Question

In: Chemistry

7. (8%) How to dispense one liter of 3 M HCl solution if you have a...

7. (8%) How to dispense one liter of 3 M HCl solution if you have a bottle of HCl that you find in the chemical stores? The bottle contains the following information: “37% w / w HCl (aq), density: 1.19 kg / L, molecular weight of HCl = 36.5 g / mol. ”

Solutions

Expert Solution

Given, density of concentrated solution = 1.19 kg/L = 1190 g/L  

37 % w/w means we have 36.5 g per 100 g of solution

molecular weight is given as 36.5 g/mol.

Concentration can be found out using the formula,

concentration(M) =purity x density x molecular weight

=> concentration(M) = (36.5 g/100 g solution) x 1190 g/L x ( 1 mol HCl/36.5 g)

=> concentration(M) = 11.9 mol/L = 11.9 M

This implies that the solution has the molarity of 11.9 M.

Now,

C1 = concentration of the concentrated solution (11.9 M)

V1= volume needed to prepare the diluted solution ( say X)

C2= concentration of the diluted solution (3M given )

V2= total volume of solution = 1 L = 1000 mL

Again,

C1V1 = C2V2

=>11.9 M * X = 3 M x 1000 mL

=> X = 252.1 mL

Hence, in order to prepare 1000 mL of a solution of HCl to 3M you have to take 252.1 mL of the concentrated solution and add 747.9 mL distilled water to make up the total volume to 1000 mL (1L).


Related Solutions

You have a one liter solution of kerosene containing 25 wt% propionic acid, add one liter...
You have a one liter solution of kerosene containing 25 wt% propionic acid, add one liter of water, mix thoroughly and allow the two phases to settle. At this temperature, the distribution coefficient for propionic acid is 0.175 mass fraction in kerosene/mass fraction in water. What is the expected composition (wt%) and mass (kg) of the two phases? You may need to acquire physical properties for some of your species.
Add 10 mL of 0.1 M HCl to one liter of a 0.10 M sodium acetate...
Add 10 mL of 0.1 M HCl to one liter of a 0.10 M sodium acetate buffer, pH 6.76 (pKa = 4.76 for acetic acid). Does the pH of the solution change? Determine the effect of the addition of 20.0 mL of 0.100 M HCl?
describe how to make one liter of the following solution: 0.3 M mannitol (FW=182), 0.02 M...
describe how to make one liter of the following solution: 0.3 M mannitol (FW=182), 0.02 M KPO4, 0.01 M KCl, 0.005 M MgCl2. You have the following stocks... 1 M KPO4, 1 M KCl, 1 M MgCl2.
1) An aqueous solution contains 0.34 M nitrous acid. One Liter of this solution could be...
1) An aqueous solution contains 0.34 M nitrous acid. One Liter of this solution could be converted into a buffer by the addition of: (Assume that the volume remains constant as each substance is added.) 0.17 mol HCl 0.35 mol HCl 0.35 mol KNO2 0.086 mol Ca(OH)2 0.34 mol KCl 2)   An aqueous solution contains 0.26 M ammonium chloride. One liter of this solution could be converted into a buffer by the addition of: (Assume that the volume remains constant...
An aqueous solution contains 0.30 M hydrocyanic acid. One Liter of this solution could be converted...
An aqueous solution contains 0.30 M hydrocyanic acid. One Liter of this solution could be converted into a buffer by the addition of which of the following reagents? (Assume that the volume remains constant as each substance is added.) Question 15 options:(more than one choice) 0.15 mol HClO4 0.30 mol KClO4 0.31 mol HClO4 0.31 mol KCN 0.149 mol NaOH
you have 1-5 ml of 0.140 M HCl solution and you want to dilute it to...
you have 1-5 ml of 0.140 M HCl solution and you want to dilute it to exactly 0.100 M. How much water should you add?
7. Calculate the volume of 1 M solution of HCl that we need to add to...
7. Calculate the volume of 1 M solution of HCl that we need to add to 100mL of 0.1 M of phosphate buffer (0.1 M H3PO4 and 0.1 M Na2HPO4) to get pH =4. Is it a buffer and why?
If you have 1 M Tris-HCl solution NaCl 100% Tween How would you make 500 mL...
If you have 1 M Tris-HCl solution NaCl 100% Tween How would you make 500 mL of 0.5 M NaCl, 0.1% Tween, and 100 mM Tris-HCl? i suck at buffer questions.... please help !!!
A solution of HCl is prepared by diluting 25.0 mL of a 1.0 M HCl solution...
A solution of HCl is prepared by diluting 25.0 mL of a 1.0 M HCl solution with enough water to make 750 mL of HCl solution. (Show your work for all calculations!) a) What is the molarity of the HCl solution? b) What is the [H3O+] and the pH of the HCl solution? c) Write the balanced chemical equation for the reaction of HCl and Ba(OH)2 d) How many milliliters of the diluted HCl solution is required to completely react...
Imagine you have two solutions, one that is 0.113 M in HCl and the other that...
Imagine you have two solutions, one that is 0.113 M in HCl and the other that is 0.085 M in Sr(OH)2. If you add 37.4 mL of the HCl solution to 31.8 mL of the Sr(OH)2 solution, which is the limiting reactant? How many grams of SrCl2 will be formed? How many moles of the excess reagent remain in solution?
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT