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How do you prepare 0.01 molar NaOH in one litter?
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+ Chemical reactions
+ Sodium hydroxide
+ Chemistry
+ Organic chemistry
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Md. Sadman Sakib
How do you prepare 0.01 molar NaOH in one litter?
Molarity tells you how many moles of a particular component you have in one liter of its solution. It has usually units mol/L (mole per liter, same as molar concentration). When you want to prepare 0.01 molar (0.01 M) solution of NaOH, you want to prepare 0.01 mol/L solution of NaOH.
Let’s designate:
n as total number of moles of NaOH (mol),
m as total mass of NaOH (g),
M[i] as molecular weight of some substance i (g/mol),
V as volume of the solution (L),
c as concentration of NaOH in the solution (mol/L).
When you want to prepare 0.01 mol/L solution of NaOH, you want to prepare a solution of concentration c = 0.01 mol/L. This concentration, you can calculate as:
c = n/V.
You probably know how many liters you want to prepare. For the sake of our calculations here, let’s say you have a 100 mL flask, therefore V = 100 mL = 0.1 L.
Now, how do we get the total number of moles n? We just need to divide the total mass (m) by the molecular weight of NaOH (M[NaOH]). In a periodic table, there you can find molecular weights for all the atoms in the NaOH molecule:
M[Na] = 22.99 g/mol,
M[O] = 16.00 g/mol,
M[H] = 1.08 g/mol,
and the molecular weight of NaOH can be calculated as:
Molarity tells you how many moles of a particular component you have in one liter of its solution. It has usually units mol/L (mole per liter, same as molar concentration). When you want to prepare 0.01 molar (0.01 M) solution of NaOH, you want to prepare 0.01 mol/L solution of NaOH.
Let’s designate:
n as total number of moles of NaOH (mol),
m as total mass of NaOH (g),
M[i] as molecular weight of some substance i (g/mol),
V as volume of the solution (L),
c as concentration of NaOH in the solution (mol/L).
When you want to prepare 0.01 mol/L solution of NaOH, you want to prepare a solution of concentration c = 0.01 mol/L. This concentration, you can calculate as:
c = n/V.
You probably know how many liters you want to prepare. For the sake of our calculations here, let’s say you have a 100 mL flask, therefore V = 100 mL = 0.1 L.
Now, how do we get the total number of moles n? We just need to divide the total mass (m) by the molecular weight of NaOH (M[NaOH]). In a periodic table, there you can find molecular weights for all the atoms in the NaOH molecule:
M[Na] = 22.99 g/mol,
M[O] = 16.00 g/mol,
M[H] = 1.08 g/mol,
and the molecular weight of NaOH can be calculated as:
Molarity tells you how many moles of a particular component you have in one liter of its solution. It has usually units mol/L (mole per liter, same as molar concentration). When you want to prepare 0.01 molar (0.01 M) solution of NaOH, you want to prepare 0.01 mol/L solution of NaOH.
Let’s designate:
When you want to prepare 0.01 mol/L solution of NaOH, you want to prepare a solution of concentration c = 0.01 mol/L. This concentration, you can calculate as:
c = n/V.
You probably know how many liters you want to prepare. For the sake of our calculations here, let’s say you have a 100 mL flask, therefore V = 100 mL = 0.1 L.
Now, how do we get the total number of moles n? We just need to divide the total mass (m) by the molecular weight of NaOH (M[NaOH]). In a periodic table, there you can find molecular weights for all the atoms in the NaOH molecule:
M[Na] = 22.99 g/mol,
M[O] = 16.00 g/mol,
M[H] = 1.08 g/mol,
and the molecular weight of NaOH can be calculated as:
M[NaOH] = M[Na] + M[O] + M[H] = 22.99 + 16.00 + 1.08 = 40.07 g/mol.
Now, the total number of moles can be calculated as:
n = m/M[NaOH].
When we put it all together, we get:
c = m/M[NaOH]/V.
As you probably want to calculate the mass of NaOH you need to add to your volume of water, you have to change the expression as:
m = cVM[NaOH],
where the concentration c is the molarity of your solution.
For our 100 mL flask, the expression will have values:
m = 0.01*0.1*40.07 = 0.04007 g.
To make a 0.01 M solution of NaOH, you need dissolve 0.04007 grams of NaOH in 100 mL of water.
Molarity tells you how many moles of a particular component you have in one liter of its solution. It has usually units mol/L (mole per liter, same as molar concentration). When you want to prepare 0.01 molar (0.01 M) solution of NaOH, you want to prepare 0.01 mol/L solution of NaOH.
Let’s designate:
When you want to prepare 0.01 mol/L solution of NaOH, you want to prepare a solution of concentration c = 0.01 mol/L. This concentration, you can calculate as:
c = n/V.
You probably know how many liters you want to prepare. For the sake of our calculations here, let’s say you have a 100 mL flask, therefore V = 100 mL = 0.1 L.
Now, how do we get the total number of moles n? We just need to divide the total mass (m) by the molecular weight of NaOH (M[NaOH]). In a periodic table, there you can find molecular weights for all the atoms in the NaOH molecule:
M[Na] = 22.99 g/mol,
M[O] = 16.00 g/mol,
M[H] = 1.08 g/mol,
and the molecular weight of NaOH can be calculated as:
M[NaOH] = M[Na] + M[O] + M[H] = 22.99 + 16.00 + 1.08 = 40.07 g/mol.
Now, the total number of moles can be calculated as:
n = m/M[NaOH].
When we put it all together, we get:
c = m/M[NaOH]/V.
As you probably want to calculate the mass of NaOH you need to add to your volume of water, you have to change the expression as:
m = cVM[NaOH],
where the concentration c is the molarity of your solution.
For our 100 mL flask, the expression will have values:
m = 0.01*0.1*40.07 = 0.04007 g.
To make a 0.01 M solution of NaOH, you need dissolve 0.04007 grams of NaOH in 100 mL of water.
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If you add 0.4g NaOH in 1L volumetric flask and then add water till the mark then you can prepare 0.01 molar NaOH.
If you add 0.4g NaOH in 1L volumetric flask and then add water till the mark then you can prepare 0.01 molar NaOH.
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