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Weigh 3g Salt into a 100ml container and bring to volume with deionized water. Mix well. This will be a 3% standard. Other standards are made in the same way (ex.: 2g in 100ml water = 2.00% or 2.5g in 100 ml = 2.50%). I use this in my lab when I make our standard. Hope your not getting this information to late!
Wiki User
∙ 14y ago
Wiki User
∙ 9y ago1.Weigh 3,5 g ultrapure NaCl dried at 110 0C for 30 min.
2. Transfer NaCl in a clean 0,1 L volumetric flask.
3. Add 0,09 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.
Wiki User
∙ 10y agoDissolve 0,75 g NaCl in 100 mL water.
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How do you prepare 0.5L of 65 percent Nitric acid from 69.3 percent of Nitric acid?
It depends on if the Assay is in wt / wt or wt / L because if that's the case you will need to find the density of the 67-70% HNO3 at room temp.But basically you used the equation:C1V1 C2V2whereC1 initial concentrationV1 the amount of solution you will needC2 final concentrationV2 final volumeI would take the average of the assay for C1, so(67+70) / 2 68.5you need to know how much of the solution you want for example 3 Lthen you plug it in, this is also assuming that the initial concentration is in wt / LC1 * V1C2 * V268.5% * V12% * 3Lrearrange to form:V1 (2% * 3L) / 68.5% 0.0876Lwhich you can change into Wt / Wt with the density, or if you need mL just convert with ( 1000mL / 1L )
How many teaspoons of one gram of salt?
1 teaspoon of salt (NaCL) = 6 grams of NaCL or 2,360 mg of sodium (Na). (Na molecular wt is 23, Cl is 35.5, so NaCl is 58.5, so Na is 40 % times grams of wt of NaCl.) So 1 gram NaCl X 1 tsp/6 g NaCl = 0.16667 tsp NaCl or if you want Sodium ( how salt is expressed on food labels) then 1 gram of Na X 1 tsp NaCl/2.360 gram Na = 0.42 tsp Na.
What holds 95 percent of the earths fresh water supply?
Glaciers
How do you convert weight percent of element into weight percent of oxides that exist?
Take 1.45 wt% oxide as an example. To remove the oxide component first you must work out the Ti component: 1.45 wt% oxide x 0.6 = Ti (wt%) because Ti in TiO2 makes up 60% its formula mass: 47.87 / 79.87 = ~0.6 Ti Thus 1.45wt% TiO2 = 0.87 wt% Ti
How will you prepare 20 wt percentage KOH from 85 percentage KOH pellet?
23.530 kg in 76.470 kg of water
How do you prepare 20 mM tris hcl buffer pH 7.4?
to prepare 100ml of 100mM Trissolution: Mol wt of Tris=121.14121.14g in 1000ml ----> 1M12.11g in 100ml -------->1M1M=1000mM121.1g---->1000mM12.11g ----------->100mM1.211g in 100ml and 100mM Tris
How does the isotopes chlorine-35 and 37 occupy the same place in the periodic table?
Isotopes of Chlorine-35 and 37 have different atomic wt. but same atomic number. And in the modern periodic table, the elements are arranged in order of their atomic number AND NOT atomic wt. hence, Chlorine-35 and 37 occupy same place in the periodic table.
What mass of na2s2o3 5h2o is needed to prepare 500.00 ml of 0.1000 m na2s2o3?
Mol.Wt =248.17Molarity =( Wt/ Mol.Wt ) /No:of litres of solution0.1 =( Wt / 248.17) / 0.5Wt =0.1 *0.5*248.17Wt = 12.4085g in 500ml of solution.
What does a quarter wt?
"wt"?
What is the percent by mass of 35g of sodium chloride mixed with 245ml of water?
Calculate the mass of water (density: 1 g/ml) --> 245 ml * 1 g/ml = 245 g of water wt % = 35 g / (35g + 245g) * 100% = 12.5%
How do you prepare 6 molar urea?
Mol. Wt 60.0 So 60.0 gm in 1L is 1M 60*6= 360gm in 1L is 6M urea
How do you prepare 5 percent nitric acid solution from 55 percent nitric acid?
To solve this problem, we basically have 2 equations and 2 unknowns. The unknowns are the (volume of water) & the (volume of 70 wt%) nitric acid to add. * This problem will assume that you are interested in making 1 L (or 1000 mL) of 5 wt% nitric acid solution. Equation 1: (volume of water) + (volume of 70 wt% nitric acid) = 1000 mL Equation 2: mass of nitric acid / [mass of water + mass of 70 wt% nitric acid solution] = 0.05 (0.05 is 5 wt%) * Remember that mass = density * volume * Remember that 70 wt% nitric acid solution mean that for 100 grams (gm) of this acid, then there's 70 grams of HNO3 * Remember that density of 70 wt% nitric acid solution is 1.413 gm/cm^3 * Remember that density of water is 1 gm/cm^3 Equation 2 is now re-written as: [(density of 70 wt% nitric acid soln)*(volume of 70 wt% nitric acid)*0.70] / [(volume water)*(1gm*cm^3) + (volume of 70 wt% nitric acid)*(1.413gm/cm^3)] = 0.05 Solving for the 2 equations gives answer to the 2 unknowns: Answer: To make 1000 mL of 5 wt% nitric acid solution, add 1) 51.63 mL of 70 wt% nitric acid solution 2) 948.37 mL of water
