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How you can find the percentage and specific gravity of unknown HCl?
find, at the given temperature and pressure, weight of HCL and volume of the same. Find density of HCL by Density of HCL= weight/volume Specific gravity of HCL= density of HCL/density of water
What is the density of HCl?
depending on its mass and volumeDensity of 1.477 g/l, gas (25 °C)
How do you convert 37 percent HCL in normality?
Density of HCl = 1.186 g/mL Molar Mass HCl = 36.46g/mol We want a concentration in mol/L so we will first convert density into g/L (1.186 g/mL)(1000mL/1L) = 1186 g/L We must now know what density 37% of that is (0.37)(1186 g/L) = 438.82 g/L Now divide this density by the molar mass to cance out the g and give you mol/L (concentration) C = (438.82g/L)/(36.46g/mol) C = 12.04 M Since HCl is monoprotic, 1M = 1N. Therefore, 37% HCl is ~12N
How much does HCL weigh per gallon?
Hydrochloric acid (HCl) has a density of approximately 1.2 grams per cubic centimeter, which is equivalent to roughly 10 pounds per gallon.
How can 1 M of HCl be prepared from 32 percent HCl concentration?
percentage = well, mostly weight percentage is the most commonly given percentage density = the density of a sol'n is constant, for HCl, the value is 1.18 g/ mL now assuming you have 34% of HCl in the sol'n in preparing 1M HCl, calculate the mass of HCl Needed. assuming there are 100g of the whole solution, therefore there will be 34g of HCl: percent by weight = (34% x 100g) / 100g = 34g now to get the mass, we need dimensional analysis. 34 g HCl x 1 mol HCl x 1 L sol'n x 1.18 g HCl x 1 mL = FINAL ANSWER 36.45 g HCl 1 mol HCl 1 mL 1 L sol'n you just get the final answer.... percentage = well, mostly weight percentage is the most commonly given percentage density = the density of a sol'n is constant, for HCl, the value is 1.18 g/ mL now assuming you have 34% of HCl in the sol'n in preparing 1M HCl, calculate the mass of HCl Needed. assuming there are 100g of the whole solution, therefore there will be 34g of HCl: percent by weight = (34% x 100g) / 100g = 34g now to get the mass, we need dimensional analysis. 34 g HCl x 1 mol HCl x 1 L sol'n x 1.18 g HCl x 1 mL = FINAL ANSWER 36.45 g HCl 1 mol HCl 1 mL 1 L sol'n you just get the final answer....
How you can find the percentage and specific gravity of unknown HCl?
find, at the given temperature and pressure, weight of HCL and volume of the same. Find density of HCL by Density of HCL= weight/volume Specific gravity of HCL= density of HCL/density of water
What is the density of HCl?
depending on its mass and volumeDensity of 1.477 g/l, gas (25 °C)
How do you convert 37 percent HCL in normality?
Density of HCl = 1.186 g/mL Molar Mass HCl = 36.46g/mol We want a concentration in mol/L so we will first convert density into g/L (1.186 g/mL)(1000mL/1L) = 1186 g/L We must now know what density 37% of that is (0.37)(1186 g/L) = 438.82 g/L Now divide this density by the molar mass to cance out the g and give you mol/L (concentration) C = (438.82g/L)/(36.46g/mol) C = 12.04 M Since HCl is monoprotic, 1M = 1N. Therefore, 37% HCl is ~12N
How much does HCL weigh per gallon?
Hydrochloric acid (HCl) has a density of approximately 1.2 grams per cubic centimeter, which is equivalent to roughly 10 pounds per gallon.
How can 1 M of HCl be prepared from 32 percent HCl concentration?
