# How do you prepare a solution of 1 M HCl?

# How do one prepare a solution of 0.01M HCl?

Answer .
0.1M IS THE CONCENTRATION THAT SHOULD BE PREPARED,i.e. C2.WE SHOULD HAVE THE IDEAL VOLUME IN WHICH WE WANT TO PREPARE THE SOLUTION,SAY 2L, IS OUR V2.IF WE ARE TAKING THE HCL FROM A 12M Hcl,C1,THEN WE SHUOLD FIND OUR V1..
C1=12M V1=? C2=0.1M V2=2L.
C1V1=C2V2.
12M.V1=0.1M.2L.
V1=0.2M.L…/12M.
=0.016L.
=16.6ml.
ADD 16.6ml OF HCL IN A 2L VOLUMETRIC FLASK AND WITH SOME DISTILLED WATER.SWIRL TO MIX AND ADD DISTILLED WATER UP TO THE MARK OF THE VOLUMETRIC FLASK..
MALAPANE L.A.
For safety purposes you should always add acid to water, especially in the case of an acid like sulfuric acid. When mixing acid and water you should add some of the water to your flask, then add the acid and swirl to mix, then add the balance of the water. ( Full Answer )

# How to prepare HCL solution?

Prepare HCl 1 M by HCl concentration 37 %.
HCl concentration 37 % have density =1.19 g/ml.
HCl 1 M use HCl 37 % 82.81 ml make volume with water to 1 liter

# How do you prepare 0.1 Molar HCl solution?

To prepare a .1 M solution, the ratio would be .1 moles of HCl perliter of water. This is equal to 3.65 grams HCl.

# How do you prepare 0.1 N HCL solution?

molecular weight of HCL multiplied by N you are looking for (in this case 0.1) so, 0.1 x 36.46 = 3.646 gm (cc) of HCL to 1 Liter DI water

# How do you prepare 1 percentage hcl solution from 35 percentage hcl stock solution?

In order to prepare a 1 percent HCl solution, a specific ratio ofthe 35 percent solution must be added per liter. This ratio is 29.5milliliters of stock solution per liter of water.

# 1N HCl solution preparation?

To prepare 1N HCl take 8.33 ml of 12N HCl and make up to 100 ml

# How do you prepare 1n hcl solution?

The density of 36% HCl is not 1000 g/L. it is closer to 1.48 g/ml. 1000 g/L is the density of water. using 1.48 g/ml means 100 ml would contain 148 g solution = .36x148 g HCl = 53.3 g HCl = 53.3 g / (36.5 g/mole) = 1.46 moles. if you dilute that to 1L you get 1.46 N HCl not 1N... *************…************** this is the correct way to do this problem.... *************************** let's use a 1000 ml volumetric flask. This will make 1000 ml of a 1N solution of HCl and will require this many grams of HCl fyi. 1 N means 1 mole of equivalents per L solution and an equivalent is what we "chemists" and "chemical engineers" call an H+ ion or an OH- ion. HCl has 1 equivalent per molecule of HCl. H2SO4 has 2.... 1000 ml solution x (1 mole equivalents / 1000 ml) x (1 mole HCl / 1 mole equivalents ) x (36.5 g HCl / mole HCl ) = 36.5 grams HCl. that's what you need in the flask to make your 1 N solution. so how much of the 36% solution do you need? 36% by the way is based on mass. 36 g HCl / 100 g of solution.... so 36.5 g HCl x (100 g solution / 36 g HCl) = 101.39 grams solution. the answer is about 100 grams. not 100 ml.... at 1.48 g/ml, 100 g = 100g x (1 ml / 1.48g) = 67.6 ml..... *************** so make this solution this way *********** read the temp requirement on the volumetric flask. fill the flask 1/2 full of distilled water. SLOWLY add 101.39 grams of your 36% HCl solution to the flask (put the flask on a balance, zero the balance, add the acid to 101.39g with a pipette if you want) . swirl the flask for a minute or so. add more water to about 90% of the way to the volumetric mark. cool the flask to the temperature indicated on it (like 25C) then fill the rest of the way to the mark with distilled water. then stopper it with a glass stopper and invert it several times to mix.... Use the equation: MaVa=MbVb M= molarity V= volume ( Full Answer )

# How do you prepare HCL solution in Laboratory?

Hydrochloric acid is prepared by dissolving hydrogen chloride gas in water. Hydrogen chloride is a covalent compound, but when dissolved in water it ionizes to form hydrogen ions and chloride ions as follows:.
By.
Kuldeep K. bansal.
INDIA

# How many milliliters of water would you add to 100 ml of 1.0 m hcl to prepare a final solution of 0.25 m hcl?

400 mL. (100 mL)(1.0 M HCl)=(0.25 M HCl)v.
v is the volume that you are trying to find..
I believe the answer is 300 ml. as the question is "How much do you add . . .".
Total volume is 400 ml; so must add 300ml to the original 100 ml

# How do you prepare 0.1M HCL solution?

8.3ml HCl from 37% v/v stock bottle is required to prepare 0.1 M HCl solution.(answered by Prof.WASEEM UR RAHMAN KHAN)

# How do you prepare the 10N HCl solution?

weigh out 365g of HCl pellets and dilute to 1 liter to prepare the 10N HCl solution..
Reasons:N is short for NORMAL SOLUTIONS, .
The definition of a NORMAL SOLUTION is a solution that contains 1 gram equivalent weight (gEW) per liter solution. An equivalent weight is equal to the molecular weig…ht divided by the valence (replaceable H ions)..
egÃ¯Â¼Âš1N NaCl = 58.5 g/L.
1N HCl = 36.5 g/L.
1N H 2 S0 4 = 49 g/L.
Problems involving normality are worked the same as those involving molarity but the valence must be considered:.
1 N HCL the MW= 36.5 the EW = 36.5 and 1 N would be 36.5 g/L 1 N H 2 SO 4 the MW = 98 the EW = 49 and 1 N would be 49 g/L 1 N H 3 PO 4 the MW = 98 the EW = 32.7 and 1 N would be 32.7 g/L.
so,u can weigh out 365g of HCl pellets and dilute to 1 liter to prepare the 10N HCl solution. ( Full Answer )

# Prepare 500ml of 0.12N HCL solution?

add 5 ml of 37% HCl to 495 ml Water. This is 0.12 N ;)

# How do you prepare 1M FeCl2 solution in HCl?

Take Fecl2 as per your desired molarity and then add it to .1 molar HCL solution. keep it on magnatic sterier for over night. for better result perform the whole experiment under an oxygen free nitrogen atmosphere

# How to prepare 1N HCl solution?

1N HCl is also 1M HCl because it is mono-protic. Therefore 36.5 g of HCl is required per liter or 3.65%. Simply take 100 g of 37% HCl and make up to the 1 liter mark on the volumetric flask. Check the value by titration against 1M NaOH. It should be perfect. If very slightly strong dilute very sligh…tly (calculate) with water and re-standardize. ( Full Answer )

# How do you prepare 6M HCl solution?

To make 6M of an HCl solution, you must first make 12M and divide.Thus, 50 mL of 12M HCl will dilute to 100mL, and will create 6M.

# What volume of 10 M HCl and 3 M HCl should be mixed to get 1 L of 6 m HCl solution?

V1= x says V2 = 1000-x M1=10mol/L M2=3mol/L M = 6mol/L M = (M1V1+M2V2)/(V1+V2) 6={10*x+3(1000-x)}/(x+1000-x) 6000=7x+3000 x=428.57 V1= 428.57ml V2= 1000-428.57 V2= 571.2ml so, the volume of 10M HCl =428.57ml the volume of 3M HCl =571.2ml IT IS DONE BY JAGADEESH SAI … VINOD ( Full Answer )

# How do you prepare 0.1n HCl solution?

By dilution, but this depends totally on: .
How much litres you want to have. (suppose V 1 Litre) .
The concentration of the UNdiluted (more concentrated) HCl you have to start with. (suppose N 2 eq/L HCl) Then, with V 1 * N 1 = V 2 * N 2 , you can calculate V 2 , which is the amou…nt of undiluted HCl solution (also in Litre, as you've already chosen with units for V 1 ): V 2 = [V 1 * 0.1] / N 2 ( Full Answer )

# How do you prepare 5 percent HCl solution?

As it is in the form of liquid dilute it with water for eg.,to make 10 ml of 5% H CL Take 0.5 ml of H CL and add 9.5 ml of water. this is based on the calculation Volume percent is a common expression of a solution,s concentration It is defined as:

# How do you prepare a solution of 1 percent HCl?

2.23 ml of HCl in 100 ml gives 1% solution. 0.23 in 10 ml also gives 1% solution

# How can you prepare several different pH solutions from a 1 Molar stock solution of HCl?

dilute your HCl solution to 0.2 M HCl solution and then follow above mentioned link : http://delloyd.50megs.com/moreinfo/buffers2.html

# How can you prepare 0.05N HCl from 1N HCl solution?

3.6ml of HCl is diluted and make it into 500ml with distilled water. --------------------------------------------------------------------------------- Add 50 mL of HCl 1 N in a 1 L volumetric flask, class A or B; add ca. 900 mL distilled water to the flask. Place the flask in a thermostat at 20 0… C. After 30 min add slowly distilled water to the mark (1 L) and stir well the closed flask. Pour the solution in a bottle. Place a label with the date, concentration, name of the solution on the bottle. ( Full Answer )

# Preparation of 0.1N HCl solution from 37 percent HCl solution?

HCl 37% TO 0.1 N HCl (d=1.19) 250 ml OF H2O + 3.57 ml of HCl

# How do you prepare 30mL of 1 M NaOH solution?

In order to prepare exactly 30 mL of 1M NaOH solution, a volumetric vessel that contains exactly 30 mL when full to a marked level will be needed. By definition, a 1 M solution contains one mole in a liter of volume, and since solutions are homogeneous, 30 mL of such a solution will require (30/1000…) mole of sodium hydroxide. The molar mass of NaOH is about 40, corresponding to 1.2 grams of sodium hydroxide, which can be determined by weighing solid sodium hydroxide, dissolving the weighed amount in a volume of water less than the 30 mL capacity of the volumetric vessel, transferring this more concentrated solution into the volumetric vessel, and diluting with pure water until the 30 mL volume is contained in the vessel. ( Full Answer )

# How do you prepare 1 molar HCl from 6 molar HCl?

Take 100 mls. 6 molar solution and make it 600 mls. by adding distilled water

# How do you prepare HCL 2N solution?

HCL 2N solution is prepared by diluting it in a one to five ratio with water. It is not necessary to provide an outside force such as heat or pressure. Simple mixing with complete the dilution.

# How do you prepare a 1N HCl solution?

Density of HCl: 1.48 g/ml Molecular weight of HCl: 36.5g/mole Concentration of HCl stock: 36% Concentration of another HCl stock: 12N Final volume: 1L Let's assume that we're making a 1N HCl solution. Using the 36% concentration stock, we'll need to find out how many ml we would need. How…ever, HCl is interesting because it has a higher density than water. For a 1N solution (also known as 1M) however, you would need this amount of grams: (1M HCl) x (36.5 g/ mole HCl) x (1L) = 36.5 grams. Now we need the amount of ml from a 36% solution. This is different from having a known concentration like 10M, for example. 36% = 36 grams HCl / 100 grams of stock concentration solution (36.5 grams HCl) x (100gram of stock solution/ 36 grams HCl) x (1 ml/ 1.48 grams) = 68.5ml Dissolve 68.5ml of 36% solution into 931.5ml of ddH20. .
If your stock concentration came in 12M, then using the following equation: M = concentrations and V = volume. M 1 V 1 = M 2 V 2 V 1 = (M 2 V 2 )/M 1 Using the second equation, V 1 = volume of your stock concentration M1 = concentration of your stock V2 = volume of your final preparation M2 = concentration of your final V 1 = (1 M x 1L )/(12M) = 0.083 L = 83ml Dissolve 83 mL of 12M HCl into 917ml of ddH2O ( Full Answer )

# How can you prepare 0.25 M HCL from 35 percent HCL?

you are not mentioned the desired volume. for example you want to prepare 0.25 M HCl in 100 ml. To make a 0.25 M solution, slowly add 2.207 mL of your stock (HCl) solution to 25 mL deionized water. Adjust the final volume of solution to 100 mL with deionized water.

# How you prepare 0.25 Molar solution of HCl?

Look at the bottle of HCl. It gives a molarity. then dilute to 0.25 M.

# How is 0.1 m HCl from 3m HCl prepared?

Dilute the acid thirty times, take one ml solution of 3m HCl and make it 30 ml by adding distilled water,.

