demal units. One demal unit represents one mole of solute present in one litre of the solution at

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 molarity of solutions if density of solution in 1.6 gm/ml?

CENGAGE CHEMISTRY-EQUIVALENT MASS -MANDATORY EXERCISE Exercise Set III
  1. 10 cm^(3) of 0.1 N monobasic acid requires 15 cm^(3) of sodium hydroge...

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  2. What is the molarity of pure water?

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  3. The volume of water to be added to 100 cm^(3) of 0.5 N H(2)SO(4) to ge...

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  4. The molarity of the solution obtained by dissolving 2.5 g of NaCl in 1...

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  5. How many grams of dibasic acid (mol. Wt 200) should be present in 100 ...

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  6. Which of the following is not true for 0.1 M Na(2)CO(3).

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  7. 480 ml of 1.5 M and 520 ml of 1.2 M solution of same substance mixed t...

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  8. Molarity of 0.2 N H(2)BO(3) is

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  9. One molar solution means 1 mole of solute present in

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  10. The volume of water to be added to 100 ml of N/(2)HCl to prepare 500 c...

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  11. 6.022xx10^(20) molecules of glucose are present in 100 ml of the solut...

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  12. The normality of mixture obtained by mixing 100 ml of 0.2 M H(2)SO(4)+...

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  13. The unit of molarity is

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  14. 1 L of NaOH solution contains 8 g if NaOH. The approximate concentrati...

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  15. A solution of oxalix acid (COOH)(2)*2H(2)O is prepared by dissolving 0...

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  16. Commercially available concentrated hydrochloric acid conatins 38% HCl...

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  17. Commercially available concentrated hydrochloric acid conatins 38% HCl...

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  18. 20 cm^(3) of 1 N HCl and 30 cm^(3) of 0.5 N HCl are mmixed together. W...

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  19. Concentrated aqueous H(2)SO(4) is 98% H(2)SO(4) by mass and has densit...

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  20. Match the following:

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