percentage = well, mostly weight percentage is the most commonly given percentage density = the density of a sol'n is constant, for HCl, the value is 1.18 g/ mL now assuming you have 34% of HCl in the sol'n in preparing 1M HCl, calculate the mass of HCl Needed. assuming there are 100g of the whole solution, therefore there will be 34g of HCl: percent by weight = (34% x 100g) / 100g = 34g now to get the mass, we need dimensional analysis. 34 g HCl x 1 mol HCl x 1 L sol'n x 1.18 g HCl x 1 mL = FINAL ANSWER 36.45 g HCl 1 mol HCl 1 mL 1 L sol'n you just get the final answer.... percentage = well, mostly weight percentage is the most commonly given percentage density = the density of a sol'n is constant, for HCl, the value is 1.18 g/ mL now assuming you have 34% of HCl in the sol'n in preparing 1M HCl, calculate the mass of HCl Needed. assuming there are 100g of the whole solution, therefore there will be 34g of HCl: percent by weight = (34% x 100g) / 100g = 34g now to get the mass, we need dimensional analysis. 34 g HCl x 1 mol HCl x 1 L sol'n x 1.18 g HCl x 1 mL = FINAL ANSWER 36.45 g HCl 1 mol HCl 1 mL 1 L sol'n you just get the final answer....
How do you prepare 0.2 mol per liter HCl from concentrated HCL?
To prepare 0.2 mol/L HCl from concentrated HCl (e.g., 37% HCl), you would need to dilute the concentrated HCl with water in the appropriate ratio. Since the concentrated HCl usually has a density of around 1.19 g/mL, you can use the formula M1V1 = M2V2 to calculate the volume of concentrated HCl needed. After calculating the volume of concentrated HCl required, add water to make up the final volume of 1 liter to achieve a 0.2 mol/L HCl solution.
Calculate the molarity of a 10 percent aqueous solution of HCl?
molarity = mol / litre The concentration is 10% HCl in water, assuming this is expressed in w/v (weight to volume) as this is the normal way. The density of 10% HCl is unknown but will be estimated to be the same as water (although slightly incorrect), since no data is given. 1 L of which 10% are HCl is assumed to weigh 1000 grams. 10% HCl x 1000g = 100g of HCl. 100g of HCl is present in 1 L. The mw of HCl = 36.5g/mol, 100g/(36.5g/mol) = 2.74mol is present in 1 L. The molarity is 2.74mol / 1 L = 2.7 M (two significant figures) (Looking up hydrochloric acid in wikipedia tells us that the density of a 10% solution is actually 1048g/L and the actual molarity becomes 2.87M. The calculated number was close enough, but it shows that the density is important. Molality on the other hand is mol/kg, so with molality we can skip the unknown density problem. For practical purposes, molarity is still the mostly used one, because volume is easier to measure than weight in the laboratory when handling toxic solvents that are unhealthy to inhale.)
How to prepare HCL solution?
To prepare a hydrochloric acid (HCl) solution, you can dilute concentrated hydrochloric acid with water. Always add the acid to water slowly while stirring, never add water to acid, as it can cause splattering. Be sure to wear appropriate protective gear and work in a well-ventilated area when handling HCl.
Calculaton of 1N HCl preparation?
take the Mr of HCl to be 36.46. to prepare 1.0M we should take 36.46g and dilute to a litre to prepare 0.10M we should take 3.646g and dilute to a litre From density =mass/volume, we get volume=mass/density. So ideally we should take that volume and dilute to a litre. However we know that most conc HCl solution are not 100% HCl. thus we must multiply that volume by a factor 100/x for an HCl solution labelled x% Tauya Chigayo
Calculate the mole fraction of HCl in 20 percent aqueous solution?
The mole fraction of HCl in a 20% aqueous solution can be calculated by converting the percentage to a molarity concentration. Assuming the density of the solution is 1 g/mL, a 20% solution means 20g of HCl in 100g of solution. If the molar mass of HCl is 36.5 g/mol, we can calculate the molarity and then use it to find the mole fraction of HCl in the solution.
What is the molarity of 32 percent HCl?
Ah, what a lovely question! To find the molarity of 32% HCl, you first need to know the density of the solution. Then you can use the formula: Molarity = (% concentration / molar mass) / density. Remember, it's all about taking your time and enjoying the process of solving this little mystery. Happy calculating!
Calculate the molarity of a hydrochloric acid solution that is 18.25 percent HCl by mass and has a density 1.2gmL?
First, calculate the mass of HCl in 100 g of the solution: 18.25% of 100 g is 18.25 g. Convert the volume to liters: 1.2 g/mL = 1.2 kg/L. Calculate molarity using the formula Molarity (M) = (moles of solute)/(volume of solution in liters), where moles of solute = mass of HCl in grams / molar mass of HCl and volume of solution = mass of solution in grams / density of solution in g/mL.
