It is not important whether this '200 ml of solution' is countable without or without the hydrated compounds contribution of H2C2O4.2H2O
At first find moles of this
3.78 grams H2C2O4 . 2H2O ( 1 mole cpd./126.068 grams)
= 0.02998 moles H2C2O4 . 2H2O
Since Molarity = moles of solute/Liters of solution ( 200 ml = 0.200 Liters )
Molarity = 0.02998 moles H2C2O4 . 2H2O/0.200 Liters
= 0.150 M H2C2O4.2H2O
3.78 (g H2C2O4.2H2O) / 126.068 (g.mol-1 H2C2O4.2H2O) = 0.02998 (mol H2C2O4.2H2O)
Molarity = moles of solute per Liters of solution
= 0.02998 (mol H2C2O4.2H2O) / 0.200 (Liters) = 0.150 (mol.L-1 H2C2O4.2H2O)
Answer: Molarity = 0.150 M
Molar mass H2C2O4.2H2O =126.0658 g/mol
2.38g = 2.38/126.0658 = 0.0189mol dissolved in 200ml solution.
Molarity = 1000/200*0.0189 = 0.094M
molar mass H2C2O4x2H2O = 2+24+64+36 = 126 g/mole
moles = 2.38 g x 1mol/126 g = 0.0189 moles
molarity = 0.0189 moles/0.200 L = 0.0944 M
The molarity of the oxalic acid is 0,094.
molarity of known H2C2O4
There is no chemical reaction between these products, so if you would bring them together nothing will happen.
Molarity is an indication for concentration.
HP- + H2O(l) ⇌ P2-(aq) + H3O+(aq)
This molarity is approx. o,89.
Molarity = moles of solute/Liters of solution Molarity = 0.202 moles KCl/7.98 Liters = 0.253 M KCl solution ================
Molarity (concentration ) = moles of solute/Liters of solution 250.0 ml = 0.250 liters 2.431 grams H2C2O4 * 2H2O ( 1mole cpd/ 126.068 grams) = 0.01928 moles H2C2O4 * 2H2O Molarity = 0.01928 moles cpd/0.250 liters = 0.07712 Molarity
0.063 g of oxalic acid * (1 mol H2C204*2H2O / 126.07 g) = 0.0004997 mol H2C2O4*2H2O 0.0004997 mol H2C204 / 0.250 L = 0.001999 M of H2C2O4
There is no chemical reaction between these products, so if you would bring them together nothing will happen.
If you raise a solution temperature the molarity will decrease.
Molarity = moles of solute/Liters of solution Molarity = 5 moles solute/4.5 Liters of solution = 1 M solution ==========
Molarity is an indication for concentration.
Molarity is an indication for concentration.
If you concentrate a solution, the molarity (moles/liter) will increase.
HP- + H2O(l) ⇌ P2-(aq) + H3O+(aq)
Adding more solvent to a solution decreases the molarity of the solution. This is based on the principle that initial volume times initial molarity must be equivalent to final volume times final molarity.
This molarity is approx. o,89.
The molarity is 0,041