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Puspak Sah

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Volumetric Analysis

How many mL of a 0.1 M HCl are required to react completely with a 1gm mixture of Na2CO3 and NaHCO3 containing the equimolar amount of the two.

solution:let, the amount of Na2Co3 in the mixture = x gmNaHCo3 present in mixture = (1-x) gmMolar mass of Na2Co3 = 2*23+12+3*16 = 106 gm/molesimilarly, molar mass of NaHCo3 = 84 gm/moletherefore, moles of Na2Co3 in x gm = x/106 and moles of NaHCo3 in (1-x) gm = (1-x)/84According to the question,x/106 = (1-x)/84 so, x = 0.558gmThus the number of moles of Na2Co3 and NaHCo3 are 0.00526 moleAgain by reaction,

Na2CO3+2HCl2NaCl+H2O+CO2

Na2CO3+2HCl2NaCl+H2O+CO2

NaHCO3+HClNaCl+H2O+CO21 mole of

Na2CO3
...

Define the molarity of a solution. Calculate the molarity of one liter of 93% H2SO4 solution (weight by volume). The density of the solution is 1.84 g/mL.

The number of moles of a solute dissolved in 1 L (1000 ml) of the solutionis known as the molarity of the solution.

we know,

Molarity * mol. wt = %(w/v) * 10

Molarity = 93*10/98 ==> 9.489

Difference between molarity and normality.

Normality	Molarity
1. It is the number of gram equivalents of solute dissolved per litre solution.	1. It is the number of gram molecules of solute dissolved per litre its solution.
2. In general, Normality(N) = (g/L)/eq. wt	2. Molarity(M) = (w1000)/(v mol. wt)

Distinguish between decinormal and decimolar solution.

Deci- Normal solution ---->The solution containing 1/10 mole of solute in 1 liter of solution is called normal solution.

Deci-molar solution(M10):The solution containing 110 th mole of solute in 1 liter of solution is known as decinormal solution.

What Are The Differences Between End Point And Equivalence Point?

The main difference between equivalence and endpoint is thatthe equivalence point is a point where the chemical reaction comes to an end while the endpoint is the point where the colour change occurs in a system.

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