What volume of concentrated H2SO4 (density = 1.84g/mL and 96% purity) would be required to prepare 500mL of a 0.2000M H2SO4 solution?
Dear anonymous,Apparently, you want us to do your homework for you. Below is the solution to your question. Do know that this solution is useless to you unless you understand each step and why it is taken. So while I give you the solution to the question, it will be up to you to study this answer carefully and make sure you understand it.To start of with, we will need to fix the question itself as it contains a rather big error. The density of any substance is given in g/cm^3. Not in g/mol as that would be the molecular weight. So the density is 1.84 g/cm^3 (=1.84 g/mL).The answer:0.2M = 0.2 mole/LTherefore, 0.5L * 0.2M = 0.1 mole of H2SO4 required.The molar mass of H2SO4 is 98.079 g/mole (see periodic table or google).Therefore, 98.079 g/mole * 0.1 mole = 9.8079 g9.8079 g/ 1.84 g/cm^3 = 5.33038 cm^3 (=5.33038 mL)The purity of your substance is 96%, therefore you will actually need:5.33038*(1/0.96) = 5.55248 mL.The required precision in your answer is 3 digits (due to the precision of 500 mL).Therefore, the answer is 5.55 mL of acid and (500–5.55 =) 494 mL of water.Note that when preparing such a dilution, always add acid to water. Never the other way around. Pure H2SO4 is an extremely dangerous substance. Handle only under the supervision of a professional.
How would you make up 200ml of a 0.3 M solution of NaCl?
The most direct method would be to add the amount of NaCl present in 200ml of 0.3M solution of NaCl, although such a method will be impractical in laboratories where often large quantities of NaCl is needed. In these situations, a stock solution of large volumes of 1.0M of NaCl is prepared. Then a sample volume of the stock solution is taken and diluted by adding water to give you the desired concentration.Anyways, one will determine the amount of NaCl present in 200ml of 0.3M solution of NaCl:concentration= 0.3M= 0.3mol/Lvolume = 200mL= 0.2Lnumber of moles of NaCl= 0.3mol/L * 0.2L = 0.06molmolar mass of NaCl= 58.44g/molmass of NaCl= 3.5064g = 3.51g.Therefore,Add 3.51g of NaCl into 200ml of water in a beaker.Then, you will end up with 200ml of 0.3M NaCl using the direct method of prepreatio!
What does it mean by CONCENTRATED nitric acid?
Nitric acid is a solution of HNO3 - a colorless liquid when it's pure - in water; as nitric acid is completely miscible with water, there is no such thing as "fully" concentrated nitric acid. The term might, however, well relate to a solution that contains 68% HNO3 by weight, which is pretty concentrated, and the way nitric acid is usually sold - pure nitric acid isn't very stable, turns yellow pretty quickly, and neither are higher concentrations (-> fuming nitric acid).
Can you calculate the molarity, molality, and normality of a H2SO4 solution, which is 98% w/w and has a density of 1.8g/mL?
There is a straight formula for converting w/w% into molarity.Molarity={(w/w%)×10×(density in g/ml)}÷(Molar mass of solute in g)Putting values, M=(98×10×1.8)/(98)=18MNow, Normality=Molarity×n-factorPutting values, N=18×2=36N (n-factor is 2 because H2SO4 is a dibasic acid)Molality is a bit tricky because the formula involves tedious calculation.Molality=(1000×Molarity)/{(1000×density in g/ml)-(Molar mass of solute in g×Molarity)}Putting values,m=(1000×18)/{(1000×1.8)-(98×18)}=18000/(1800–1764)=18000/36=500m
How do i prepare a solution of calcium chloride and water?
OxyChem's calcium chloride website has an FAQ with a calculator on it. Maybe that will help you. here it is cut and pasted: How do I make solutions by mixing solid calcium chloride products with water? Use cool water! Significant heat is released when dissolving. Add solid calcium chloride slowly while continuously mixing. If solids are allowed to sit motionless while in contact with water, a hard cake will form that will be slow to dissolve. The observed temperature increase during dissolving will vary depending on the conditions associated with each specific application. However, a rough estimate may be calculated as follows: For DOWFLAKE™ Xtra 83-87% Calcium Chloride Flakes, assume a temperature increase of 2.8°F per percent increase in concentration. For PELADOW™ Premier Snow & Ice Melter and Anhydrous Calcium Chloride 94-97% Mini-Pellets, assume 3.2°F and 3.5°F, respectively, per percent increase in concentration. For example, when making up a 30% solution from DOWFLAKE™ Xtra 83-87% Calcium Chloride Flakes, the solution temperature may be expected to increase approximately (30 x 2.8°F) = 84°F. A spreadsheet tool is available to determine the amount of dry calcium chloride to mix with water to achieve solutions of various concentrations. The link is provided below. Making Solutions Using Dry Calcium Chloride Products Calculator http://www.oxycalciumchloride.com/faq/Making%20Solutions%20Calculator.xls