I am going to assume that your "exactly" has some reasonable leeway associated with it. Molar concentration = (no. of mols)/volume (in L). Therefore 4.75 M = (no of mols) /0.25 L Therefore no. of mols = 0.25 * 4.75 = 1.1875 mols Molar mass of NaOH = 23 + 16 + 1 = 40 g/mol Therefore mass of 100 % NaOH required = 1.1875 mol * 40 g/mol =47.5 g NaOH So - in detail, you would weigh out the mass of solids NaOH, dissolve it in 250 ml of water and you would have the required solution. The volume won't be EXACT, but close as.
0.250 Mols in 1 litre, so there are 0.5 mols in 2 litres.
0.5 mols NaOH * 40 grams NaOH(molecular weight) = 20 grams NaOH.
Therefore, just add 20 grams of NaOH to water, and your good to go!
Hope this helps :D
For making 1 MSolution, 40 gm NaoH dissolved in 1000 ml Distilled water .then10 ml solution of 1 M (Stock solution) dissolved in 500 ml distilled water for 0.02 M NaOH solution.
R.C Joshi.
1. Weigh 0,8 g ultrapure dried NaOH.
2. Transfer NaOH in a clean 1 L volumetric flask using a funnel. 3. Wash the funnel with 0,9 L demineralized water.
4. Put the flask in a thermostat and maintain 30 min at 20 0C.
5. Add demineralized water up to the mark.
6. Stir vigorously and transfer in a clean bottle with stopper.
7. Add a label with necessary information.
You need 2,4 g NaOH (0,06 moles).
MaVa=MbVb (6.0M NaOH)(x)=(0.10M solution)(1.0L) x=0.017L of 6.0M NaOH Convert to mL (1000mL in 1L) 17mL of 6.0M NaOH
Concentration of NaOH = 0.025 M = 0.025 Moles per Litre of SolutionVolume of Solution required = 5.00LWe can say therefore that:Number of Moles of NaOH needed to prepare the solution= Concentration of NaOH * Volume of Solution requiredTherefore:Number of Moles of NaOH needed to prepare the solution= 0.025M * 5.00L= 0.125molesFrom this we can say that 0.125 moles of NaOH are needed to prepare a 5.00 L solution with a concentration of 0.025M of NaOH.
Hi, 6N NaOH = 6M NaOH 6M NaOH are 6 moles in 1L Mw (NaOH) = 39.88 gr/mole so: m = n x MW = 6 x 39.88 = 239.28 gr NaOH. :)
95g NaOH * 1 mol NaOH/ = 2.375 mol NaOH 40g NaOH Molarity (M) = mol / L M = (2.375) / (0.450) M = 5.28
You need 2,4 g NaOH (0,06 moles).
MaVa=MbVb (6.0M NaOH)(x)=(0.10M solution)(1.0L) x=0.017L of 6.0M NaOH Convert to mL (1000mL in 1L) 17mL of 6.0M NaOH
Concentration of NaOH = 0.025 M = 0.025 Moles per Litre of SolutionVolume of Solution required = 5.00LWe can say therefore that:Number of Moles of NaOH needed to prepare the solution= Concentration of NaOH * Volume of Solution requiredTherefore:Number of Moles of NaOH needed to prepare the solution= 0.025M * 5.00L= 0.125molesFrom this we can say that 0.125 moles of NaOH are needed to prepare a 5.00 L solution with a concentration of 0.025M of NaOH.
Hi, 6N NaOH = 6M NaOH 6M NaOH are 6 moles in 1L Mw (NaOH) = 39.88 gr/mole so: m = n x MW = 6 x 39.88 = 239.28 gr NaOH. :)
95g NaOH * 1 mol NaOH/ = 2.375 mol NaOH 40g NaOH Molarity (M) = mol / L M = (2.375) / (0.450) M = 5.28
Simple equality will do here as you have three things and require a fourth. (X L)(2.5 M NaOH) = (2.0 L)(0.75 M NaOH) 2.5X = 1.5 X = 0.60 Liters needed ================
One mole of NaOH weighs 23(Na)+16(O)+1(H)=40 g A 0.05 M NaOH is then 2 g NaOH/L. So dissolve 2 g NaOH in 500 ml water let it cool down to room temperature and fill it up to one liter. For accurate results you can use an analytical balance and a volumetric flask.
Given: 27 mL of NaOH, 0.45M; 20 mL HCI Need: M of HCI 27 ml NaOH*(1 L NaOH/1000mL NaOH)*(0.45M NaOH/1L NaOH)*(1mole HCI/1 mole NaOH)=0.012 0.012/0.02=0.607 M HCI (or rounded 0.61 M HCI)
base
4 moles or 160 g NaOH is required for one litre solution.
na+oh +25=53 ph+poh=2.3
- log(0.048 M NaOH) = 1.3 pH --------------need Molarity? 1/10 1.3 = 0.050 M H3O ---------------------