# How to prepare 0.2M HCl solution?

I assume you mean 0,2 M (0,2 mole/dm 3 ). Say we have a volume of 1 dm 3 , since you didn't specify that in your question. M HCl =35,5+1,01 g/mole = 36,51 g/mole n HCl =C/V n HCl =(0,2 moles/ dm 3 )/1 dm 3 = 0,2 moles m HCl =M/n m HCl =(36,51 g/ mole )/0,2 moles m H…Cl =182,55 gram. The reaction formula: H 2 (g)+ Cl 2 (g) --> 2 HCl (aq) Now that you know how that you get 2 moles of HCl by the reaction, then you need to calculate how much H 2 and Cl 2 you need for the reaction. Remember that the mass we get from this reaction is 2 moles x 182,55 g/ moles = 365,10 gram. That means we need to use a lot of gas when we lead it down in the specified volume of water to form a solution of HCl. Then only use half as much volume of this solution to get the desired concentration of 0,2 M HCl. It is easier if you have the salt HCl (s), then you only take 182,55 gram of the salt and solve it in a volume of destilled water that is not 1 dm 3 , but a little less, since the solution might change the density, thus exceeding 1 dm 3 . Then, when you have dissolved all the solid salt to ions in the solution, you can fill up to the specified volume of 1 dm 3. ( Full Answer )

# How to prepare 0.2N HCl solution?

0.2 N HCl solution means 0.2 equivalents of HCl dissolved in 1 litre of water. Normality = Molarity x n-factor => Molarity =Normality/n-factor=0.2/1=0.2 M 0.2 moles should be present in 1 litre of solution. 0.2moles =0.2 x 36.5 = 7.3 grams of HCl =>Dissolve 7.3 grams of HCl in 1 litre i…f water to get a 0.2N solution. ( Full Answer )

# How do you prepare 5M HCL solution?

To prepare a 5M HCl solution, you need to know the concentration ofyour source of HCl. Then you can use this proportion C1V1=C2V2,where C=Concentration in M(moles/liter) and V=Volume(liters).

# How do you prepare a solution of 1 M H2NO4?

It depends on how much you are trying to make and what you are diluting it from, but the formula for figuring it out is Molarity of starting solution times X (in which X is how much you will be adding) equals Molarity of the solution you are producing times its volume

# Where do you get the 82.81 ml during the preparation of 1 N solution of HCl from a concentrated 37 percent HCl?

Try a gradual measuring pipet max. 100 mL from which you'll get 83 ( + / - 1) mL. More accurate then this is not easily done and besides that it's also not usefull: the given concentrated 37% is also accurate between 36% - 38%, so you'll never get an exact 1.00 N HCl.

# How do you prepare 2M HCl solution from HCl?

There is 2 formula you need to know: M: n/V and n: m/Ma Ma: Molecular mass of HCI First step calculate the mol 2M: n/ 0.1 n: 0.2 n: m/Ma 0.2: m/ 36.5 m:7.3 Preparation: Get 7.3 ml of HCI pour it in the graduated cylinder (100ml) and add distilled water until it reaches 100ml. Thats all.

# How do you prepare a solution of 1 M HCL using 35 percent HCL?

From interpolation of table values: (between 34% and 36%) 35.0 %(m/m) HCl => Concentration 413 g HCl/L => density 1.174 kg/L => molarity 11.27 mol/L [ cf. link to in Related links on: Concentration table of concentrated HCl solutions] To prepare an 1.0 M HCl (= 1.0 Molar) solution …you take .
10.0 mL of the original 35%HCl and add up the volume to exactly 112.7 mL. Or you take .
100/11.42 mL, which is 8.87 mL , and add up to 100 mL ( Full Answer )

# What is the OH concentration of a 1 M HCL solution?

Water equilibrium equation: Kw = [H + ] * [OH - ] = 1.0*10 -14 (at 25 o C) So [OH - ] = 1.0*10 -14 / 1.0 M HCl = 1.0*10 -14 mol/L OH -

# How do you prepare 0.2N HCl solution from 1.0N HCl?

Add 200 mls of the 1.0N HCl solution to a 1 liter volumetric flask. Make up to the mark with water. Standardize against a known weight of Sodium Carbonate.

# How do you prepare 1 mM HCL using 1 M HCL?

Suppose your question is to prepare 1 mM HCl of 100 ml using 1 M HCl? Take equation V1N1 = V2N2 V1 is the volume of your 1mM HCl, here V1= 100 ml N1 is the your desired concentration of HCl. here N1= 1 mM V2 is the required volume (ml) of 1M HCl to prepare 100 ml of 1mM, here V2 N1 is th…e concentration of your available stock acid, here N1= 1M 1mM= 0.001 M Now, V2 = (100ml x 0.001)/1 = 0.1 ml Therefore, 0.1 ml of 1 M HCl with remaining 99.9 ml of distilled water addition will give 100 ml of 1mM HCl from 1M HCl stock. ( Full Answer )

# How do you prepare 1 M solution from 6 M solution?

It's simple to dilute a solution, just add more water. If you have one liter of 6 molar solution, and add another 5 liters of water, it becomes a 1 molar solution. .
You can also use M 1 V 1 = M 2 V 2 formula for dilution. For example, if you want to prepare 1 M of solution in 1 litre of wat…er, then how much volume you need from the initial 6 M solution? Simply use the equation, (6 M) x (V 1 ) = (1 M) x (1 litre) ---> V 1 = (1 M) x (1 litre)/(6 M) = 0.167 L or 167 ml ( Full Answer )

# How can 1 M of HCl be prepared from 32 percent HCl concentration?

You should also know the density of the 32 %(m/m) HCl. Maybe found answer in ' Related questions ': " How do you prepare a_solution of 1 M HCL using 35 percent HCL ", a link is just below this answer.

# How do you prepare a solution of 1 M butyric acid?

You'll need to know two things: what is the concentration of butyric acid you are starting with and how much 1 M butyric acid you want to end up with. From this, you can calculate how much water you need to add to a given volume of concentrated butyric acid to make 1 M butyric acid.

# How do you prepare 10 M HCL from 37 percent HCL?

37% HCl = { [ 37 (gHCl) / 100 (g sol'n) ] / 36.46 (gHCl/molHCl) } * 1,18 (g sol'n/mL sol'n) * 1000 (mL/L) = about 12 M HCl To prepare V Litres of 10M sol'n you should dilute [10*V]/12 Litre of 37% HCl solution to the total volume of V. Be very carefull with this addition of water.

# How do you prepare 0.05 molar hcl solution?

You will need to know the molarity of the solution you work from. Remember when working with acid - always put acid to the water, never vice versa. If you have a 1M solution you will need to put 20 times the amount of water. If you have a 5M solution you will need to 100 times the amount of wa…ter. It is more difficult if the basic solution is given in percentage. In this case you have to calculate how much HCl the solution contains. Eks:: A 37% HCl has a density of 1,19g/cm 3 and a molarity of 12,1 (12,1M). so the amount of water will be 242 times more to get the specified solution. Be very careful if you are working with this stuff - you could get injuries on you skin, eyes and lounges. ( Full Answer )

# How do you prepare a solution of 100 ml of 1 mol HCl from 3 mol HCl?

C 1 V 1 =C 2 V 2 This is the equation you need to prepare your solution. In order to see how much of solution 1, in your case 3M HCl, you need solve for V 1 . So Divide (1MHCl x 100mL) by 3M HCl. Or (1M)(100mL)/(3M) = 33.33mL

# What is theoretical pH value for 1 m hcl solution?

It doesn't matter how much you have, HCl (Hydrochloric Acid) has a pH of 1

# How do you prepare 0.02 M of HCl?

0.02M=20mM(multiply x1000) From a 1M stock HCL I shall prepare 100ml of 20mM HCl by the following equation V1N1=V2N2 100mlx20mM=1000mMx"V2" V2=100x20/1000 =2ml. So add 2ml of 1M stock HCl plus 98ml of water to make 100ml of 0.02M HCL; this formula applies for any amount/concentration of …solution. Hope this help you. ( Full Answer )

# How you prepare 1 M KCl solution?

\n.
Dissolve 74.55g of KCL in some water then volume it up to 1 liter.

# What is the OH 1 in a 0.0001 M solution of HCl?

From the equilibrium of water dissociation, kW is equal to the product of hydrogen ions and hydroxyl ions. The hydrogen ion concentration is 1x10^(-4). Hence, at 298 K, the hydroxyl ion concentration would be 1x10^(-10).

# How would you prepare 17.2 L of a 3.8 M HCl solution?

First get moles HCl, then get the grams HCl. Molarity = moles of solute/Liters of solution 3.8 M HCl = X moles/17.2 Liters = 65.36 moles HCl ===so, 65.36 moles HCl (36.458 grams/1 mole HCl) = 2382.89 grams HCl ==and, put this amount, 2382.89 grams, 65.36 moles HCl into the 1…7.2 liters of solution ( water, I suppose ) 2382.89 grams = 2.38 kilograms. I suppose you could weigh out the HCl in a flask of some sort. ( Full Answer )